Topic outline

  • General

  • UNIT 1: PROPERTIES AND USES OF TRANSITION METALS

     Key Unit Competence:

    The learner should be able to explain the properties and uses of transition metals.
    Learning objectives
    At the end of this unit , students will be able to:
    • Discuss qualitatively the propertie of transition elements;
    • Explain the principle of ligan exchange;
    • State the rules of naming complex ions and stereoisomers;
    • Describe reactions of transition metals;
    • State the use of transition metals;
    • Relate the electronic configurations to special properties of transition metals;
    • Predict the shape of the complex compounds of transition metal cations;
    • Perform the confirmatory tests for transition metal ions.

    Most of the metals in the periodic table belong in the d-block of transition metals. They are hard and strong, and many of them are very familiar to us. For instance, zinc Chemistry Senior Six Student Book 3 is in brass instruments like trumpets and tubas. Have you ever heard of the element “scandium” before? But you’ve interacted with it if you have ever ridden a bicycle.
    1.1. Definition and electronic configuration of transition metals.

    According to IUPAC system, a transition metal is “an element whose atom has a partially filled d sub-shell, or which can give rise to cations with an incompleted-orbitrals”. Transition metals are located between groups 1& 2 (s-block) and group 13 (p-block) on the periodic table. The elements are also called d-block elements because their valence electrons are in d-orbitals.

    The properties of transition elements are between the highly reactive metallic elements of the s-block which generally form ionic compounds and the less reactive elements of the p-block which form covalent compounds. Transition metals form ionic compounds as well as covalent compounds.
    The first 3 rows, i.e. period 4, period 5 and period 6, are called first transition series, second transition series and third transition series respectively. The metals of the first series are all hard and dense, good conductors of heat and electricity.
    This block is known as the transition metals because some of their properties show a gradual change between the active metals in s-block and p-block where non-metals are found. Electronic configuration is the arrangement of electrons in orbitals around the nucleus. The electronic structure of the first transition series is shown in the table below:

    When building electronic structure of transition metals, 4s orbital is filled before 3d orbitals. The transition elements are stable when their d-orbitals are filled (d10) or when theird-orbitals are half filled (d5).This explains the electronic structure of copper, [Ar] 4s13d10 instead of [Ar] 4s23d9. The same applies for Cr: [Ar] 4s13d5 and not [Ar] 4s23d4.
    In order to attain that stability an electron can jump from 4s orbital to 3d orbital because those two orbitals are close in energy.
    This also explains why Fe2+ with 3d6 is easily oxidized to Fe3+ with 3d5 and Mn2+ with 3d5 is resistant to oxidation to Mn3+ with 3d4. Transition metals form ions by losing electrons first from the 4s sub-shell rather than the 3d sub-shell. Hence electronic configuration of Fe, Fe2+ and Fe3+ are the following:

    The 4s electrons are removed before 3d electrons. This is because the 3d electrons are inner while the 4s electrons are outer therefore the outer electrons (4s) have to be removed before the inner electrons.

    1.2. Properties of the transition metals
    1.2.1. Melting and boiling points

    The melting points and the molar enthalpies of fusion of the transition metals are both high in comparison to main group elements. Most of the transition metals have melting points above 1000 oC; mercury is liquid at room temperature.
    This is due to the high number of valence electrons that increases the electrostatic attraction force between those electrons and the metallic cations, hence increasing the strength of the metallic bond and the melting point.

    1.2.2. Densities and atomic/metallic radii

    The transition elements are much denser than the s-block elements and show in general a gradual increase in density from left to right in a period as you can see  below from scandium to copper. This trend in density can be explained by a decrease in metallic radii coupled with the relative increase in atomic mass

    1.2.3. Ionization energies

    The ionization energy of transition metals is related to the energies of its d orbitals, its ease of oxidation, and its basicity.In simplest terms, the greater the ionization energy of a metal, the harder it is to pull an electron from it.
    As the number of protons increases across a period (or row) from left to right of the periodic table, the first ionization energies of the transition-metal elements are relatively the same, while that for the main-group elements increases. In moving across the series of metals from scandium to zinc, a small change in the values of the first and second ionization energies is observed. This is due to the buildup of electrons in the immediately underlying d-sub-shells that efficiently shields the 4s electrons from the nucleus and minimizing the increase in effective nuclear charge from element to element.


    In general, ionization energy increases as we move from left to right across theperiod. Notable dips occur at row 1, group 10 (Ni) and row 3, group 7 (Re).

    Oxidation state is a number assigned to an element in chemical combination which represents the number of electrons lost or gained.The transition elements from Titanium to Copper all form ions with two or more oxidation states. In most cases, this is the result of losing the two electrons of 4s orbital and electeons in 3d orbitals. The 4s electrons are lost first because they are in the highest energy level. However, because the 3d and 4s energy level are so close in energy, the 3d electrons can also be lost when an atom forms a stable ion. The common oxidation states shown by the first transition series are:
    1. The common stable oxidation states for those transition metals with variableoxidation states are bolded and underlined.
    1. The oxidation state corresponding to a full or half-filled d-orbital is energetically stable. For example, Fe3+ is more stable than Fe2+and Mn2+ is more stable than Mn3+.
    1. However, in most compounds and solutions, copper exist as Cu2+ ion rather than Cu+ ion. Meaning that the former is more stable than the latter. The explanation of this is beyond this level.
    1.2.5. Most transition metals and their compounds have high ability of being catalyst

    A catalyst is a substance that can speed up (positive catalyst) or that can slow down (negative catalyst) the rate of reaction and is found unchanged at the end of the reaction. But generally the term catalyst is used for the substance that helps in accelerating the rate of the reaction. A catalyst that speeds up the reaction provides another pathway with lower activation energy.
    In some catalytic process, transition metal ions undergo changes in their oxidation states but are regenerated at the end of the reaction.
    The reasons for transition metals to work as catalysts:
    • Presence of empty d orbitals which enable transition metal ions (or atoms) to form temporary bonds with reactant molecules at the surface of a catalyst and weakens the bond in the reactant molecules
    . Variable oxidation states which allow them to work as catalysts in the reactions involving the transfer of electrons
    Table 1.6: Reactions catalysed by transition metals


    1.2.6. Most transition metal ions are paramagnetic

    Paramagnetism is a property of substances to be attracted in a magnetic field. Substances which are not attracted (i.e slightly repelled) in a magnetic field are said to be diamagnetic.Transition metal ions show paramagnetism because of the presence of unpaired electrons in their 3d arbitrals.
    The greater the number of unpaired electrons, the stronger the paramagnetism; that is the reason why:
    1. Fe3+ is more paramagnetic than Fe2+ because Fe3+ has five unpaired electrons while Fe2+ has four unpaired.
    1. Sc3+ and Zn2+ are not paramagnetic, they are diamagnetic because they do not have unpaired electrons
    Other examples of paramagnetic substances are: Cr, Mn, CuSO4, Fe, Co, Ni, Pt. Examples of diamagnetic substances are: Zn, Cu+, Au+, TiO2.

    1.2.7. Formation of alloys

    An alloy is a homogenious solid mixture (solid solution) made by combining two or more elements where at least one is a metal.
    Importance of alloying:
    • Increase of the strength of a metal,
    • Resistance to corrosion,
    •  Gives to the metal a good appearance
    Generally, alloys are needed and used to improve the quality of the required material. For example, brass (alloy of zinc and copper) is much stronger than eitherpure copper or pure zinc. Pure gold is too soft to be used in some applications.
    Table 1.7: The properties and uses of some common alloys formed by transition metals (first series)




    1.2.8. Formation of complex ions

    A complex or coordination compound is a chemical species made of a central metal (cation or neutral) bonded to other chemical species called ligands by coordination or dative bonds. A complex may be neutral, positively or negatively charged.
    Transition metal form complexes because of:
    1. Their small and highly charged ions,
    1. The presence of vacant (empty) d-orbitals which can accommodate lone pair of electrons donated by other groups (ligands)
    The general formula of a complex is: [MLn]y
    Where:
    1.  M-metal ion or atom
    1.  L-Ligand
    1. n-the number of ligands surrounding the metal 
    1. y-the charge of the complex; [MLn] indicates a neutral complex
    - Coordination number of a complex: is the number of coordinate bonds on the central metal in a complex.
    - Ligand: It is a species (anion or a molecule) that is bonded to a central metal ion or atom in a complex. A ligand should have at least one lone pair of electrons to form a coordinate bond.
    Ligands are classified depending on the number of sites at which one molecule of a ligand is coordinated to the central metallic atom; the ligands are classified as monodentate (or unidentate), ambidentate and polydentate (or multidentate) lingards.
    a. Monodentate ligands
    The ligands which have only one donor atom or are coordinated through one electron pair are called monodentate ligands because they have only one tooth with which to attach themselves to the central cation or atom. Such ligands are coordinated to the central metal at one site or by one metal-ligand bond only. These ligands may be neutral molecules or in anionic form.

    Notice that a ligand with a donor atom that possesses 2 lone pairs of electrons, such as H2Ö:, is not bidentate, since it cannot use both lone pairs simultaneously to bind to the metal because of the steric effect.
     b. Polydentate ligands


    These may be bidentate, tridentate, tetradentate, pentadentate, and hexadentateligands if the number of donor atoms present in one molecule of the ligand attached with the central metallic atom is 2, 3, 4, 5, and 6 respectively. Thus one molecule of these ligands is coordinated to the central metallic atom at 2, 3, 4, 5, and 6 sites respectively. In other words, we can say that one molecule of these ligands makes 2, 3, 4, 5, and 6 metal-ligand coordinate bonds respectively.



    • Hexadentate

    The structure shows that it has two neutral N- atoms and four negatively charged Oatoms as its donor atoms which can form coordinate bonds with a transition metal ion.


    The complex ions which form between polydentate ligands and cations are known as chelates or chelated complexes.

    In general, polydentate ligands form more stable complexes than monodentate ligands. The stability of complex is much enhanced by chelation. A polydentate ligand can hold the central cation more strongly.


    Geometry of complexes

    Complexes have a variety of geometries or shapes, but the most common geometries are the following:

    • Complexes with coordination number 2 adopt a linear shape. Example:

    [Ag(NH3]2 +: [H3N-Ag-NH3]+

    The complexes having coordination number of 2 are linear since minimises ligand repulsion.


    • Complexes with coordination number 4 generall adopt a tetrahedral shape. But few of them can form a square planar shape.

    The square plannar geometry is characteristic of transition metal ions with eight d electrons in the valence shell, such as platinum(II)and gold(III).


    Copper (II) and cobalt (II) ions have four chloride ions bonded to them rather than six, because the chloride ions are too big to fit any more around the central metal ion.


    • Complexes with coordination number 6 adopt an octahedral shape. Example:[Cr(NH3)6]3+.

    These ions have four of the ligands in one plane, with the fifth one above the plane, and the sixth one below the plane.



    1.2.9. Many transition metal ions and their compounds are coloured



    The formation of colored ions by transition elements is associated with the presence of incompletely filled 3d orbitals.



    This property has its origin in the excitation of d electrons from lower energy d-orbitals to higher energy. In fact, when the central metal is surrounded by ligands, these cause d orbitals to be split into groups of higher and lower energy orbitals. When electrons fill d-orbitals, they fill first of all the lower energy orbitals; if there is free space in higher energy d-orbitals, an electron can be excited from lower energy d-orbitals to higher energy d-orbitals by absorbing a portion of light corresponding to a given colour, the remaining color light is the white light minus the absorbed colour.


    When a coloured object is hit by white light, the object absorbs some colour and the colour transmitted or reflected by the object is the colour which has not been absorbed. The observed colour is called complementary colour.

    When a metal cation has full d-orbitals, such as Cu+or Zn2+ or no electron in d orbital, such as Sc3+.

    Table1.9: Complementarities of colors observed and absorbed when light is emitted



    The colour of a particular transition metal ion depends upon two factors:

    • The nature of the ligand


    The principle of ligand exchange

    Complexing reactions involve competitions between different ligands for central metal. A more powerful ligand displaces a less powerful ligand from a complex. During the process there is a change in colour.

    Here below is a list of some ligands in increasing order of strength.


    The above series are called the spectrochemical series and shows that cynide ion and carbon monoxide are very strong ligands

    The stability of a complex ion is measured by its stability constant. The higher the stability constant of a complex, the more stable is the complex.


    1.3. The anomalous properties of Zinc and Scandium


    On the basis of the properties of transition metals, zinc and scandium are not considered as typical transition metals even though they are members of the d-block.

    Zinc:

    • It has a complete d-orbital.
    • Zinc forms only the colourless Zn2+ ion, isoelectronic with the Ga3+ion, with 10 electrons in the 3d subshell.
    • Zinc and its compounds are not paramagnetic

    Scandium:

    • Has one oxidation state,+3
    •  Sc forms only the colourless Sc3+ion, isoelectronic with the Ca2+ ion, with no electrons in the 3d subshell.
    • Its compounds are diamagnetic
    • It forms compounds containing ions with a completely empty 3d subshell.


    1.4. Naming of complex ions and isomerism in of transition metal complexes 

    1.4.1. Naming of complex ions


    Naming molecules requires the knowledge of certain rules, such as how to name cations, anions, where to start from when both a cation and an anion are combined in an ionic molecule or when two non metals are combined in a covalent molecule.

    Like other compounds, complex compounds/ions are named by following a set of rules. You are familiar with some of them and the new ones can be understood and applied easily.

    1. In simple metal compounds, the metal is named first then the anion.

    Example: CaCl2: calcium chloride

    2. In naming the complex:

    • Name the ligands first, in alphabetical order, then the metal atom or cation, followed by its oxidation state written between brackets as Roman number, though the metal atom or cation is written before the ligands in the chemical formula.

    Example: [CuBr4]2-: Tetrabromocuprate (II) ion

    The names of some common ligands are listed in the table below:

    Table 1.10: Names of common ligands


    • Greek prefixes are used to indicate the number of each type of ligand in the complex:

    The numerical greek prefixes are listed in the following table:

    Table 1.11: Greek numerical prefixes


    • After naming the ligands, name the central metal.

    - If the complex bears a positive charge (cationic complex), the metal is named by its usual name.

    Example: Cu: Copper               Pt: Platinum

    - If the complex bears a negative charge (anionic complex), the name of the metal ends with the suffix –ate

    Example: Co in a complex anion is called cobaltate and Pt is called platinate.

    For some metals, the Latin names are used in the complex anions e.g. Fe is called ferrate (not ironate). See table below:

    Table 1.12: Latin names of some transition metals in anionic complexes


    1. For historic reasons, some coordination compounds are called by their common names.

    Example: Fe(CN)6 3- and Fe(CN)6 4- are named ferricyanide and ferrocyanide respectively, and Fe(CO)5 is called iron carbonyl.

    2. To name a neutral complex molecule, follow the rules of naming a complex cation

          Example: [Cr(NH3)3Cl3]: triamminetrichlorochromium (III)

    You can have a compound where both the cation and the anion are complex ions. Notice how the name of the metal differs even though they are the same metal ions. Remember: Name the cation before the anion.

    Example: [Ag(NH3)2][Ag(CN)2] is diamminesilver(I)dicyanoargentate(I)

    Note that:

    • The names are written as a one word: Tetraamminecopper (II), not Tetraammine copper (II).
    •  Complex ions formula is written between square brackets and the charge of the ion as superscript outside the brackets: [Cu(NH3)4]2+. When oppositely chargedions approach the complex ion, a neutral molecule can be obtained:

    [Cu(NH3)4]2+2Cl- or simply, [Cu(NH3)4]Cl2: tetraamminecopper(II)chloride.

    The ions outside the square brackets are known as “counter ions”.



    1.4.2. Isomerism in complexes


    Isomers are chemical species that have the same molecular formulal, but different molecular structures or different arrangements of atoms or groups of atoms in space. Isomerism among transition metal complexes arises as a result of different arrangements of their constituent ligands around the metal.

    The diagram below shows the different categories of isomerism in transition metal complexes.


    In this unit, we are specifically concerned with ‘stereoisomerism’ which gives rise to isomers known as “stereoisomers”. Stereoisomers have the same structural formulal but different arrangements of ligands in space.

    They are classified in two categories: geometrical isomers and optical isomers.

    1. Geometrical isomers

    Coordination complexes, with two different ligands in the cis and trans positions from a ligand of interest, form isomers.

    For example, the square planar, diammine dichloroplatinum (II) Pt(NH3)2Cl2),can be presented as follows:


    Different geometrical isomers are different chemical compounds. They exhibit different properties, even though they have the same formula. For example, the two isomers of [Co(NH3)4Cl2]NO3 differ in color; the cis form is violet, and the trans form is green. Furthermore, these isomers have different dipole moments, solubilities and reactivities.

    2. Optical isomers (enantiomers)

    example of this is your two hands (left and right); hold them face-to-face: one is the mirror image of the other. Now try to superimpose them one over another: they are non superimposable (only the middle fingers superimpose one over the other. Chemical compounds that behave like the hands are called “chiral”, in reference to the Greek word for hands.

    Optical isomers are very important in organic and biochemistry because living systems often incorporate one specific optical isomer and not the other.

    Unlike geometric isomers, optical isomers have identical physical properties (boiling point, polarity, solubility, etc.). Optical isomers differ only in the way they affect polarized light and how they react with other optical isomers.

    For coordination complexes, many coordination compounds such as [M(en)3]n+ [in which Mn+ is a central metal ion such as iron(III) or cobalt(II)] form enantiomers, as shown in figure below.These two isomers will react differently with other optical isomers. For example, DNA helices are optical isomers, and the form that occurs in nature (right-handed DNA) will bind to only one isomer of [M(en)3]n+ and not the other.




    1.5. The Chemistry of individual transition metals


    1.5.1. Scandium


    2. Uses

    • Scandium has as low density (2.99 g/cm3) asaluminium (2.7 g/cm3) but a much higher melting point.
    • An aluminium-scandium alloy has been used in fighter planes, high-end bicycle frames and baseball bats.
    • Scandium iodide is added to mercury vapour lamps to produce a highly efficient light source resembling sunlight. These lamps help TV cameras to reproduce colour well when filming indoors or at night-time.

    1.5.2. Titanium



    2. Uses

    • Titanium is as strong as steel but much less dense. It is therefore important as an alloying agent with many metals including aluminium, molybdenum and iron. These alloys are mainly used in aircraft, spacecraft and missiles because of their low density and ability to withstand extremes of temperature. They are also used in golf clubs, laptops, bicycles and crutches.
    • Power plant condensers use titanium pipes because of their resistance to corrosion. Because titanium has excellent resistance to corrosion in seawater, it is used in desalination plants and to protect the hulls of ships, submarines and other structures exposed to seawater.
    • Titanium metal connects well with bone, so it has found surgical applications such as in joint replacements (especially hip joints) and tooth implants.
    • The largest use of titanium is in the form of titanium (IV) oxide. It is extensively used as a pigment in house paint, artists’ paint, plastics, enamels and paper. It is a bright white pigment with excellent covering power. It is also a good reflector of infrared radiation and so is used in solar observatories where heat causes poor visibility.

    1.5.3. Vanadium

    Vanadium is a grey, solid with a density of about 6.11. It melts at 1915 oC and boils at 3350 oC. It is insoluble in water at room temperature.

    2. Uses

    • About 80% of the vanadium produced is used as a steel additive. Vanadium- steel alloys are very tough and are used for spanners, armour plate, axles, piston rods and crankshafts. Less than 1% of vanadium, and as little chromium, makes steel shock resistant and vibration resistant. Vanadium alloys are used in nuclear reactors because of vanadium’s low neutron-absorbing properties.
    • Vanadium (V) oxide is used as a pigment for ceramics and glass, as a catalyst and in producing superconducting magnets.

    1.5.4. Chromium

    Chromium is a silver gray metal with density of about 7.14. It melts at 1900 oC and boils at 2690 oC. Chromium is insoluble in water at room temperature.



    2. Uses

    • Chromium is used to harden steel, to manufacture stainless steel (resists to corrosion) and to produce several alloys.
    • Chromium plating can be used to give a polished mirror finish to steel. Chromium-plated car and lorry parts, such as bumpers, were once very common. It is also possible to chromium plate plastics, which are often used in bathroom fittings.
    • About 90% of all leather is tanned using chromium. However, the waste effluent is toxic so alternatives are being investigated.
    • Chromium compounds are used as industrial catalysts and pigments (in bright green, yellow, red and orange colours). Rubies get their red colour from chromium, and glass treated with chromium has an emerald green colour.
    • Chromium (IV) oxide is used in magnetic tapes for sound/video recording.
    • Chromium is used in the control of cholesterol and help insulin sugar control in blood.

    1.5.5. Manganese

    Manganese is a grey-white solid with a slightly red colour. Its density is about 7.44 oC. Manganese melts at 1244 oC and boils at 2060 oC. It is insoluble in water but soluble in diluted acids, at room temperature.


    2. Uses

    • Manganese is too brittle to be of much use as a pure metal. It is mainly used in alloys, such as steel. Steel contains about 1% manganese, to increase the strength and also improve workability and resistance to wear. Manganese steel contains about 13% manganese. This is extremely strong and is used for railway tracks, safes, rifle barrels and prison bars.
    • Drinks cans are made of an alloy of aluminium with 1.5% manganese, to improve resistance to corrosion. With aluminium, antimony and copper it forms highly magnetic alloys.
    • Manganese (IV) oxide is used as a catalyst, a rubber additive and to decolourise glass that is coloured green by iron impurities. Manganese (IV) oxide is a powerful oxidising agent and is used in quantitative analysis. It is also used to make Fertilizers and ceramics.
    • Manganese sulphate is used to make a fungicide.

    1.5.6. Iron

    Iron is a grey to black, odourless metal with density 7.874. It melts at 1535 oC and boils at 2750 oC.



    2. Uses

    • Iron is an enigma – it rusts easily, yet it is the most important of all metals. 90% of all metal that is refined today is iron. Most is used to manufacture steel, used in civil engineering (reinforced concrete, girders etc) and in manufacturing.
    • Alloy steels are carbon steels with other additives such as nickel, chromium, vanadium, tungsten and manganese. These are stronger and tougher than carbon steels and have a huge variety of applications including bridges, electricity pylons, bicycle chains, cutting tools and rifle barrels.
    • Stainless steel is very resistant to corrosion. It contains at least 10.5% chromium. Other metals such as nickel, molybdenum, titanium and copper are added to enhance its strength and workability. It is used in architecture, bearings, cutlery, surgical instruments and jewellery.
    • Cast iron contains 3–5% carbon. It is used for pipes, valves and pumps. It is not as tough as steel but it is cheaper.
    • Magnets can be made of iron and its alloys and compounds.
    • Iron catalysts are used in the Haber process for producing ammonia, and in the Fischer–Tropsch process for converting syngas (hydrogen and carbon monoxide) into liquid fuels.
    • Iron plays an important role in the transfer of oxygen by hemoglobin. Each hemoglobin binds four iron atoms. Iron in hemoglobin binds with oxygen as it passes through the blood vessels in the lungs and releases it in the tissues.

    1.5.7. Cobalt

    Cobalt is a dark grey metal with a density of 8.90. It is insoluble in water at room temperature.



    2. Uses

    • Cobalt, like iron, can be magnetized and so is used to make magnets. It is alloyed with aluminium and nickel to make particularly powerful magnets.
    • Other alloys of cobalt are used in jet turbines and gas turbine generators at high temperature.
    • Cobalt metal is sometimes used in electroplating because of its attractive appearance, hardness and resistance to corrosion.
    • Cobalt salts have been used for centuries to produce brilliant blue colours in paint, porcelain, glass, pottery and enamels.
    • Cobalt is an essential trace element and found at the centre of the vitamin B12 (cobalmin, C63H88CoN14O14P). It contains a cobalt(III) ion and is necessary for the prevention of pernicious anaemia and the formation of red blood corpuscles, but it is involved many other functions too.

    1.5.8. Nickel

    Nickel is a grey solid metal with density of about 8.9. It melts at 1455 oC and boils at 2920 oC.

    1. Chemical reactions

    a. Reaction of nickel with air

    Nickel does not react with oxygen, O2, at room temperature, under normal conditions. Finely divided nickel can burn in oxygen, forming nickel (II) oxide, NiO.



    2. Uses

    • Nickel resists corrosion and is used to plate other metals to protect them. It is, however, mainly used in making alloys such as stainless steel. Nichrome is an alloy of nickel and chromium with small amounts of silicon, manganese and iron. It resists corrosion, even when red hot, so is used in toasters and electric ovens. A copper-nickel alloy is commonly used in desalination plants, which convert seawater into fresh water. Nickel steel is used for armour plating. Other alloys of nickel are used in boat propeller shafts and turbine blades.
    • Nickel is used in batteries, including rechargeable nickel-cadmium batteries and nickel-metal hydride batteries used in hybrid vehicles.
    • Nickel has a long history of being used in coins. The US five-cent piece (known as a ‘nickel’) is 25% nickel and 75% copper.
    • Finely divided nickel is used as a catalyst for hydrogenating vegetable oils. Adding nickel to glass gives it a green colour.

    1.5.9. Copper

    Copper is a light pink to red (shiny-reddish) metal of density 8.95 g/cm3. It melts at 1083 oC and boils at 2570 oC.



    2. Uses

    • Historically, copper was the first metal to be worked by people. The discovery that it could be hardened with a little tin to form the alloy bronze gave the name to the Bronze Age.
    • Traditionally it has been one of the metals used to make coins, along with silver and gold. However, it is the most common of the three and therefore the least valued. All US coins are now copper alloys, and gun metals also contain copper.
    • Most copper is used in electrical equipment such as wiring and motors. This is because it conducts both heat and electricity very well, and can be drawn into wires. It also has uses in construction (for example roofing and plumbing), and industrial machinery (such as heat exchangers).
    • Copper sulphate is used widely as an agricultural poison and as an algaecide in water purification.
    • Copper compounds, such as Fehling’s solution, are used in chemical tests for sugar detection.
    • Copper helps in storing iron, is involved in production of pigments for colouring hair, skin and eyes.

    1.5.10. Zinc

    Zinc is a grey solid with a density of 7.14 g/cm3. It melts at 419.5 oC and boils at 907 oC.



    2. Uses

    • Mostly, zinc is used to galvanise other metals, such as ironsheets (amabati), to prevent corrosion. Galvanised steel is used for car bodies, street lamp posts, safety barriers and suspension bridges.Many houses in Rwanda are covered by galvanized iron sheets (amabati).
    • Large quantities of zinc are used to produce die-castings, which are important in the automobile, electrical and hardware industries.
    • Zinc is also used in alloys such as brass, nickel silver and aluminium solder.
    • Zinc oxide is widely used in the manufacture of many products such as paints, rubber, cosmetics, pharmaceuticals, plastics, inks, soaps, batteries, textiles and electrical equipment. Zinc sulphide is used in making luminous paints, fluorescent lights and x-ray screens.
    • It is a component of insulin.



    1.6. Identification of transition metal ions



    Different transition metals have different colors. Also, different charges, or cations of one transition metal can give different colors. Another factor is the natural of the ligand. The same cations of a transition metal can produce a different color depending on the ligand it binds to.

    Many compounds containing transition metals have certain characteristic colours and thus, by observing a compound, we can not identify it.

    • Appearance or colour of different solid compounds containing transition metals

    Table 1.13: Colours of different solid compounds containing transition metals (first series)




    • Colours of aqueous solutions of some transition metal ions

    In aqueous solutions where water molecules are the ligands, the colours of some metal ions observed are listed in the table below:

    Table 1.14: Colours of different aqueous solutions containing some transition metals (first series)


    • Action of heat on solid compounds containing transition metal ions

    Table 1.15: Colours of different solid compounds containing transition metals (first series) due to action of heat.


    Note: On heating the following temporary colour changes may also occur:

    Effect of aqueous sodium hydroxide and aqueous ammonia on solutions containing transition metal ions

    The hydroxides of transition metals are precipitated from solutions of the metal ions by the addition of hydroxide ions or ammonia. The colour of the precipitate can often be used to identify the metal present. The precipitates formed are gelatinous and often coloured and some form soluble complex ions with excess ammonia.

    a. To about 1cm3 of the solution containing the positive ion (cation), add 2M aqueous sodium hydroxide dropwise until in excess



    b. To about 1cm3 of the solution containing the positive ion (cation), add 2M aqueous ammonia dropwise until in excess




    • Confirmatory tests for some transition metal ions

    Confirmatory tests are the tests required to confirm the analysis. Generally, a confirmatory test is used after other tests have been carried out to isolate/identify   the ion. In order to confirm the ion without any dought.

    1. Zinc ions

    i. Addition of little solid ammonium chloride followed by disodium hydrogen phosphate solution to a solution of zinc ions gives a white precipitate. The precipitate dissolves in excess ammonia or dilute mineral acids

    ii. Addition of potassium ferrocyanide solution to a solution of zinc ions gives a white precipitate.

    Zn2+(aq) + [Zn(CN)6] - (aq) Zn2[Fe(CN)6](s)

    2.Chromium ions

    To a solution of chromium (III) ions, add excess aqueous sodium hydroxide followed by little hydrogen peroxide and boil the resultant mixture. A yellow solution of a chromate is formed. 

    2Cr3+(aq) + 10OH-(aq) + 3H2 O2 (aq) → 2CrO4 2-(aq) + 8H2 O(l)

    Treatment of the yellow solution with:

    i. Lead (II) ethanoate or Lead(II)nitrate solution gives a yellow precipitate of Lead(II) chromate. Pb2+(aq) + CrO4 2-(aq) →PbCrO4(s)

    ii. Barium nitrate (or chloride) solution gives a yellow precipitate of barium chromate.


    iii. Silver nitrate gives a brick red precipitate of silver chromate


    iv. A little alcohol (for example, butan-1-ol) and dilute sulphuric acid , a blue color is formed in the alcohol layer. The blue color is due to unstable CrO5

    c. Manganese (II) ions

    To the solution of manganese (II) ions, add little concentrated nitric acid followed by little solid lead(IV) oxide or solid sodium bismuthate(V) and boil the mixture. A purple solution is formed due to MnO4 - ion


    d. Iron (II) ions

    i. Addition of potassium hexacyanoferrate (III) solution to a solution of iron (II) ions gives a dark blue precipitate .

    ii. Addition of potassium thiocyanate or ammonium thiocyanate solution to a solution of iron (III) ions gives a blood red coloration.

    f. Cobalt (II) ions

    Addition of potassium thiocyanate or ammonium thiocyanate solution to a solution of cobalt(II) ions gives a blue colored product of potassium cobalt(II) tetrathiocyanate.


    g. Nickel (II) ions

    i. Addition of potassium cyanide solution gives a yellow-green precipitate of Nickel(II) cyanide. The precipitate dissolves in excess reagent to form a dark yellow solution tetracyanonickel (II) ion.


    ii. Addition of aqueous ammonia followed by 2 to 3 drops of dimethylglyoxime solution to a solution of nickel (II) ions gives a red precipitate. The formation of this precipitate may sometimes require that the solution mixture would be warmed.

    h. Copper (II) ions

    In addition to use of aqueous ammonia, the copper(II) ions can be confirmed by addition of the following reagents to an aqueous solution of copper(II) ions:

    i. Potassium iodide solution: A white precipitate of copper (I) iodide stained brown with free iodine.


    Brown color fades on addition of sodium thiosulphate solution due to the reaction below:


    ii. Potassium hexacyanoferrate (II) solution: A brown precipitate is formed.


    iii. Potassium (or ammonium) cyanide solution: A yellow precipitate is formed. The precipitate rapidly turns white.






    Checking up 1.6 (c)

    Aqueous sodium hydroxide is added separately to solutions of salts of the transition metals A, B and C. Identify A, B and C from the following observations

    A: The white precipitate which appears is soluble in an excess of aqueous sodium hydroxide and also in aqueous ammonia.

    B: The blue precipitate which appears is insoluble in an excess of aqueous sodium hydroxide but dissolves in aqueous ammonia to form a deep blue solution.

    C: The green precipitate which appears is insoluble in an excess of aqueous sodium hydroxide and also in aqueous ammonia.

    END UNIT ASSESSMENT

    a. Multiple choice questions: Write the Roman number corresponding to the correct answer.

    1. Which of the following elements is not a transition metal?

    i. Copper

     ii. Nickel 

    iii. Iron


     iv. Magnesium

    2. Which of the following complexes is linear?




    5. Which of the following complexes forms both geometric and optical isomers?


    6. Which of the following properties is not a characteristic of transition metal ions

    i. Variable oxidation states

     ii. Form coloured solutions

     iii. Act as catalysts 

    iv. Are diamagnetic

    7. Which complex ion shows optical isomerism and geometrical isomerism?


    8. All the following complex ions contain metal ions. Overall charges are not shown.

    Which complex ion has no overall charge? The charge of the central metal ion is given in brackets next to the formula of the complex


    9. Which atom(s) among the following transition elements have only 1 electron in 4s orbital? Chromium

    i. Cobalt

     ii. Scandium 

    iii. Zinc

    b. Open Questions 1.

     Complete the following table:


    2. What is the characteristic of electron configurations of transition metals?

    3. Which electrons, 3d or 4s, have the lowest ionization energies in a transition metal?

    4. a. Name any three transition metals that are essential to the biological system.

     b. Why do you think transition metals form coordination compounds that have covalent bonds?

    5. Name the following coordination compounds using systematic nomenclature.


    6. a. (i) What is meant by the term co-ordinate bond?

    (ii) Explain why co-ordinate bonds can be formed between transition metal ions and water molecules.

    b. What name is given to any ligand that can form two co-ordinate bonds to one metal ion? Give an example of such a ligand.

    7. In order to determine the concentration of a solution of cobalt(II) chloride, a 25.0 cm3 sample was titrated with a 0.0168 M solution of EDTA4–; 36.2 cm3 were required to reach the end-point. The reaction occurring in the titration is:

    a. What type of ligand is EDTA4–?

    b. Calculate the molar concentration of the cobalt (II) chloride solution.

    8. The ethanedioate (oxalate) ion, 2− C2O4 , acts as a bidentate ligand. This ligand forms an octahedral complex with iron (III) ions.

    a. Deduce the formula of this complex and draw its structure showing all the coordinate bonds present.

    b. Give the name of a naturally-occurring in human body complex compound which contains iron

    c. What is theimportant function of this complex compound?

    9. The compound [Co(NH3 ) 4 Cl2 ]Cl contains both chloride ions and ammonia molecules as ligands.

    a. State why chloride ions and ammonia molecules can behave as ligands.

    b. What is the oxidation state and the co-ordination number of cobalt in this complex compound?

    b. Name and give the formula of an ammonia complex used to distinguish between aldehydes and ketones

    11. Chloride ions form the tetrahedral complex ion [AlCl4 ] – but fluoride ions form the octahedral complex ion [AlF6 ] 3-. Suggest a reason for this difference

  • UNIT 2: EXTRACTION OF METALS

    UNIT 2: EXTRACTION OF METALS

    Key Unit Competence

    To be able to: Relate the properties of metals to their methods of extraction and uses and suggest preventive measures to dangers associated with their extraction.

    Learning objectives

    At the end of this unit , students will be able to:

    •  Describe the extraction of copper, iron, sodium, tantalum, zinc, wolfram and aluminium;
    • Outline and explain the uses of copper, iron, tantalum, zinc, wolfram, and tin ore (cassiterite);
    • Explain the issues associated with the extraction of metals and preventive measures;
    • Relate the properties of metals to their methods of extraction.

    Introductory activity

    1. a. Do you know any metal and mineral extracted in Rwanda?

    b. If yes, name them? 

    c. Give the applications of those metal and mineral .

    2. Most of the metals are found in nature, not as pure metals, but as compounds, i.e. combined with other chemical elements. Such metals are extracted from their compounds using chemical reactions. The following setup shows one example of a laboratory chemical reaction. Analyze it and follow the procedure to be able to interpret the results.


    Procedure

                    1. Transfer one spatula measure of copper (II) oxide to a hard-glass test-tube.  

                   2. Carefully add one spatula of charcoal powder on top of the copper (II) oxide without any mixing.  

                   3. Strongly heat these two layers for 5 minutes in a Bunsen flame.  

                  4. Allow the tube to cool and then look closely at where the two powders meet in the test tube

    Questions

                    1. Describe the solid copper (II) oxide before heating.

                    2. Name the gas formed in the reaction. 

                     3. Describe the solid remaining after heating. 

                     4. Name the solid formed in the reaction. 

                     5. Write the word and symbol equations for the reactions. 

                      6. What does this reaction tell you about the relative reactivities of carbon and copper? 

                       7. Explain why this reaction is a redox reaction.

    The chemical substances in the earth’s crust obtained by mining are called minerals. Minerals, which are source of metal economically needed, are called “Ore”. The unwanted impurities present in ore are called gangue. A native metal is any metal that is found in its metallic form, either pure or alloyed, in nature (example: Gold). The entire process of extraction of metal from its ore is called metallurgy.

    Many metals are found in the Earth’s crust as ores. An ore is usually a compound of the metal mixed with impurities. An ore is any naturally-occurring source of a metal that you can economically extract the metal from. Most metals exist in in nature as compounds, usually oxides or sulphides.

    Sulphide ores cannot be converted directly into the metal. Instead they must be converted to the oxide. This is achieved by roasting them in air. Roasting involves heating of ore in presence of air below melting point of metal in reverberatory furnace.

    Reverberatory furnace, in zinc, copper, tin and nickel production, is a furnace used for smelting or refining in which the fuel is not in direct contact with the ore but heats it by a flame blown over it from another chamber. In steel making, this process, now largely obsolete, is called the open-hearth process.

    In this process, volatile impurities escape leaving behind metal oxide and sulphur dioxide (metal sulphide is converted to metal oxide).


    This process causes problems because of the large quantity of sulphur dioxide produced. Sulphur dioxide is one of the principal causes of acid rain; hence SO2 is one of the air pollutants.

    However if the sulphur dioxide can be collected before being released into the atmosphere, it can be used to make sulphuric acid.

    Metals in their compounds are in oxidized form, i.e. have lost electron(s) and bear a positive charge. In order to get them as metals, they need to gain electrons: this process or reaction of gaining electrons is called “reduction”. Reduction of metals can be carried out using a chemical reducing agent such as carbon (coke, charcoal) or electricity. 

    When the mineral is dug up, a method must be used to separate the metal from the rest of the ore. This is called extraction of the metal.

    2.1. Relating the properties of metals to their methods of extraction

    Activity 2.1

    Make a research (in books or internet) in order .to:

       1. Find different methods of extraction of metals referring to the reactivity.

        2. Explain why the ores have to be concentrated and different ways that can be used.

    2.1.1. Methods of metal extraction according to their properties

    A number of methods are used to extract metals from their ores. The best method to use depends on a number of factors. These factors are based on the properties of the metal.

    The main factor here is the reactivity of the metal (the position it takes in the reactivity series). Let us use the following question method to clarify these factors.

    • Will the How much do the reactants cost? Raw materials vary widely in cost.
    • method successfully extract the metal? This depends on the reactivity of the metal.
    • What purity is needed, and are the purification methods expensive? Some metals are not useful unless very pure, others are useful impure.
    • How much energy does the process use? High temperatures and electrolysis use a lot of energy.
    • How efficiently, and in what quantities, can the metal be made? Continuous processes are more efficient than batch processes.
    • Are there any environmental considerations? Some processes produce a lot of pollutants.

    Different methods of metal extraction will be considered in this unit. Some examples are given below:

    • Reduction of metal oxides with carbon

    Carbon (as coke or charcoal) is cheap. It not only acts as a reducing agent, but it also acts as the fuel to provide heat for the process. However, in some cases (for example with aluminium) the temperature needed for carbon reduction is too high to be economic - so a different method has to be used. Carbon may also be left in the metal as an impurity. Sometimes this can be removed afterwards (for example, in the extraction of iron); sometimes it cannot (for example in producing titanium), and a different method would have to be used in cases like this.

    • Electrolysis of the metal ore

    This method is used to extract metals which are difficult to reduce by chemical agents. These metals include aluminium or metals which are difficult to reduce such as Group 1 and 2 metals.

    Reduction of the metal oxide with hydrogen

    Hydrogen can be used as a reducing agent, it is also used in purification of cpper. This is the main method for the extraction of tungsten from its oxide.

    Sustainable use of natural resources: As these extraction processes are expensive and the supply of ore is not infinite, it is essential to recycle the metals as much as possible. Recycling of metals is one way of conservation and sustainable use of natural resources.

    Metallurgical operations are sources of pollution, water and air pollution. Measures must be taken to eliminate or at least to minimize that kind of pollution.


    2.1.2. Concentrating the ore

    Concentrating the ore is also called “Dressing” or “Benefaction of ore”. The ore from which the metal will be extracted has to be prepared before extraction. Concentrating the ore is getting rid of as much of the unwanted rocky material as possible before the ore is converted into the metal. This simply means “Removal of gangue from ore”. This may be done by chemical or physical means.

    • By physical processes

    Physical operations use physical techniques that do not change the chemical nature of the minerals; these techniques are based on physical properties such as: density, magnetic properties, etc.… In many cases, it is possible to separate the metal compound from unwanted rocky material by physical means.

    • Mechanical sorting (Hand picking): this involves use of hands to pick the gangue and breaking away the gangue using a hammer.
    • Magnetic separation: the ore is crushed and a very strong magnet is used to sort out magnetic materials from non-magnetic materials. This method is for example used to separate wolframite from cassiterite where cassiterite being non-magnetic is not attracted by the magnet.
    • Washing: the ores are usually denser than the gangue, which may be washed away in a stream of water on an inclined table. Examples of ores separated in this way are galena and limestone; cassiterite from silicates.
    • Froth flotation method: this process is important in treating many sulphide ores like galena, zinc blende (zinc sulphide), copper pyrites, etc. Separation is based on different abilities of mineral and gangue particles to be moistened by water. During this process, the ore is first powdered and fed into a large concentration tank containing water and a suitable oil (frothing agents).

    The mixture is agitated by blowing air through at a high pressure. The sulphide ores rise to the surface in the froth while the gangue sinks to the bottom. The froth is skimmed off the surface, and an acid is added to break up the froth. The concentrated ore is filtered and dried.

    By chemical processes.

    For example, pure aluminium oxide is obtained from bauxite by a process involving a reaction with sodium hydroxide solution. Some copper ores can be converted into copper (II) sulphate solution by leaving the crushed ore in contact with dilute sulphuric acid for a long time and then copper can be extracted from the copper (II) sulphate solution.

    Leaching with aqueous solvents: in this method the finely powdered ore is treated with a suitable reagent that dissolves the ore but not impurities, for example:

    1. Bauxite is crushed and digested with sodium hydroxide solution
    2. Zinc ores can be leached with dilute sulphuric acid and electrolysed.
    • Roasting in air and Calcination: Here the ore is powdered and roasted in air to drive off the water (for the hydrated ores) and other volatile substances. For example, Carbonates decompose to release carbon dioxide. Roasting: Sulphides release sulphur dioxide gas:

    • Calcination: It is a process heating the ore strongly either in limited supply of air ih the absence in air

    Smelting is the process by which a metal is obtained, either as the element or as a simple compound, from its oxide ore by heating beyond the melting point, ordinarily in the presence of reducing agents, such as coke.

    CuO + C → Cu +CO

    Checking up 2.1

    1. What is an ore? 

    2. What is the difference between an ore and a mineral? 

    3. Are ores a finite resource? 

    4. Are ores renewable?

     5. When is carbon used for extraction?

     6. Name a metal that could be extracted from its ore using carbon. 

    7. When is electrolysis used for extraction? 

    8. What do you understand with dressing of ore, smelting, froth flotation and gangue? 

    9. Name two metals that can only be extracted by electrolysis. 

    10. Suggest a reason why iron is extracted using carbon rather than by electrolysis.

     11. State three factors which determine the choice of reduction method used for the extraction of metals from their ores.

     12. Complete with the following words: iron, extracted, crust, gold, native, elemental, reduced.

    “Metals come from the Earth’s …….. Some metals like ……. are very unreactive and are found as ………. in their ………state. Metals such as zinc, lead and ………are found combined with oxygen in compounds. These metals can be ……… using chemical reactions. The metal oxides are ………as oxygen is removed from the compound”. 

    13. Why most of metals are produced by reduction method ?

    2.2. Methods of extraction of Copper

    Activity 2.2

     Use the search engine and the library: 

    1. To find out the name of the two main ores of Copper.

     2. To describe the full process in copper metal is extracted from its ores.

     3. To demonstrate how copper is useful in our daily life.

    We are going to deal with the extraction of copper from its ores, its purification by electrolysis, and some of its uses.

    2.2.1. Extracting copper from its ores

    There are two main copper ore types of interest, copper  oxide ores  and copper sulphide ores. Both ore types can be economically mined, however, the most common source of copper ore is the sulphide ore mineral chalcopyrite also known as copper pyrites, which accounts for about 50 percent of copper production.

    Table 2.1: Some main ores of copper

    The ores typically contain low percentages of copper and have to be concentrated by, for example, froth flotation before processing.

    The method used to extract copper from its ores depends on the nature of the ore. Sulphide ores such as chalcopyrite are converted to copper by a different method from silicate, carbonate or sulphate ores. Copper, Cu, is mainly extracted from the ore chalcopyrite, CuFeS2 , in a three stage process.

    • In the first stage, chalcopyrite is heated with silicon dioxide and oxygen

    2 CuFeS2 + 2 SiO2 + 4 O2 → Cu2 S + 2 FeSiO3 + 3 SO2

    • In the second stage, the copper (I) sulphide is roasted with oxygen at a high temperature in a reverberatory furnace giving copper (II) oxide.

    Cu2 S + 2 O2 →2 CuO + SO2

    • In the third stage, the copper (II) oxide is reduced by heating with carbon.

    CuO + C → Cu +CO

    The end product of this is called blister copper - a porous brittle form of copper, about 98 - 99.5% pure.

    2.2.2. Purification of copper

    When copper is made from sulphide ores by the first method above, it is impure. The blister copper is first treated to remove any remaining sulphur (trapped as bubbles of sulphur dioxide in the copper - hence “blister copper”) and then cast into anodes for refining using electrolysis(electrolytic refining).The purification uses an electrolyte of copper (II) sulphate solution, impure copper anodes, and strips of high purity copper for the cathodes.

    The diagram shows a very simplified view of a cell.



    • At the cathode, a reduction reaction takes place; copper (II) ions are deposited  as pure copper: Cu2+(aq) + 2 − e →Cu(s)
    • At the anode, an oxidation reaction takes place; impure copper goes into solution as copper (II) ions: Cu(s) → Cu2+(aq) + 2 −

    For every copper ion that is deposited at the cathode, in principle another one goes into solution at the anode. The concentration of the solution should stay the same.

    All that happens is that there is a transfer of copper from the anode to the cathode. The cathode gets bigger as more and more pure copper is deposited; the anode gradually disappears.

    In practice, it is not quite as simple as that because of the impurities involved. What happens to the impurities?

    • Any metal in the impure anode which is below copper in the electrochemical series (reactivity series) does not go into solution as ions. It stays as a metal and falls to the bottom of the cell as “anode sludge” together with any unreactive material left over from the ore. The anode sludge may contain valuable metals such as silver and gold.
    • Metals above copper in the electrochemical series (like zinc) will form ions at the anode and go into solution. However, they will not get discharged at the cathode provided their concentration does not get too high.

    Extracting copper from other ores

    Copper can be extracted from non-sulphide ores by a different process involving three separate stages:

    Step 1: Reaction of the ore (over quite a long time and on a huge scale) with a dilute acid such as dilute sulphuric acid to produce a very dilute copper (II) sulphate solution.

    Step 2: Concentration of the copper (II) sulphate solution by solvent extraction.

    The very dilute solution is brought into contact with a relatively small amount of an organic solvent containing a substance which will bind with copper (II) ions so that they are removed from the dilute solution. The solvent must not mix with water. Copper (II) ions are removed again from the organic solvent by reaction with fresh sulphuric acid, producing a much more concentrated copper (II) sulphate solution than before.

    Step 3: Electrolysis of the new solution. Copper (II) ions are deposited as copper on the cathode. The anodes for this process were traditionally lead-based alloys, but newer methods use titanium or stainless steel. The cathode is either a strip of very pure copper or stainless steel.

    Checking up 2.2

    1. Based on the knowledge you have on unit 1, give 3 uses of copper.
    2. Describe the process by which copper is extracted from chalcopyrite, CuFeS2
    3. Give any difference between the extraction of copper from chalcopyrite and from cuprite.

    2.3. Methods of extraction of Iron

    Activity 2.3 

    Using your own research, use the available resources (chemistry books, notebooks, internet...) to make a succinct summary of:

    1. The main ores of iron.

     2. The full process involved in the blast furnace while the iron is being extracted (Include the diagram, the raw materials introduced and the role of each and the equations of the main reactions occurring).

     3. The main different forms of iron, its properties and their respective uses.

    The common ores of iron are iron oxides, and these can be reduced to iron by heating them with carbon in the form of coke. Coke is produced by heating coal in the absence of air. Coke is cheap and provides both the reducing agent for the reaction and also the heat source - as you will see below.

    2.3.1. Iron ores

    The most commonly used iron ores are haematite, Fe2 O3 , and magnetite, Fe3 O4 . The other examples of iron ores are: Limonite (Fe2 O3 •3H2 O), Iron pyrites (FeS2 ) and Siderite (FeCO3 ).

    2.3.2. The heat source

    The air is blown into the bottom of the giant chimney called a blast furnace. 

    The blast furnace is about 30 metres high and lined with fireproof bricks. This furnace is heated using the hot waste gases from the top. Heat energy is valuable, and it is important not to waste any.

    The coke (essentially impure carbon) burns in the blast of hot air to form carbon dioxide - a strongly exothermic reaction. This reaction is the main source of heat in the furnace.

    C + O2 →CO2


    2.3.3. Extraction

    Three substances are needed to enable extraction of iron from its ore. The combined mixture is called the “charge”:

    • Iron ore 

    • Limestone (calcium carbonate). 

    • Coke - mainly carbon.

    The charge is placed into the blast furnace. Hot air is blasted through the bottom. Several reactions take place before the iron is finally produced. This is a continuous process that needs a high temperature. The high temperature is produced by burning the carbon in a blast of hot air.  Oxygen in the air reacts with coke to give carbon dioxide.

    C(s) + O2 (g) → CO2(g)

    Limestone (calcium carbonate) is added to the blast furnace to remove sandy impurities (siO2 ). The limestone breaks down to form carbon dioxide.


    Carbon dioxide produced (both from carbon and from calcium carbonate) reacts with more coke to produce carbon monoxide.


    2.3.4. The reduction of the ore

    The Fe2 O3 is reduced by both carbon (C) and carbon monoxide (CO) as shown by the equations below.


    The limestone reacts with the sand to form slag (calcium silicate)


    Both the slag and iron are drained from the bottom of the furnace.

    The calcium silicate melts and runs down through the furnace to form a layer on top of the molten iron. It can be tapped off from time to time as slag.

    The slag is mainly used in the construction industry (to build roads, to make breeze blocks, as “slag cement” - a final ground slag which can be used in cement, often mixed with Portland cement…)

    The iron whilst molten is poured into moulds and left to solidify - this is called cast iron.

    In Rwanda tradition, iron was produced from an iron ore (heamatite, Fe2 O3 , and magnetite,Fe3 O4 ) called ubutare ,by traditional smelters called abacuzi, they used charcoal as reducing agent. Then from that, they were able to produce traditional tools such hoes, machets, arrows speras, etc…..

    2.3.5. Different forms of iron

    • Pig iron (Cast iron after removing some impurities), an alloy of iron that contains 2 to 4 percent carbon, along with varying amounts of silicon and manganese and traces of impurities such as sulfur and phosphorus.

           - It is made by reducing iron ore in a blast furnace.  

           - It has a low tensile strength

           - It is used in making gates, pipes, lamp posts where high strength is not needed.

    • Wrought iron is a soft, ductile, fibrous variety that is produced from a semi-

    fused mass of relatively pure iron globules (haematite) partially surrounded by slag. It usually contains less than 0.1 percent carbon and 1 or 2 percent slag.

    - It is purer than cast iron.

     - It is fibrous and tough

     - It can be welded (joined by hammering when red hot)

     - It is malleable and ductile

     - It is used for making sheets, wire and nails. 

    - Steel is an alloy of iron, carbon, manganese, nickel and vanadium.

    2.3.6. Alloys of iron and their uses


    Checking up 2.3

    1. Iron is extracted using the Blast Furnace

         a. What is introduced into the top of the blast furnace? 

       b. What is the source of heat used in the blast furnace? Write the involved equation

       c. What is the main reducing agent and how is it produced? (give an equation)

        d. How is the iron oxide reduced by this reducing agent? (give an equation) 

       e. What is the other reducing agent and how does it reduce the iron oxide? (give an equation)

       2. The blast furnace is a continuous process. What does this mean and why is it advantageous?

    2.4. Methods of extraction of tin

    Activity 2.4

    Make a research using the appropriate books and internet to:

    1. Find out the main tin ore and state 2 regions in Rwanda where it is mined.
    2. . Describe the process taken to extract tin from its principal ore
    3. State three properties and uses of tin.

    The principal tin ore is a compound of tin and oxygen called cassiterite (gasegereti in Kinyarwanda).The main component of cassiterite is tin (IV) oxide or tin dioxide, SnO2 .

    From the time before independence of our country, cassiterite has been one of Rwandan exported products. It is extracted in some regions such as: Rutongo, Rwinkwavu, Gatumba, etc…

    2.4.1. Extraction of tin from cassiterite

    Extraction of tin from cassiterite is done into the following steps.

    • Washing: Here the minerals dug from the site must be washed to remove the soil/earth accompanying the mineral.
    • Concentration: The crushed cassiterite is concentrated by gravity separation and the magnetic impurities like wolframite [(Mn,Fe)WO4 ], etc, are separated from cassiterite by magnetic separators.
    • Roasting: The tin ore is roasted in air to remove other impurities, such as arsenic and sulphur as volatile oxides. Iron compounds, which might be present as impurities are removed by electromagnetic separation and iron pyrites change to their oxides and sulphates.
    • Leaching and washing: The roasted ore is treated with water and the soluble CuSO4 or FeSO4   are washed away from the main ore. Further lighter ferric oxide is washed away leaving behind heavier ore particles known as black tin containing 60 to 70 % SnO2 .
    • Smelting: The tin metal is extracted from its ore by carbon reduction. The concentrated ore is mixed with coke/charcoal and heated in a furnace.

           SnO2 + 2 C → Sn + 2 CO

    In the furnace, there are other impurities such as silica (SiO2 ). This one is removed using limestone. Limestone is added in the furnace and undergoes the thermal decomposition giving calcium oxide. Calcium oxide then reacts with SiO2 to form calcium silicate which has a relatively low melting point.


    Molten tin is drawn into blocks. It contains 99.5 % of tin metal and is called block tin.


    (Source: http://onelearningsolution.blogspot.com/2015/02/33-reactivity-series-of-metals-and-its.html)

    Refining of tin:  The tin obtained is purified. It is separated from copper, iron and any other element present as impurities by either thermal (liquation) -heating beyond its melting point of 232o C, and running off the molten tin, leaving behind any less fusible impurities - or by electrolytic means.

    Purer tin is obtained by the electrolysis of aqueous solution of tin (II) chloride, SnCl2  - the impure tin is made anode, while the cathode is pure tin. The electrolyte may also consist of tin sulphate containing a small amount of hydrofluorosilicic acid (H2 SiF6 ) and sulphuric acid


    2.4.2. Uses of tin

    • Tin is used to plate iron to prevent it from rusting and as alloys such as bronze (tin and copper) and solder (tin and lead). This silvery, malleable p-block metal is not easily oxidized in air and is used to coat other metals to prevent corrosion. In modern times tin is used in many alloys. The first alloy, used in large scale since 3000 BC, was bronze, an alloy of tin and copper. Most notably tin/lead soft solders, typically containing 60% or more of tin
    • Another large application for tin is corrosion-resistant tin plating of steel.
    • Because of its low toxicity, tin-plated metal is also used for food packaging, giving the name to tin cans, which are made mostly of steel.
    • Due to its resistance to atmospheric corrosion and low melting point, it can be used to make sheet glass. 

    Checking up 2.4

    1. Name the main ore of tin.
    2. Explain the extraction of tin from tin oxide.
    3. Tin metal is obtained by removing oxygen from the metal oxide. What name do we give to this chemical reaction?
    4. Explain why tin is said to be very useful.

    2.5. Methods of extraction of Zinc

    Activity 2.5

    Use the library or other search engine to

    1. Find out the main ores of zinc.
    2. Describe all steps followed to obtain the purified zinc from its sulphide ore.
    3. Demonstrate how zinc is so useful.

    The main ore of zinc is zinc blende, ZnS which is contaminated with lead sulphide. Another example of zinc ore is calamine (ZnCO3 ).

    Zinc is extracted from zinc blende in various steps such as concentration, roasting, smelting and purification which are given below in details.

               a. Process of concentration

    The first process in the extraction of zinc is the concentration. As shown in the figure 2.2, this process involves the implementation of froth floatation method for the extraction of zinc ores from zinc blende.

    Zinc blende is mixed up in a large tank consisting of a mixture of pine oil and water. Later compressed air is passed through this combination. The froth containing the concentrated zinc sulphide ores settles on the surface leaving behind the impurities in water

             b. Process of roasting

    The concentrated ore is then treated at 900o C in the presence of excess air, on the base of a reverberatory furnace.This process of heating is called roasting. During this process, zinc oxide is obtained from the zinc sulphide ore. The equation for this process is:

    2 ZnS + 3 O2 →2 ZnO + 2 SO2

           c. Process of smelting

    Here, the mixture of zinc oxide and coke is heated in the presence of carbon to obtain zinc. This is a reduction of zinc. The involved equation is: ZnO + C →Zn + CO

    The process is employed in a vertical container. In this whole process, the zinc oxide and coke are mixed in the ratio 2:1 and in the form of a compressed mixture. This mixture is introduced into the furnace and is heated inside at a temperature of about 1400 o C. Zinc is obtained in the form of vapors which later condenses in the condenser which gives out molten zinc called spelter zinc (impure zinc).

          d. Purification process

    This is the last step of the entire process of zinc extraction. The molten zinc obtained from the previous process contains some impurities. Hence the process of the removal of these impurities is called Purification. This process can be done in two ways as given below.

             • Fractional distillation

    This is very useful for low boiling metals like zinc and mercury. The impure metalsis evaporated to obtain the pure metal as distillate.

           • Electrolysis process

    Electrolysis is one method of removing impurities from the zinc spelter. The method uses a zinc rod which acts as a cathode, while the impure zinc serves as an anode. ZnSO4 and dil H2 SO4 are mixed up and used as an electrolyte.

    The current is passed through the electrolyte; Zinc deposited on the cathode leaving the impurities in the electrolyte solution.


    Checking up 2.5

    1.      Recall 2 uses of zinc (refer to unit 1)
    2. Describe the extraction of zinc from zinc oxide.
    3. Zinc is extracted by removing oxygen from zinc oxide.

               a. What name is given to a reaction in which oxygen is removed from a substance?

                b. Explain how oxygen can be removed from zinc oxide to make zinc.

          4.  Describe different methods by which the impurities in zinc extracted can be removed

    2.6. Methods of extraction of Sodium

    Activity 2.6

    You are requested to use all resources about sodium (books, internet, textbooks).

    1. Discuss on the importance of sodium and its compound in Chemistry and in everyday life.
    2. Sodium metal does not occur in Free State in nature. Explain why these statement?
    3. Use the available resources to describe the way this valuable metal can be obtained at large scale (include the mining process, separation methods from its compounds, reaction equations where necessary, the main drawbacks that can be encountered during this process and the way to overcome them).

    On industrial scale sodium metal is extracted by “Down’s Process”. Down’s Process is based on the electrolysis of fused salt (NaCl).  This compound is found all around the world, dissolved in sea water. It is also mined from the ore called rock salt, which is made up mainly of sodium chloride (NaCl).

    2.6.1. Extraction using Down’s Cell

    The salt is found mixed with insoluble impurities of sand and bits of rock. Once the dissolved rock salt has been filtered, we are left with a solution of sodium chloride in water. You might think that this could be electrolysed to extract the sodium. However, because sodium is more reactive than the hydrogen in the water, hydrogen would be produced at the cathode instead of sodium. Instead, sodium chloride is crystallized out of the solution and melted. The molten sodium chloride is then electrolysed to extract the sodium metal. This is carried out in a Down’s cell as shown in figure below.

    (Source:http://chem1180.blogspot.com/2010/11/199-1911-electrolysis-of-molten-salts.html)

    • Down’s cell consists of a container of steel.
    • Inside of the tank is lined with firebricks.
    • Anode is a graphite rod which projects centrally up through the base of the cell.
    • Cathode is a ring of iron, which surrounds the anode.
    • The anode and cathode are separated from each other by a cylindrical steel gauze diaphragm (iron screen) so that Na and Cl2  are kept apart
    • A bell-like hood is immersed in electrolyte over the anode.
    When an electric current is passed through the molten mixture of NaCl and CaCl2 , NaCl decomposes into Na+ and Cl-  ion. Na+ ions migrate towards cathode while Cl-  ions towards the anode. The molten sodium collects in the cathode compartment where it rises to the top and is tapped off by a pipe. Chlorine is collected at the anode.

    During electrolysis, calcium is also obtained at cathode but sodium and calcium are separated from each other due to the difference in density. Density of Na is 0.67 g cm-3 and the density of Ca is 2.54 g cm-3i.e.much higher than that of Na. That is why they do not mix with each other.

    2.6.2. Problems with Down’s method
    Down’s Cell NaCl is a poor conductor in its solid form, but fusing it allows for conduction of electric current by mobile ions. However, in its liquid form, its melting point is at about 800ºC, a point at which a “metallic fog”  will form between the electrolyte (NaCl) and the metallic sodium (Na) being formed and this is impossible to separate.

    2.6.3. Steps to overcome this difficulty
    In order to overcome this difficulty instead of only NaCl, a mixture of NaCl and CaCl2  is electrolyzed in Down’s cell. The melting point of this mixture is 600 o C. At 600 o C, no metallic fog is formed. The composition of the charge in Down’s Cell is NaCl = 42 %
    and CaCl2 = 58 %

    2.6.4. Uses of sodium

    • Molten sodium is used as a coolant in some types of nuclear reactor. Its high thermal conductivity and low melting temperature and the fact that its boiling temperature is much higher than that of water make sodium suitable for this purpose.
    • Sodium wire is used in electrical circuits for special applications. It is very flexible and has a high electrical conductivity. The wire is coated with plastics to exclude moisture.
    • Sodium vapour lamps are used for street lighting; the yellow light.
    • Sodium amalgam and sodium tetrahydridoborate, NaBH4 , are used as reducing agents.
    • Sodium  is also a component of  sodium  chloride (NaCl), a very important compound found everywhere in the living environment; particularly as cooking and table salt.
    • Other uses are: to improve the structure of certain alloys; in soap, in combination with fatty acids, to purify molten metals, etc.
    • In countries that experience very cold winter, NaCl is spread on the roads to de-ice the roads.

    Checking up 2.6

    1. Why is sodium not extracted by carbon reduction process? What is the method used?
    2. What difficulties arise in the extraction of sodium from its ore?
    3. Choose the suitable answer. In sodium extraction, fused (molten) NaCl is used rather than the dissolved (aqueous) NaCl because: 
    •  Obtaining molten NaCl is easy than obtaining aqueous NaCl.
    • In molten NaCl, the ions are free to move and not in aqueous NaCl. 
    •  Molten sodium NaCl is an electrolyte and not the aqueous NaCl.
    •  d. Electrolysis of molten NaCl gives Na metal at the cathode but that of aqueous NaCl gives H2 gas

    2.7. Methods of extraction of Aluminium

        Activity 2.7

    Research in library textbook or search engine about aluminium and its extraction and make a good summary containing the following:

    1. The main ores of aluminium.
    2. Why aluminium extraction is suitable to be done by electrolytic method rather than reduction with carbon.
    3. The way the main ore is purified to have the pure aluminium oxide
    4. The process by which aluminium is extracted from the purified ore by electrolytic method (include the diagram, reaction equations at electrodes and the way to solve some difficulties which may arise during this extraction process)
    5. The properties of aluminium which makes it to be very important in our daily uses and the uses of aluminium.
    The main ore of aluminium is called bauxite (Al2 O3.2H2 O). Other examples of ores are: Cryolite (Na3  AlF6 ), Feldspar (KAlSiO3 O8 ) and Mica [KAlSiO10 (OH)2 ].

    Bauxite is purified to yield a white powder, aluminium oxide, from which aluminium can be extracted. Aluminium is too high in the electrochemical series (reactivity series) to extract it from its ore using carbon reduction. The temperatures needed are too high to be economic. Instead, it is extracted by electrolysis as follows

    2.7.1. Purifiying the bauxite (The Bayer Process)

    The bauxite (red-brown solid) - hydrated aluminium oxide mixed with impurities - is extracted from the earth-crust. The extracted aluminium oxide (bauxite) is then treated with alkali; this separates insoluble impurities from aluminium which forms soluble complex ion Al(OH)4 -.

                  a. Reaction with sodium hydroxide solution

    Crushed bauxite is treated with moderately concentrated sodium hydroxide solution. The concentration, temperature and pressure used depend on the source of the bauxite and exactly what form of aluminium oxide it contains. Temperatures are typically from 140 °C to 240 °C; pressures can be up to about 35 atmospheres. High pressures are necessary to keep the water in the sodium hydroxide solution liquid at temperatures above 100 °C. The higher the temperature, the higher the pressure needed.

    With hot concentrated sodium hydroxide solution, aluminium oxide reacts to give a solution of sodium tetrahydroxoaluminate (sodium aluminate).

    Al2 O3 + 2 NaOH + 3 H2 O →2 NaAl(OH)4

    The impurities in the bauxite remain as solids. For example, the other metal oxides present tend not to react with the sodium hydroxide solution and so remain unchanged. Some of the silicon dioxide reacts, but goes on to form a sodium aluminosilicate which precipitates out.

    Silica (SiO2 ) also dissolves in sodium hydroxide to form soluble sodium trioxosilicate (IV), Na2 SiO3 .

    SiO2  + 2 NaOH →Na2 SiO3  + H2 O

    The impurities are filtered out and the filtrate contains sodium tetrahydroxoaluminate (III) and sodium trioxosilicate (IV) only

                  b. Precipitation of aluminium hydroxide

    CO2  is bubbled through the filtrate containing sodium tetrahydroxoaluminate (III) and sodium trioxosilicate (IV). At this stage the solution may be seeded with freshly precipitated aluminium hydroxide.

    NaAl(OH)4 (aq) + CO2 (g)  →  NaHCO3 (aq) + Al(OH)3 (s)

                     c. Formation of pure aluminium oxide

    Aluminium oxide (sometimes known as alumina) is made by heating (decomposition) the aluminium hydroxide to a temperature of about 1100 – 1200 °C.

    2 Al(OH)3 → Al2 O3 + 3 H2 O

    2.7.2. Extraction of the aluminium from purified bauxite by electrolysis (Hall-Heroult Process)

    Alumina (purified bauxite) is then transported to huge tanks. The tanks are lined with graphite that acts as the cathode. Also blocks of graphite hang in the middle of the iron (steel) tank, and acts as anodes.

    The alumina is mixed with cryolite, Na3 AlF6 and this lowers the melting point of the mixture - Cryolite is another aluminium ore, but is rare and expensive, and most of it is now synthesized.


    The electrode equations are as follows:

    • At the cathode: Here the aluminium ions capture electrons to become atoms again:

                 Al3+ + 3e- → Al

    •   At the anode: The oxide ions lose electrons to become oxygen molecules, O2 :

                  2 O2-→ O2 + 4e-

    The positive electrode burns away as the carbon reacts with the oxygen produced there.

    C + O2 →CO2

    Since during electrolysis, the carbon electrodes get consumed, they have to be replaced periodically. For each kg of aluminium about 0.5 kg carbon is burnt away.

    2.7.3. Uses of aluminium

    • It is a good conductor of electricity. Since it is not as good conductor as copper, thicker cables of aluminium are used for transmission of electricity.
    • Aluminium forms many useful alloys e.g., magnalium (Al and Mg), duralumin (Al, Cu, Mg and Mn). Aluminium alloys are used in aircraft and other transportation vehicles because of its low density.
    • It is used as jewellery because it is a shiny metal, it has a good appearance.
    • Resists corrosion because of the strong thin layer of aluminium oxide on its surface. This layer can be strengthened further by anodising the aluminium.
    • It is used for making window frames.
    • Aluminium foil is used for wrapping cigarettes, food, etc because it reflects light.
    • Drink cans because it is not toxic.
    • Aluminium utensils are extensively used for household purposes.
    • Aluminium is used to produce metals such as chromium and manganese from their ores (aluminothermic process).

                                                                                                                        Cr2 O3  + 2 Al   →  Al2 O3  + 2 Cr

                                                                                                                         3 MnO2  + 4 Al → 2 Al2 O3  + 3 Mn

    2.7.4. Recycling of aluminium

    Aluminum is one of the most recycled materials in the world. This is due to high cost of new aluminium that involves high cost of electricity needed to produce aluminium. Recycled aluminium cost less in production and constitutes another way of sustainable management of our natural resources.

    • The consumer throws aluminium cans and foil into a recycle bin.
    • The aluminium is then collected and taken to a treatment plant.
    • In the treatment plant the aluminium is sorted and cleaned ready for reprocessing.
    • • It then goes through a re-melt process and turns into molten aluminium, this removes the coatings and inks that may be present on the aluminium.
    • The aluminium is then made into large blocks called ingots.
    • The ingots are sent to mills where they are rolled out, this gives the aluminium greater flexibility and strength.
    • This is then made into aluminium products such as cans, chocolate wrapping and ready meal packaging.
    • In as little as 6 weeks, the recycled aluminium products are then sent back to the shops ready to be used again.

                    Checking up 2.7

     Consider the electrolytic extraction of aluminium.

    1. How is aluminium ore called?
    2. Explain why cryolithe is added to aluminium oxide
    3. 3. Describe the process by which the ore of aluminium is purified.
    4. Write half-equations for the reactions at each electrode, and write an overall equation for the reaction.
    5. 5. State what each electrode is made of.
    6. Explain why                  
    • The anodes need to be regularly replaced.
    • The electrolysis of aluminium oxide is expensive.
    • Aluminium is recycled.

    7. Give three uses of aluminium and the properties responsible for each use.

    2.8. Methods of extraction of Wolfram (Tungsten)

                    Activity 2.8

    1.      Visit the nearby mining sites of wolfram and make a field report.
    2. Research using internet and some books and make a summary about the following:
    •    The ores of wolfram.
    • Where in Rwanda do we find wolfram?
    • How wolfram extraction differs from that of zinc in terms of reduction.
    • Full description of the extraction process of tungsten from its ore.
    • The main uses of tungsten

    Tungsten ore is a rock from which the element tungsten can be economically extracted. The ore minerals of tungsten include wolframite [(Fe, Mn)WO4 ], scheelite (CaWO4 ) and ferberite (FeWO4 ).

    Tungsten is a dull silver-colored metal with the highest melting point (3410 ºC) of any pure metal. Also known as Wolfram, from which the element takes its symbol, W, tungsten is more resistant to fracturing than diamond and is much harder than steel. It is unique in being a refractory metal - its strength and ability to withstand high temperatures - that make it ideal for many commercial and industrial applications.

    Most tungsten ores contain less than 1.5% WO3  and frequently only a few tenths of a percent. On the other hand, ore concentrates traded internationally require 65-75% WO3 .  Therefore, a very high amount of gangue material must be separated.  This is why ore dressing plants are always located in close proximity to the mine to save transportation costs.

    2.8.1. Processing

    Modern processing methods dissolve scheelite and wolframite concentrates by an alkaline pressure digestion, using either a soda ash (Na2 CO3 ) or a concentrated NaOH solution. The sodium tungstate solution obtained is purified by precipitation and filtration, before it is converted into an ammonium tungstate solution. This stage is carried out exclusively by solvent extraction or ion exchange resins. Finally, high purity Ammonium paratungstate (APT) is obtained by crystallization.

    Wolframite concentrates can also be smelted directly with charcoal or coke in an electric arc furnace to produce ferrotungsten (FeW) which is used as alloying material in steel production. Pure scheelite concentrate may also be added directly to molten steel

    Once tungsten ore has been processed and separated, the chemical form, ammonium paratungstate (APT), is produced.

    2.8.2. The extraction process

    APT can be heated with hydrogen to form tungsten oxide (WO3 ) or will react with carbon at temperatures above 1050°C to produce tungsten metal. Pure tungsten cannot be obtained by reducing tungsten (VI) oxide using carbon, because it reacts with carbon to make tungsten carbide. Instead, the reducing agent is hydrogen.

    Powdered tungsten (VI) oxide is heated to temperatures in the range 550 - 850°C in a stream of hydrogen.

    WO3  + 3 H2  W + 3 H2 O

    An excess of hydrogen is used, and this carries away the steam produced during the reaction. The hydrogen is dried and recycled.

    Great care obviously has to be taken to keep the whole system free of air to avoid explosion risks with the hydrogen at these high temperatures.

    2.8.3. Advantages and disadvantages of the process

    a. Advantages:

    • It produces very pure tungsten
    • Hydrogen is a cheap reagent

    b. Disadvantages:

    • The energy cost are high
    • Using a flammable gas such as hydrogen at high temperatures is very dangerous

    2.8.4. Uses

    • Tungsten is mostly used in light bulb filaments which heat up to 2000ºC, when many other metals would vaporise, particularly at the pressures found inside light bulbs. This is because it has a very high melting point.
    • Tungsten has the highest melting point of all metals and is alloyed with other metals to strengthen them. Tungsten and its alloys are used in many high-temperature applications, such as arc-welding electrodes and heating elements in high-temperature furnaces.
    • Tungsten carbide (WC) is extremely hard and is very important to the metalworking, mining and petroleum industries. It is made by mixing tungsten powder and carbon powder and heating to 2200°C. It makes excellent cutting and drilling tools, including a new ‘painless’ dental drill which spins at ultrahigh speeds.
    • Calcium and magnesium tungstates are widely used in fluorescent lighting. Tungsten mill products are either tungsten metal products, such as lighting filaments, electrodes, electrical and electronic contacts, wires, sheets, rods etc or tungsten alloys.
    • Due to tungsten’s ability to keep its shape at high temperatures, tungsten filaments are now also used in a variety of household applications, including lamps, floodlights, heating elements in electrical furnaces, microwave ovens, x-ray tubes and cathode-ray tubes (CRTs) in computer monitors and television sets.
    • The metal tolerance to intense heat also makes it ideal for thermocouples and electrical contacts in electric arc furnaces and welding equipment.
    • Applications that require a concentrated mass, or weight, such as counterweights, fishing sinkers, and darts often use tungsten because of its high density (19.3 g/cm3 ).

    Checking up 2.8

    1. Nowadays, there is a special reduction method used to extract Tungsten from its ores.
    • State 2 main ores of tungsten
    • Write the balanced equation of the reduction reaction of tungsten (II) oxide.

    2. Suggest the reason why ore concentrating plants are always located in close proximity to the mine.

    3. Give 2 widely known physical properties of tungsten and the uses associated to these properties.

    2.9. Methods of extraction of tantalum

    Activity 2.9

    • Visit the nearby mining sites of tantalum and make a field report.
    • The picture below shows the miners at work in Rwanda. The metal being extracted here is very important in modern area. According to Merchant and Consulting Ltd (2018), Rwanda is the world’s largest producer of this metal which is called “tantalum”

                                                                                                                                   

    Research using any relevant source of information about tantalum:

    • To find out the physical properties of tantalum metal and its main uses.
    • To make a description of the extraction of tantalum from its main ore tantalite.

    Tantalum is a hard, heavy, shiny, grayish-blue metal that is very stable, almost impervious (impermeable) to air, water and all but a few acids. It has the third highest melting point of all elements (over 3000 o C), and its primary use is in capacitors for electronic applications, and for vacuum furnace parts. 

    It is classified as a “refractory” metal, which means it can sustain high temperatures and resist corrosion. It is a good conductor of heat and electricity, which makes it useful in various electronics. Pure tantalum can be drawn into fine wire filament, which is used to evaporate other metals.

    2.9.1. Where tantalum is found

    Tantalum is found in hard rock deposits such as granites, carbonites and pegmatites (igneous rock that consists of coarse granite). The chief tantalum ores are tantalite [(Fe, Mn)(Ta, Nb)2 O6 ], which also contains iron, manganese and niobium (former name is columbium), and samarskite, which contains seven metals. Another ore which contains tantalum and niobium is pyrochlore. In Rwanda tantalum is found with niobium in mineral known as coltan (colomb-tantalite).

    Tantalum is an important component in many modern technologies, and is used in capacitors for everything from computers to mobile phones.

    Despite its importance in the world today, tantalum mining takes place in very few countries and mining it is difficult. Only four countries produced tantalum in 2016, and most was mined  in the Democratic Republic of Congo (DRC). Rwanda, Brazil and China were the other top countries for tantalum mining in that year. Sites are being identified for future development, and existing sites are being evaluated for expansion.

    2.9.2. How tantalum is mined

    Tantalum comes from the processing and refining of tantalite. Tantalite is the common name for any mineral ore containing tantalum. Most tantalum mines are open pit; some are underground.

    The process of mining tantalum involves blasting, crushing and transporting the resulting ore to begin the process of freeing the tantalum. Before transportation, the ore is concentrated at or near the mine site, to increase the percentage (by weight) of tantalum oxide and niobium. The material is concentrated through wet gravity techniques, gravity, electrostatic and electromagnetic processes.

    2.9.3. How tantalum is processed

    The tantalum concentrate is transported to the processor for chemical processing. The concentrate is then treated with a mixture of hydrofluoric and sulphuric acids at high temperatures. This causes the tantalum and niobium to dissolve as fluorides.

    Numerous impurities are also dissolved. Other elements, such as silicon, iron, manganese, titanium, zirconium, uranium and thorium, are generally present and processed for other uses.

    The concentrate is broken down into a slurry (A slurry is a watery mixture of insoluble matter such as mud, lime, or plaster of Paris). The slurry is filtered and further processed by solvent extraction. Using methyl isobutyl ketone (MIBK), or liquid ion exchange using an amine extract in kerosenes, produces highly purified solutions of tantalum and niobium. In this way, the tantalum oxide is obtained which is finally reduced with molten sodium to produce tantalum metal in powder form.

    It can then be compacted (as it is for capacitors) to final shape, or may be melted (and refined) in an electron beam furnace.

    2.9.4. Uses for tantalum

    • Tantalum is used to make electrolytic conductors, aircraft engines, vacuum furnace parts, nuclear reactors and missile parts.
    • Tantalum is unaffected by body fluids, and is non-irritating, which makes it useful for surgical appliances.
    • It is common in the production of cell phones, personal computers, igniter chips in car air bags, cutting tools, drill bits, teeth for excavators, bullets and heat shields.
    • Because the metal is an electrical conductor, it is useful in many consumer electronics, such as microprocessors for plasma televisions.

    Checking up 2.9

    In pairs, answer the following questions:

    1. Where tantalum is found in Rwanda?
    2. How tantalum is mined.
    3. How tantalum is processed
    4. Give 3 uses of tantalum.
    5. What is the role of methyl isobutyl ketone (MIBK) in tantalum processing?

    2.10. Dangers associated with extraction of metals

    Activity 2.10

    If you have ever visited a mining site, remember all the processes involved and suggest all possible common dangers associated with the extraction of metals.

    The following are some of the dangers associated with metals extraction. Especially, these hazards are found in smelting and refining and in addition mining.

    1. Injuries

    Metal extraction industry has a higher rate of injuries than most other industries. Sources of these injuries include: splattering and spills of molten metaland slag resulting in burns; gas explosions and explosions from contact of molten metal with water; collisions with moving vehicles; falls of heavy objects; falls from a height,slipping and tripping injuries from obstruction of floors and passageways.

    Precautions

    Adequate training, appropriate personal protective equipment (PPE) [for example, hard hats, safety shoes, work gloves and protective clothing]; good storage, housekeeping and equipment maintenance; traffic rules for moving equipment (including defined routes and an effective signal and warning system); and a fall protection programme.

    2.   Heat illnesses

    Heat stress illnesses such as heat stroke are a common hazard, primarily due to infrared radiation from furnaces and molten metal. This is especially a problem when strenuous work must be done in hot environments.

    Prevention of heat illnesses

    Water screens or air curtains in front of furnaces, spot cooling, enclosed airconditioned booths, heat-protective clothing and air-cooled suits, allowing sufficient time for acclimatization, work breaks in cool areas and an adequate supply of beverages for frequent drinking.

    3.   Pollutions

    Mining operations are major contributors to the pollution of our environment such as: air pollution, water pollution, degradation of landscape, etc.

    Exposure to a wide variety of hazardous dusts, fumes, gases and other chemicals can occur during smelting and refining operations. Crushing and grinding ore in particular can result in high exposures to silica and toxic metal dusts (containing lead, arsenic and cadmium, for example). There can also be dust exposures during furnace maintenance operations. During smelting operations, metal fumes can be a major problem especially risk of developing respiratory system illness. In metallurgical operations, the carbon dioxide released has more dangers especially the global warming because it is a greenhouse gas. Acid gases released in atmosphere such as SO2 , SO3 , NOx are sources of acid rains.

    Control

    Dust and fume emissions can be controlled by enclosure, automation of processes, local and dilution exhaust ventilation, wetting down of materials, reduced handling of materials and other process changes. Where these are not adequate, respiratory protection would be needed.

    Many smelting operations involve the production of large amounts of sulphur dioxide from sulphide ores and carbon monoxide from combustion processes. Dilution and local exhaust ventilation (LEV) are essential.

    Sulphuric acid is produced as a by-product of smelting operations and is used in electrolytic refining and leaching of metals. Exposure can occur both to the liquid and to sulphuric acid mists. Skin and eye protection and LEV are needed.

    The extraction of some metals can have special dangers. Examples include fluorides in aluminium smelting, arsenic in copper, etc. These processes require their own special precautions

    Other dangers

    •   Glare and infrared radiation from furnaces and molten metal can cause eye damage including cataracts. Proper goggles and face shields should be worn. High levels of infrared radiation may also cause skin burns unless protective clothing is worn.
    • High noise levels from crushing and grinding ore, gas discharge blowers and high-power electric furnaces can cause hearing loss. If the source of the noise cannot be enclosed or isolated, then hearing protectors should be worn. A hearing conservation program including audiometric testing and training should be instituted.
    • Electrical hazards can occur during electrolytic processes. Precautions include proper electrical maintenance with lockout/tagout procedures; insulated gloves, clothing and tools; and ground fault circuit interrupters where needed.
    • Manual lifting and handling of materials can cause back and upper extremity injuries. Mechanical lifting aids and proper training in lifting methods can reduce this problem.

    CASE OF RWANDA

    According to Rwanda Environment Management Authority (REMA), mining activities often impact significantly on the environment. For instance, sand collecting and quarrying are already shown some significant environmental impacts, including resource depletion, energy consumption, waste generation and emissions of air pollutants. The dangers to human life and health associated with mining include the displacement of people, land use changes, dust and noise pollution.

    In fact, the preparation of ores which uses a lot of water constitutes a major pollutant of stream water in Rwanda. For example, the waters draining the mining sectors of Rutongo and Gatumba pollute the rivers of Nyabarongo and Nyabugogo by sediments of clay and sand which they transport over long distances. It is this considerable mineral load which partly gives them the brown

    colour that is characteristic of the rivers in Rwanda. Mining and quarrying produce massive rejects which appear in nature in the form of enormous lots of earth and rocks. Erosion from rain water transports the mineral residue towards the valleys where streams are filled and covered by the residue which may be toxic to biodiversity

    Checking up 2.10

    1. State 5 sources of injuries associated with the extractions of metals
    2. Give 3 ways you can prevent from heat illnesses.
    3. Describe 2 ways you can control the dangers associated with the chemicals in extraction of metals.
    4. Suggest a way of protecting mining workers against the risk of lung disease due to dust at their working place?

    2.11. Preventive measures associated with metal extractions

    Activity 2.11

    We already know that there are many dangers associated with the extraction of metals.

    Recommend measures that must be taken to prevent from these dangers (risks).

    Effort should be made by mining companies or planned for the future, to eliminate or minimize the environmental problems associated with metal extractions include:

    1. The potential sources of air contaminants should be enclosed and isolated.
    2. Brief, for any operation related to metal extraction, measures must be adopted to protect the workers in particular and the environment in general by:
    • Elimination or reduction of air polluting gases
    • Avoiding water and soil pollution.
    • Protect the landscape.
    • Using cleaner production techniques i.e Minimize sources of pollution and use of energy.

    3.  Adopt technology that minimizes wastes produced through processreengineering/recycling

    Checking up 2.11

    1. In extraction of metals, the best and least costly preventive measures are those taken at the planning stage of a new process of extraction. Explain the main aspects that should be taken into account.
    2. what are the main sources of pollution in metallurgy?

    END UNIT ASSESSMENT

    1. Which metal is extracted from Bauxite?

                a. Tin

                b. Tantalum

                 c. Copper

                 d. Aluminum

    2. Brass is 

               a. An Element 

                b. A Compound

                c. A Mixture

                d. An Alloy

    3. Bronze is an alloy of 

        a. Copper and Zinc  

        b. Lead and Copper

         c. Copper and Tin

          d. Barium, Zinc and Iron

    4. Which of the following metals is often found in pure state? 

             a. Copper 

             b. Iron

              c. Gold 

              d. Aluminum

    5. Which metal is extracted from Haematite?

                a. Tin

                b. Iron 

               c. Manganese 

               d. Cadmium

    6. Rocks rich in metals with economic value are known as

              a. Metalloids

               b. Ores 

               c. Allotropes 

                d. Slag

    7. An alloy is a

               a. Compound of three elements 

                b. Homogeneous mixture of two or more metals

                 c. Heterogeneous mixture 

                 d. Element in impure form

    8. If a metal ore is called "pyrites" then it most probably has 

                 a. Chlorine 

                 b. Oxygen 

                  c. Sulphur 

                   d. Nitrogen

    9. Often to prevent corrosion, metals are galvanized by covering them with a layer of 

                 a. Copper 

                 b. Sodium 

                 c. Zinc 

                d. Tin

    10. What is not true about Tantalum? 

             a. It is classified as a "refractory" metal

            b. Tantalum oxide is reduced with molten sodium to produce tantalum metal in powder form.

             c. Its ore minerals include scheelite

             d. It is found in hard rock deposits such as granites, carbonites and pegmatites

    11. Complete with the terms applied in the Extraction of iron from haematite in industry (Blast Furnace).

                a. Raw materials: ___________________________________

                  A mixture of ___________, __________ and _____________ is added at the top of the furnace. ________ air is blown into the furnace from the bottom. A chain of chemical reactions occur:

               b. Carbon reacts with oxygen in air to form ______________. Equation:

               c. The hot carbon dioxide rises in the furnace and is reduced by _________ to form __________. Equation:                                               ____________________________ _______________________________________________

                d. Carbon monoxide is a ____________ agent. It ___________ iron(III) oxide in haematite to form hot molten                                             ___________.  

              Equation: ______________________________________________ The hot molten iron is then rum out from the bottom of              the furnace.

                 e. The formula of limestone: ________________ Limestone breaks up into____________ and_______________ when                       heated    

                 Equation: ________________________________________________

              f. Calcium oxide helps to remove ___________ (the impurities) to form a liquid ‘_______’. Equation:                                                              ________________________________

               12. a. By giving reagents and conditions, state three different methods of extracting metals starting from their oxides. In                    each case, write equation(s) to illustrate the extraction of an appropriate metal.

                      b. i. Why are metals more usually extracted from their oxides rather than from any other compound?

                           ii. State two environmental problems associated with the extraction of metals from their oxides or sulphides and                                   give     the chemical responsible for each problem.

                13. a. Give the ores of iron.

                        b. Explain the extraction of iron from its ores.

                14. a. Give 2 or 3 uses of aluminium, copper, zinc, and iron.

                      b. Give two reasons why the extraction of aluminium is expensive.

              15. Tungsten is prepared in a pure form by high temperature reduction of tungsten (VI) oxide with hydrogen.

                       a. Construct an equation for this reaction. 

                       b. Suggest why carbon is not used as the reducing agent.

                       c. Suggest one advantage (other than purity of the product) and one disadvantage of using hydrogen as the reducing                          agent on an industrial scale.

             16. Zinc and copper are extracted in the same way as iron (in blast furnace) but exist as their sulphide ores.

                      a. How is the sulphide ore converted into an oxide and what is the problem with this process? (give an equation) 

                      b. Why can aluminium not be extracted in this way? 

                      c. Why can tungsten not be extracted in this way?

            17. Copper is a widely used metal. The main ore of copper contains copper sulphide. Copper can be extracted from copper              sulfide in a three stage process.

                 a. In the first stage of extraction the copper sulfide is heated in air.

                  i. Balance the symbol equation for the reaction.

                          Cu2 S + O2 → CuO + SO2

                  ii. Explain why there would be an environmental problem if the gas from this reaction were allowed to escape into the                      atmosphere.

                   b. In the second stage copper oxide, CuO, is reduced using carbon. Describe and explain what happens during this                              reaction.

                   c. During the third stage the copper can be purified as shown in the diagram.

                  


                  i. What is the name of the type of process used for this purification? 

                  ii. Give one use of purified copper.

    d. Copper-rich ores are running out. New ways of extracting copper from low grade ores are being researched. Recycling of copper may be better than extracting copper from its ores. Explain why.


  • Topic 3

  • Topic 4