| 1 |
The range of types, properties and uses of steel (Storyline
SS1 and SS2). |
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| 2 |
The importance of the composition of a steel in determining its
properties (Activity SS2.5). |
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| 3 |
Redox processes that occur during steelmaking (including removal of
sulphur and the reactions during the oxygen blow) (Storyline SS2;
Activities SS2.2-SS2.4). |
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| 4 |
How some substances appear coloured because they absorb radiation in
specific parts of the visible spectrum. |
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| 5 |
The use of colorimetric measurements to determine the concentration of
a coloured solution (Activity SS1.1). |
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| 6 |
The procedure for carrying out a simple redox titration involving
manganate(VII) ions and how to work out the results (Activity SS1.2). |
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| 7 |
Transition metals are d-block elements that form one or more stable
ions with incompletely filled d-orbitals. |
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| 8 |
Typical properties of transition metals in the first row of the
d-block with particular reference to iron and copper; existence of
more than one oxidation state for each element in its compounds,
formation of coloured ions in solution, reactions with ligands to form
complexes and reactions involving ligand substitution, catalytic
behaviour of the elements and their compounds. |
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| 9 |
The reactions of Fe2+(aq), Fe3+(aq)
and Cu2+(aq) ions with sodium
hydroxide solution and ammonia solution (Activity SS5.3). |
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| 10 |
The variable oxidation states of transition metals in terms of
electronic energy levels. |
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| 11 |
The catalytic activity of transition metals and their compounds in
terms of variable oxidation states (Activity SS5.2). |
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| 12 |
The meaning of the terms: ligand, complex/complex ion
and ligand exchange. |
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| 13 |
The formation of complexes in terms of bonding between ligands and the
central metal ion. |
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| 14 |
The meaning of the term polydentate as applied to ligands,
exemplified by edta4+. |
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| 15 |
The shapes of complexes with coordination numbers 4 and 6. |
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| 16 |
Ligand exchange reactions and stability constants. |
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| 17 |
Redox reactions of d-block elements in terms of electron transfer, and
represented by (i) using half-equations for the oxidation and reduction
reactions and (ii) combining half-equations to give the overall equation
for the reaction. |
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| 18 |
The construction of simple electrochemical cells involving metal
ion/metal half-cells based on different oxidation states of the same
element in aqueous solution. |
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| 19 |
The meaning and use of the term: standard electrode potential;
how a standard electrode potential is measured. |
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| 20 |
The action of an electrochemical cell in terms of half-equations and
external electron flow. |
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| 21 |
The use of standard electrode potentials to calculate Ecell,
and to predict the feasibility of redox reactions and the relative
stability of oxidation states. |
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| 22 |
Rusting in terms of electrochemical processes involving iron and
oxygen and subsequent reactions (Storyline SS3; Activity
SS3.4). |
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| 23 |
Approaches to corrosion prevention (Storyline SS3). |
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| 24 |
Issues in the recycling of iron (Storyline SS4). |
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