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Salters A2 Chemistry - SS "The Steel Story"

Unit map and learning objectives list - part of module 2849

My revision index * SS exam bashing thoughts * other SS backup material * My Salters AS homepage * My Salters A2 homepage * Email

PLEASE REMEMBER, THESE ARE NOT 'STAND ALONE' NOTES, and were designed for my classes for use alongside the Salters resources - Chemical Ideas, Chemical Storylines, Practical Activities-Investigations and the AS-A2 Revision guides all published by Heinemann Secondary Series, to reduce the reading workload and offer a study strategy. From your teacher (not me!), its handy to have the answers to the Chemical Ideas, Storylines Assignments and Activities Questions side by side with the texts and these strategy pages. You haven't time to redo the Q's but a quick read of the Q's and connecting with the official answers is valuable revision.

SS ACTIVITIES

STORYLINES

CHEMICAL IDEAS for SS

SS1.1 How much manganese is there in a paper clip?

SS1.2 A redox titration

SS1 What is steel?

9.1 Oxidation and Reduction (revision)

6.7 Where does colour come from

SS2.1 A simple redox reaction

SS2.2 What changes occur during steel making?

SS2.3 Getting the 'heat balance' right

SS2.4 How much aluminium do we need to add?

SS2.5 Which is the right steel for the job? (SS 2.3 to 2.5 are optional)

SS2 How is Steel Made?

6.1 Light and electrons (revision)

SS3.1 A simple redox reaction

SS3.2 Simple electrochemical cells

SS3.3 More electrochemical cells

SS3.4 How does steel rust

SS3.5 Understanding redox reactions

SS3 Rusting

9.2 Redox Reactions and electrode potentials

9.3 Predicting the direction of redox change

SS4 Recycling steel

SS5.1 Investigating the oxidation states of vanadium

SS5.2 How do transition metal ions act as catalysts?

SS5.3 Looking at some transition metal complexes

SS5 A Closer Look at the Elements in steel

11.5 The d Block: Characteristics of Transition Elements

2.4 Electronic Structure: sub-shells and orbitals (revision)

10.4/10.5 catalysts (revision)

11.6 The d Block: Complex Formation

SS6 Check your notes on SS

SS6 Summary

SS UNIT TEST

Unit SS Learning Outcomes

KEY: CS = Chemical storylines, CI = Chemical Ideas, Act = Activity: be able to

1. O show awareness of the range of types, properties and uses of steel; [CS SS 1 Ass1; Act SS 2.5]
2. O explain the importance of the composition of a steel in determining its properties*; [CS SS 1/2 Ass 1/6; Act SS 2.5] * know theory of alloy structure
3. O describe important redox and other processes occurring during steel making* (including removal of S with Mg, oxidising of P and Si during the oxygen blow, slag formation from CaO addition, controlling % of C, adding C, Mn or Cr etc.); [CS SS 2 Ass 2/3/4/5/6; Act SS 2.1/2.2/2.4] * could be asked about removing pollutents like carbon monoxide and dust
4. O understand that some substances appear coloured because they absorb in specific parts of the visible spectrum; [CS SS 5 Ass; Act SS 5.1; CI 6.1/6.7/11.6]
5. O use and describe the making of colorimetric (absorption) measurements to determine/calculate the concentration of a coloured solution and the production and use of a calibration graph; [Act SS 1.1]
6. O recall the procedure for carrying out a simple redox titration involving manganate(VII) ions (apparatus, end-point etc.) and be able to work out the results for eg molarity of an Fe solution, % iron in a compound or tablet; [Act SS 1.2]
7. O recall that transition metals are d-block elements forming one or more stable ions which have incompletely filled d orbitals (ie ions of electron configuration of [Ar]3d¹ to [Ar]3d⁹); [CS SS 5; Act SS 5.1; CI 2.4/11.5/11.6]
8. O describe the typical physical and chemical properties of transition metals, exemplified by the first row of the d block with particular reference to iron and copper, including from [CS SS5; Act SS 3.1/5.1/5.2/5.3; CI 10.1/10.4/10.5/11.5/11.6]:
   • (i) the existence of more than one oxidation state for each element in its compounds
   • (ii) the formation of coloured ions in solution
   • (iii) reactions with ligands to form complexes and reactions involving ligand substitution
   • (iv) the catalytic behavior of the elements and their compounds
     • physical properties like heat/electrical conduction, melting points, hardness and density etc. though they can vary significantly within the 3d block.
9. O describe the reactions of Fe²⁺ (aq), Fe³⁺ (aq) and Cu²⁺ (aq) ions with sodium hydroxide solution and ammonia solution (using observations, ionic equations and complex ion formation equations with state symbols etc.) [Act SS 5.3]
10. O explain the variable oxidation states of transition metals in terms of electronic energy levels*; [CS SS; CI 2.4/11.5/11.6] * be able to write out the electron configurations of any atom/ion from Sc/Sc³⁺ to Zn/Zn²⁺ and/or box diagrams, relate to ease of 3d electron gain/loss, relate maximum oxidation state from Sc to Mn to the total number of outer 3d/4s electrons, and to the relatively low ionisation energies (x-ref with Gp 1 and 2, with 1 or 2 outer electrons easily lost) before big rise in IE when removing an electron from an inner filled shell. 
11. O explain the catalytic activity of transition metals and their compounds in terms of variable oxidation states; [CS SS 5 Ass 10; Act SS 5.2; CI 10.4/10.5/11.5]
12. O explain and use the terms: ligand, complex or complex ion (neutral or charged), ligand exchange reaction [CS SS 5 Ass; Act SS 5.2/5.3; CI 11.6]
13. O describe the formation of complexes in terms of bonding between ligand and central metal ion, lone pair donation from ligand, dative covalent bond formation and the ligand co-ordination number and shape of complex; [CS SS 5;Act SS 5.2/5.3; CI 11.6]
14. O explain the term polydentate* as applied to ligands, exemplified by [edta]^4- [Act SS 5.3; CI 11.6] * bidentate means two lone pair donation points from the same ligand molecule eg diamine, dicarboxylic acid, amino acid, hydroxycarboxylic acid, and EDTA is a hexadentate ligand!
15. O discuss/sketch the shapes of complexes with coordination numbers 4 and 6;and be aware of possible cis and trans isomers for eg [CrCl₂(H₂O)₆]⁺ and be able to work out the oxidation state of the metal (+3 in this case), which means you need to know the charge, or lack of it on ligands such as NH₃, H₂O, Cl^-, CN^-, (COO^-)₂, EDTA^4- etc.[CI 11.6]
16. O relate ligand exchange reactions of complexes to stability constants K_stab (just a specific K_c) of different complexes (e.g. same ion with different ligands or same ligand with different ions), and be able to write Kc expressions and use Le Chatelier's principle concentration rule to suggest which species might predominate under different concentration conditions [Act SS 5.3; CI 11.6]
17. O describe redox reactions of d-block elements in terms of electron transfer by: (i) using half-equations to represent the oxidation and reduction reactions and (ii) combining half-equations to give the overall equation for the reaction; [CS SS 3 Ass; Act SS 3.1/3.2/3.3/3.4/5.2/5.3; CI 9.1/9.2/9.3/11.5]
18. O describe the construction of simple electrochemical cells involving: (i) metal ion/metal half-cells, and (ii) half-cells based on different oxidation states of the same element in aqueous solution; [CS SS 3; Act SS 3.2/3.3/3.4; CI 9.2/9.3]
19. O explain and use the term: standard electrode potential; [CS SS 3 Ass 7/8; Act SS 3.2/3.3/3.4/5.2; CI 9.2/9.3]
20. O describe and explain how a standard electrode potential is measured by using a known standard half-cell eg H_2(g)/H⁺_(aq) = 0.00V, 1M solutions of ion, and a high resistance voltmeter [Act SS 3.2/3.3/3.4; CI 9.2]
21. O explain the action of an electrochemical cell in terms of half-equations and external electron flow; [CS SS 3; Act SS 3.2/3.3/3.4; CI 9.2]
22. O measuring or using standard electrode potentials to calculate E_cell ; [CS SS Ass 3; Act SS 3.2/5.2; CI 9.2/9.3]
23. O use standard electrode potentials to predict the feasibility of redox reactions; [CS SS 3 Ass 7/8; Act SS 5.2; CI 9.2/9.3]
24. O use standard electrode potentials to predict the relative stability* of oxidation states; [CS SS 3 Ass 7/8; Act SS 5.1/5.2; CI 9.2/9.3] * examples may include changing the ligand of a transition metal ion
25. O describe rusting in terms of electrochemical processes involving iron and oxygen and subsequent reactions; [CS SS 3; Act SS 3.4]
26. O use knowledge and understanding* of redox, electrochemistry and complex formation where appropriate to interpret: (i) rate of corrosion under different conditions and (ii) approaches to corrosion prevention (including Zn coating and Cr addition) [CS SS 3 Ass 7/8; Act SS 3.4; CI 9.2/9.3/11.6] * can including half-cell equations, E theta potentials and what can influence their value 
27. O discuss and evaluate approaches to the recycling of iron; [CS SS 4 Ass 9]

GENERAL REVISION NOTES