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Salters A2 Chemistry - O "The Oceans"

Unit map and learning objectives list - part of module 2854

O1.2 What change occurs when an ionic solid dissolves

O1.3 What factors affect the enthalpy change of formation of an ionic compound

3.2 The size of ions

4.5 Energy changes in solution

4.6 The Born-Haber cycle

O3.2 What crystals form when a solution is cooled?

5.4 Forces between molecules: hydrogen bonding (revision)

O4.2 Investigating some buffer solutions

7.2 Equilibria and concentrations (revision)

8.1 Acid-base reactions (revision)

7.7 Solubility equilibria 

11.2 The s block: Groups 1 and 2 (revision)

8.2 Weak acids and pH

8.3 Buffer solutions

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

1. O describe the factors determining the relative solubility of a solute in aqueous and non-aqueous solvents [Act O 1.1; CI 4.5/5.1]
2. O explain and use the terms: (i) enthalpy change of solution, (ii) lattice enthalpy, and (iii) enthalpy of solvation of ions (= hydration for water*) in solvents [Act O 1.2; CI 4.5] * describe the hydration of (+) and (-) ions in terms of (i) their interaction with the d⁺ and d^- dipoles of water, and (ii) the extent of hydration and energy release with respect to the size of ionic radii and the charge on the ion.
3. O describe the dissolving of an ionic solid to form a solution in terms of an enthalpy cycle involving (i) enthalpy change of solution, (ii) lattice enthalpy and (iii) enthalpies of solvation of ions (hydration in water) [Act O 1.3; CI 4.5/4.6]
4. O use enthalpy cycles to perform calculations involving enthalpy change of: (i) solution, (ii) lattice enthalpy and (iii) enthalpy of solvation (hydration) [Act O 1.3; CI 4.5/4.6]
5. O explain the factors determining the radii of anions and cations, including atomic number, charge and hydration, and relate ionic size and properties [CI 3.2]
6. O construct and use a Born-Haber cycle* for a simple ionic compound [CI 4.6] * involving enthalpies of: atomisation, bond strength, electron affinity, ionisation, formation, lattice energy and be acquainted with different layout styles to solve problems eg a Hess's law quadrangle or graphical method and watch the signs and sums!
7. O discuss entropy changes in a qualitative manner, interpreting entropy as a measure of the number of ways that molecules/'formulae' and their associated energy quanta can be arranged [CI 4.3/4.4/4.5]
8. O discuss qualitatively the process of dissolving in terms of energy and entropy factors [CS O 4 Ass 1/2; Act O 3.2; CI 4.3/4.4/4.5 ]
9. O interpret the tendency of a process to occur in terms of entropy changes in the system (S^ø_sys) and surroundings (S^ø_surr), and the requirement that the total entropy change (S^ø_total) should be positive for the change to be feasible [CS O4 Ass 1/2; Act O 3.2; CI 4.4/4.5]
10. O calculate entropy changes (i) using the expression*: S_total = S_sys + S_surr and (ii) the entropy change for a reaction given the entropies of the reactants and products [Act O 3.2; CI 4.4]  * S^ø_sys = S^ø_reaction = S^ø_products - S^ø_reactants and S_surr = -H^ø/T, for physical changes the initial/final physical states equate to reactants/products, H^ø is the enthalpy for the change of state e.g. enthalpy of evaporation or melting etc. AND watch the units! H is usually in kJmol^-1 and S in Jmol^-1K^-1 
11. O compare the following properties of water to those of other liquids, and other hydrides of Group 6 elements, and relate them to (i) molecular structure, (ii) specific heating capacity, (iii) enthalpy change of vaporisation, (iv) density changes on melting [CS O 3; Act O 3.1; CI 5.4]
12. O account for the influence of oceans on climate in terms of the characteristic properties of water [CS O3]
13. O define, explain and use the following terms: weak/strong acid, weak/strong base and pH [CS O 4; Act O4.2; CI 8.1/8.2]
14. O know and explain the significance of the ionic product of water, K_w = [H⁺_(aq)][OH^-_(aq)] see[CI 8.2]
15. O use given data to calculate the pH of solutions of strong acids and strong bases* [CI 8.2] * involves using K_w 
16. O explain and use the following terms: weak acid, acidity constant K_a and pK_a (= -log₁₀[Ka]) [CS O 4; Act O 4.1; CI 8.1/8.2]
17. O use given data* to calculate the pH of solutions of weak acids [CI 7.1/7.2/8.2] * eg given K_a or pK_a and concentration to calculate pH OR given pH and concentration to calculate K_a or pK_a 
18. O explain the action of buffer solutions [CS O 4; Act O 4.2; CI 7.1/7.2/8.3]
19. O describe applications of buffer solutions [CS O 4; CI 8.3]
20. O use given data to calculate the pH of a buffer solution [CI 8.3]
21. O explain and use the term solubility product, K_sp, for simple ionic compounds of formula Xⁿ⁺ Y^n– [CI 7.7]
22. O use solubility products, K_sp's, quantitatively to perform calculations concerning dissolving and precipitation processes [CI 7.7]
23. O interpret acid-base and precipitation processes in the oceans in terms of K_a and K_sp [CS O4 Act O; CI 5.1/7.1/7.2/7.7]
24. O discuss the global influence of the processes occurring when carbon dioxide dissolves in water [CS O 4] for all of LO's 13. to 24. you may have to deal qualitatively with multiple connected so be prepared to operate Le Chatelier's Principle in this context in terms of concentration, pressure or temperature.

GENERAL REVISION NOTES

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