Advanced A level theoretical chemistry - chemical equilibrium

INDEX of CHEMICAL EQUILIBRIA and associated topics NOTES

+ 4Cl^-   + 6H₂O

ALL my advanced A level theoretical chemistry revision study notes

Part 0. Examples of reversible reactions

and Reversible reactions & what we mean by chemical equilibrium

(GCSE/IGCSE level, but a useful simple 'revision' introduction, the links below are all for advanced A level students)

Advanced equilibrium chemistry notes

Parts 1 to 4 - the 'basics' but advanced too!!!

Part 1. Introduction - examples of reversible reactions described, dynamic equilibrium and Le Chatelier's Principle

Part 2a. How to write equilibrium expressions and the effect of temperature on the equilibrium constant K

Part 2b. How to write K_c equilibrium expressions, units and exemplar K_c calculations including esterification

Part 2c. How to write K_p expressions, units, partial pressures and exemplar K_p equilibrium calculations

Part 3. Applying Le Chatelier's Principle and equilibrium expressions to Industrial Processes

Part 4. Partition between two phases, solubility product and ion–exchange

4.1 Partition between two phases

4.2 Solubility product K_sp & common ion effect

4.3 Ion–exchange systems

Part 5. pH, weak–strong acid–base theory and calculations

GCSE 9-1 /IGCSE notes on acids and bases (lots of basic stuff, read 1st)

5.0 A level notes on Acids, Bases, Salts, uses of acid–base titrations – upgrade from GCSE level (~US grades 9-10) (read 2nd)

5.1 Lewis and Bronsted–Lowry acid–base theories

5.2 self–ionisation of water and pH scale

5.3 strong acids - examples - pH calculations

5.4 weak acids - examples & pH-K_a-pK_a calculations

5.5 strong bases -examples -pH calculations

5.6 weak bases - examples & pH-K_b-pK_b calculations

Part 6. Salt hydrolysis, Acid–base titrations–indicators, pH curves and buffers

6.1 Salt hydrolysis

6.2 Acid–base indicator theory, pH curves and titrations

6.3 Buffers – definition, formulation and action

6.4 Buffer calculations

6.5 Case studies of buffer function

Part 7. Redox equilibria, half–cell electrode potentials, electrolysis and electrochemical series

7.0 GCSE/IGCSE/O level Notes on Electrochemistry (lots of basic stuff on several pages)

7.1 Half cell equilibria, electrode potential

7.2 Simple cells notation and construction

7.3 The hydrogen electrode and standard conditions

7.4 Half–cell potentials, Electrochemical Series and using E^θ_cell for reaction feasibility

7.5 Electrochemical cells ('batteries') and fuel cell systems

7.6 Electrolysis and the electrochemical series

7.7 Exemplar Questions, Appendix 1. The Nernst Equation, Appendix 2 Free Energy, Cell Emf and K

Part 8. Phase equilibria–vapour pressure, boiling point and intermolecular attractive forces (intermolecular bonding)

(8.1) Vapour pressure - origin and examples

(8.2) Introduction to the different types of intermolecular bonding forces operating between covalent molecules (index for 6 linked pages of examples described and explained 8.2.1-6)

(8.2.1) Three introductory sections important to read (a) to (c) first

(section 8.2.1 a-c on same page)

(a) Introduction to intermolecular forces – Van der Waals forces

(b) Dipole moments and the polarizability of a molecule

(c) Electronegativity, covalent bond character and polar molecules

Four types of intermolecular attractive force sections (2) to (6) on separate pages

(8.2.2) Instantaneous dipole – induced dipole interactions (London forces or dispersive forces)

(8.2.3) Permanent dipole – permanent dipole interactions (Keesom forces/orientation forces)

(8.2.4) Hydrogen bonding intermolecular forces

(8.2.5) Permanent dipole – induced dipole interactions (Debye forces or induction forces)

(8.2.6) Comparing the relative intermolecular bonding contributions for 8 organic molecules

(8.3) Boiling point plots of 6 organic homologous series of molecules - trends, comparisons, explanations

(8.4) Other case studies of boiling points related to intermolecular bonding forces for inorganic molecules with a similar number of electrons

(8.5) Steam distillation – theory, apparatus and practice and calculations

Evidence and theory of hydrogen bonding in simple covalent hydrides, water and other molecules and lots of other situations of hydrogen bonding described (no 8.6, now part of 8.2)

(8.7) Intermolecular bonding and solubility of covalent compounds and explaining miscible and immiscible liquids