1. Chemistry 2000 - Overview Review: Concepts from chem. 1000 important to chem. 2000 Chapter 13 - Intermolecular forces Chapter 14 – Solutions and their behaviour Dipole-dipole, dipole-induced dipole and london forces Hydrogen bonding and surface tension Properties of liquids: vapour pressure boiling points Properties of Solids: melting points, crystallinity, types of solids Concentration: Morality, molality, mole fraction and weight percent Phase diagrams Colligative properties: b.p. elevation, f.p depression and osmotic pressure Chapter 22 Transition metals and Coordination Compounds Lewis acids and Lewis bases ligands (monodentate, bidentate, chelating) co-ordination number naming co-ordination complexes and complex salts

2. Chapter 15 – Chemical Kinetics Chapter 16 – Chemical Equilibrium Chemistry 2000 Rate constant, and rate equations Zero-, first-, and second-order rate laws Collision theory and Arrhenius law Reaction co-ordinates, intermediates and transition states Mechanisms, catalysts, rate determining steps Dynamic equilibrium Equilibrium Constants Le Châtelier’s principle and reaction quotient Problem solving

3. Chapter 17 – Acids and bases Chapter 18 – Other aspects of aqueous equilibria Chemistry 2000 Lewis, Brønsted and Arrhenius definition Conjugate acid-base pairs, acid-base properties and reactions Ionization constants- Ka, Kb, Kw – and thier expressions pH, pOH, pKw, pKa and pKb More problem solving Titrations and Buffers Solubility rules, Ksp and effects on solubility Henderson-Hasselbach equation Indicators Equivalence point vs. end poin Even more problem solving

4. Chapter 6 – Energy and chemical reactions Chapter 19 – Entropy and Free energy Chapter 20 – Electron transfer reactions Chemistry 2000 Energy, stability and chemical reactions Exothermic vs. endothermic System vs. surroundings – movement of heat - “thermodynamics” Calorimetry Enthalpy calculations Laws of thermodynamics Enthalpy, entropy, and Gibbs free energy Gibbs free energy and equilibrium Temperature and equilibrium constants Oxidation states, half- reactions and balancing redox reactions Voltaic cells, electrolytic cells (batteries) and cell potentials Fuels cells and energy efficiency

5. Chemistry 1000 Review Relevant chemical concepts and related ideasKotz 6 th ed Units and significant figures Ch 1 Atomic theory of matter; element symbols and names Ch 2 Writing chemical formulae; empirical, molecular, structural and condensed structural formulae Ch3 Naming common molecular and ionic compounds Ch 3 Recognize common ions; ionic compounds and dissociation of ionic compounds in solution Ch 3 & 5 Strong and weak electrolytes; basic solubility rules for ionic compounds Ch 5 Recognize common strong and weak acids and bases; acid dissociation; base dissociation Ch 5 Classification of reactions; assigning oxidation states and recognizing oxidation reduction reactions Ch 5 Stoichiometry: moles, balancing equations, limiting reagents, percent yield Ch 2 & 4 A basic understanding of periodicity and the underpinnings of atomic and molecular structure. Ch 2 and 7-10 Molecular shape and molecular polarity Ch 9 Ideal gases; gas pressure ; gas stoichiometry; partial pressures; kinetic molecular theory Ch12

6. Common Formulae from Chem 1000 The mole Density Ideal Gases Kinetic Theory of gases Waves Quantum mechanics Nuclear Chemistry

7. Wavefunctions of H

8. Hydrogen Orbitals

9. Radial Probability Density Plot

10. P Orbitals

11. D Orbitals

12. F Orbitals

13. The Orbitals of the Hydrogen Atom 0 nodes 1 node 2 nodes Radial nodes 1 planar node 2 planar nodes

14. Atoms with more than one electron

15. Aufbau order and Energy Levels

16. Traditional aufbau sequence diagram

17. s block d block p block f block Afbau sequence from Periodic Table

18. Electron Dot Structures

19. Bond polarity and electronegativity F-F- Li + FF d

20. Pauling Electronegativity General trend in element electronegativity

21. Lewis diagrams and Molecular Shape

22. The 5 Shape Families

23. General Shape Families AX 2 & AX 3

24. Shape Family AX 4 Lone pairs and shape: 4 Electron Pairs Linear Hydrogen Fluoride, HF 1 bond pair 3 lone pairs X

25. Shape Family AX 5 : Five Electron Pairs

27. The AX 6 Family :Six Electron Pairs

28. Special features of VSEPR

29. Geometry of Large Molecules

30. Shape and Polarity

31. Permanent Dipole Moments

32. Simple Molecular Orbitals

33. Energy Levels of LCAO-Molecular Orbitals  H2H2 He 2   

34. LCAO From Atomic P Orbitals: σ-MO’s

35. LCAO From Atomic P Orbitals: π-MO’s

36. The complete energy level diagram      Li 2 – bond order 1 Be 2 - fills the σ 2s * orbital, BO = 0 B 2 - partially fills π 2p levels, BO = 1 -2 e’s parallel i.e. paramagnetic C 2 - fills π 2p, - BO = 2 - diamagnetic O 2 - partially fills π 2p * levels, BO = 2 - paramagnetic F 2 - fills π 2p * levels - BO = 1 Ne 2 – fills σ 2p *, BO = O, does not exist N 2 - fills σ 2p - BO = 3 - diamangetic

37. Electron Configurations of diatomic molecules

38. BeH 2 and sp Hybridization   

39. BH 3 and sp 2 Hybridization     

40. CH 4 and sp 3 Hybridization       

41. H 2 O and sp 3 Hybridization O 2 H sp 3 hybrids 1 s 1 s 2 C-H    2 LP’s

42. Bonding in Large Molecules sp 3 sp 2

43. Chapter 22 Transition Metal Coordination Compounds

44. Synthesis and Analysis of an Iron Complex

45. The Transition Metals

46. Variable Oxidation States

48. Chelating Ligands

49. Six-Coordinate Metals Complexed by Three Bidentate Ligands

50. Electronic Structure and Colour of Transition Metal Coordination Compounds

51. D orbitals in an octahedral ligand field

52. Origin of Colour

53. Spectrophotometer

54. Lewis acids and Lewis bases ligands (monodentate, bidentate, chelating) co-ordination number naming co-ordination complexes and complex salts electron configurations of cations d electrons and crystal field splitting why co-ordination complexes are often coloured spectrophotometry (especially for labs!) Important Concepts from Chapter 22