Download
slide1 n.
Skip this Video
Loading SlideShow in 5 Seconds..
Chemistry 2000 - Overview PowerPoint Presentation
Download Presentation
Chemistry 2000 - Overview

Chemistry 2000 - Overview

136 Vues Download Presentation
Télécharger la présentation

Chemistry 2000 - Overview

- - - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

  1. Chemistry 2000 - Overview Review: Concepts from chem. 1000 important to chem. 2000 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 Chapter 13 - Intermolecular forces 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 Phase diagrams Chapter 14 – Solutions and their behaviour Concentration: Morality, molality, mole fraction and weight percent Colligative properties: b.p. elevation, f.p depression and osmotic pressure

  2. Chemistry 2000 Chapter 15 – Chemical Kinetics 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 Chapter 16 – Chemical Equilibrium Dynamic equilibrium Equilibrium Constants Le Châtelier’s principle and reaction quotient Problem solving

  3. Chemistry 2000 Chapter 17 – Acids and bases 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 Chapter 18 – Other aspects of aqueous equilibria Titrations and Buffers Henderson-Hasselbach equation Indicators Equivalence point vs. end poin Solubility rules, Ksp and effects on solubility Even more problem solving

  4. Chemistry 2000 Chapter 6 – Energy and chemical reactions Energy, stability and chemical reactions Exothermic vs. endothermic System vs. surroundings – movement of heat - “thermodynamics” Calorimetry Enthalpy calculations Chapter 19 – Entropy and Free energy Laws of thermodynamics Enthalpy, entropy, and Gibbs free energy Gibbs free energy and equilibrium Temperature and equilibrium constants Chapter 20 – Electron transfer reactions 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

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

  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 2 nodes 1 node 0 nodes Radial nodes 2 planar nodes 1 planar node

  14. Atoms with more than one electron

  15. Aufbau order and Energy Levels

  16. Traditional aufbau sequence diagram

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

  18. Electron Dot Structures

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

  20. Pauling Electronegativity General trend in element electronegativity

  21. Lewis diagrams and Molecular Shape

  22. The 5 Shape Families

  23. General Shape Families AX2 & AX3

  24. X Shape Family AX4Lone pairs and shape: 4 Electron Pairs Linear Hydrogen Fluoride, HF 1 bond pair 3 lone pairs

  25. Shape Family AX5: Five Electron Pairs

  26. Shape Family AX5: Five Electron Pairs

  27. The AX6 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. H2 He2     Energy Levels of LCAO-Molecular Orbitals          

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

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

  36. The complete energy level diagram Li2 – bond order 1  Be2 - fills the σ2s* orbital, BO = 0     B2 - partially fills π2p levels, BO = 1 -2 e’s parallel i.e. paramagnetic  C2 - fills π2p,- BO = 2 - diamagnetic      N2 - fills σ2p- BO = 3 - diamangetic  O2- partially fills π2p* levels, BO = 2 - paramagnetic F2 -fills π2p* levels - BO = 1 Ne2 – fills σ2p*, BO = O, does not exist

  37. Electron Configurations of diatomic molecules

  38. BeH2 and sp Hybridization      

  39. BH3 and sp2 Hybridization         

  40. CH4 and sp3 Hybridization            

  41. H2O and sp3 Hybridization O 2 H 2 LP’s       sp hybrids 3   s s 1 1   2 C-H

  42. Bonding in Large Molecules sp2 sp3 sp2 sp3 sp3 sp3 sp3

  43. Chapter 22 Transition Metal Coordination Compounds

  44. Synthesis and Analysis of an Iron Complex

  45. The Transition Metals

  46. Variable Oxidation States

  47. Chelating Ligands

  48. Six-Coordinate Metals Complexed by Three Bidentate Ligands

  49. Electronic Structure and Colour of Transition Metal Coordination Compounds