Objectives for CHEM 1412

General Chemistry II

This is a list of topics to be taught in General Chemistry II. It does not reflect the order in which the topics need be taught.

 

Reference based on 6/e of General Chemistry, Whitten, Davis & Peck

 

1 Chemical Kinetics: Chapter 16

Rate of a reaction 16-1

Factors that affect reaction rates

a. Nature of reactants 16-2

b. Concentration of reactants: Rate-law expressions & Reaction order 16-3

c. Concentration vs. time: Integrated rate equations and half-life 16-4

Collision theory, activation energy 16-5

Transition state theory 16-6

Mechanisms and Rate-law expressions 16-7

Arrhenius equation: temperature and rate 16-8

Catalysts 16-9

2 Chemical Equilibria Chapter 17

Dynamic equilibria 17-1

Equilibrium constant Kc 17-2 to 17-3

Reaction quotients 17-4

Calculations with Kc 17-5

Heterogeneous equilibria 17-11

Kp and Kc 17-9

Le Chatelier's Principle: factors affecting equilibria 17-6

3 Acid-Base Theories Chapter 10

Arrhenius Acid-base theories 10-2

Bronsted-Lowry Acid-base theories 10-4

Strength of acids: binary and ternary acids 10-7

Lewis Acid-base theories 10-10

4 Acid-Base Equilibria Ch. 10, 18, 19

Ionization of water 10-5, 18-2

pH and pOH 18-3

Ka and Kb for weak acids and bases, % ionization 18-4

Polyprotic acids 18-5

Hydrolysis of salts: Relationship between Ka and Kb 18-7 to 18-10

Hydrolysis of metal ions 18-11

Common ion effect and Buffer solutions, Henderson-Hasselbalch equation 19-1

Buffering action and preparation of buffer solutions 19-2 & 19-3

Acid-base indicators 19-4

Acid-base titrations 19-5 to 19-7

5 Ionic equilibria: Solubility Chapter 20

Ksp and solubility 20-1 to 20-2

Common ion effect of solubility Reaction quotients 20-3

Predicting precipitate formation 20-3

Fractional precipitation 20-4

Simultaneous Equilibria: Ksp & Kb/Ka 20-5

Dissolving precipitate, complex formation 20-6

6 Thermodynamics Chapter 15

The First Law of Thermodynamics 15-1

Enthalpy, DH 15-2 , 15-3, 15-6

Calorimetry (constant-pressure and constant volume) 15-4

Thermochemical equations 15-5

Internal energy, DE 15-10

Relationship between DE and DH 15-11

Hess' Law 15-8

Standard enthalpies of formation and reaction 15-7

Bond energy and DH 15-9

The Second Law of Thermodynamics & Spontaneity 15-12 & 15-13

Entropy and Third Laws of Thermodynamics 15-14

Gibb's free energy 15-15

Relationship between DG and K 17-12

7 Electrochemistry Chapter 21

Balancing redox reactions 11-5 to 11-7

Electrical conduction & electrodes 21-1 & 21-2

Electrolysis 21-3 to 21-5

Faraday's law of Electrolysis 21-6

Voltaic cells 21-8 to 21-10

Standard electrode potentials 21-11 to 21-16

Nernst equation 21-19

Concentration cells 21-20

Relationship of e, DG and K 21-21

8 Coordination Compounds Chapter 25

Basics: ligands, coordination number 25-1 to 25-3

Nomenclature 25-4

Structural Isomers 25-6

Stereoisomers: geometric & optical isomers 25-7

*** Crystal field theory: high spin, low spin 25-8

*** Color & spectrochemical series 25-9

9 Nuclear Chemistry Chapter 26

n/p ratio and nuclear stability 26-2

Nuclear binding energy & nuclear stability 26-3

Radioactive decay 26-4

Nuclear equations 26-5 to 26-8

Kinetics 26-10

Nuclear fission, fusion and reactors 26-14 & 26-15

10 Introduction to Organic Chemistry Chapter 27

Types of hydrocarbons 27-1 to 27-7

Functional groups: halides, alcohols, ethers, aldehydes, ketones, amines,

carboxylic acids & derivatives 27-8 to 27-15

Nomenclature 27-2

Typical reactions: substitution, addition, elimination & polymerization 27-16-27-19

Isomers 28-1, 28-2

*** Optional