الكيمياء العامة 1

101 Chem 3+1
General Chemistry
 
Reference: Chemistry 11th ED.
By
T.L. Brown, H.E. Le May, B.E. Bursten and C.J. Murphy
 
I. Introduction
1.4 Units of Measurement
 
II. Stoichiometry                                                                           (7 Lectures)
3.1 Chemical Equations
3.2 Some Simple Patterns of Chemical Reactivity
3.3 Formula Weights
3.4 Avogadrro's Number and the Mole
3.5 Emperical Formulas from Analyses
3.6 Quantitative Information from Balanced Equations
3.7 Limiting Reactants and Theoretical yiels
4.5 Concentrations of Solutions
13.4 Ways of Expressing Concentrations
 
III. Gases                                                                                            (6 Lectures)
10.1 Charcteristics of Gases
10.2 Pressure
10.3 The Gas Lwas
10.4 The Ideal Gas Equation
10.5 Further Applications of the Ideal Gas Equation
10.6 Gas Mixutres and Partial Pressures
10.7 Kinetic Molecular Theory
10.8 Molecular Effusion and Disffusion
10.9 Real Gases Deviations from Ideal Behavior
 
First Mid Term Exam
 
IV. Thermochemistry and Thermodynamics                                 (6 Lectures)
5.1 The Nature of Energy
5.2 The First Law of of Thermodynamics
5.3 Enthalpy
5.4 Enthalpies of Reaction
5.5 Calorimetry (Heat Capacity and Specific Heat-Constant Pressure Calorimetry), Bomb calorimetry (constant volume calorimetry)
5.6 Hess's Law
5.7 Enthalpies of Formation
V. Properties of Solutions                                                                 (6 Lectures)
13.1 The Solution Process
13.3 Factors Affecting solubility (Pressure Effects and Temperature Effects)
13.5 Solutions of Two Volatile Liquids, Colligative Properties of Non-electrolyte Solutions and Electrolyte solutions (van’t Hoff Factor)
 
VI. Chemical Kinetics                                                                       (5 Lectures)
14.1 Factors That Affect Reaction Rates
14.2 Reaction Rates
14.3 The Rate Law: The Effect of Concentration on Rate
14.4 The Change of Concetration with Time. The Half-life (First Order Reactions Only)
14.5 Temperature and Rate
 
Second Mid Term Exam Limit
 
VII. Chemical Equilibrium                                                              (5 Lectures)
15.1 The Concept of Equilibrium
15.2 The Equilibrium Constant
15.3 Interpreting and working with Equilibrium Constants
15.4 Heterogeneous Equilibria
15.5 Calculating Equilibrium Constants
15.6 Applications of Equilibrium Constants
15.7 Le Chatelier's Principle and its Applications on Equilibria
 
VIII. Acid Base Equilibria                                                               (7 Lectures)
16.1 Acids and Bases
16.2 Bronsted-Lory Acids and Basis
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Strong Acids and Bases
16.6 Weak Acids
16.7 Weak Bases
16.8 Relationship Between Ka and Kb
16.9 Acid-Base Properties of Salt Solutions
17.1 The Common Ion Effect
17.2 Buffered Solutions
17.4 Solubility Equilibria, the solubility product Ksp