Chem. 101 Course Topics (2009-2012)

Topics for Chem 101
(2009-2012)

1.      Working with Numbers
1.1.   Scientific Notation
2.      Sig Figs
2.1.   Rules for Counting
2.2.   Rules for Calculations
2.3.   Rules for Measurements
3.      Metric System
3.1.   Memorize metric prefixes
4.      Conversions
4.1.   Dimensional Analysis
4.2.   Conversions with metric
4.3.   Conversion with non metric
4.4.   Conversion with powers
5.      Density
5.1.   Calculating
5.2.   Sinking and Floating
6.      Classification of Matter
6.1.   Elements
6.1.1.    Periodic Table
6.1.1.1.  Basic Shape/order
6.1.1.2.  Names/symbols
6.1.1.3.  Metals/Nonmetals
6.1.1.4.  Group names
6.2.   Compounds
6.2.1. Writing Formulas
6.2.2.  Law of Constant Composition
6.3.   Mixtures
6.3.1.  Homogeneous
6.3.2.  Heterogeneous
7.      Properties
7.1.   Chemical
7.2.   Physical
8.      Separations
8.1.   Chemical
8.1.1. Chemical reactions
8.2.   Physical
2.1.    Filter
8.2.2.  Decant
8.2.3.  Distillation
9.      Energy
9.1.   Definition
9.2.   Specific heat
9.2.1.  Constants
9.2.2.  Calculations
9.2.2.1.  Calorimetry: Heat Lost = Heat Gained
10.  Modern definition of atoms
10.1.1.  Protons, Neutrons, Electrons
10.1.2.  Nucleus
10.2.   Periodic Table
10.2.1.  Atomic Numbers
10.3.   Ions
10.3.1.  Cations
10.3.2.  Anions
10.4. Isotopes
10.5.  Atomic Mass
11.  Electron Configuration
11.1.  Orbitals
11.1.1.  Types/Shapes
11.1.2.  Levels
11.2. Periodic Table and Order of orbitals
11.2.1.  Aufbau Principle
11.2.2.  Hunds Rule
11.2.3.  Pauli Exclusion Principle
11.2.4.  Shorthand
12.  Periodic Trends
12.1.  Size
12.2.  Ionization Energy
13.  Octet Rule
13.1. Valence Electrons
13.2. Common Charges of ions
13.2.1.  Noble Gas Electron Configuration
13.3.  Size of Ions
13.4.  Lewis Dot Structures of Atoms
14.   Ionic Compounds
14.1. Cations and Anions
14.2.  Names and Formulas
14.2.1.  Balancing Charges
14.2.2.  Polyatomic Ions
14.2.3.  Transition Metal Ions
14.2.4.  Variable charges
14.2.5.  Roman Numerals
14.2.6.  Exceptions
15.  Properties of Ionic Compounds
16.  Naming Binary Covalent Compounds
17.  Naming Acids
17.1.  Strong and Weak Acids and Bases (Memorize)
18.  Drawing Lewis Structures
18.1.  Multiple Bonds
18.2. Symmetric/Unsymmetric Molecules
18.3.  Electronegativity
18.3.1.  Polar bonds
18.4.  Polar Molecules
19.  Moles
19.1.  Definition
19.2.   Avogadro's Number
19.3.   Counting by Weighing
19.3.1.  Molar Mass
20.  Stoichiometry
20.1.   Calculations with just atoms
20.2.  Molecules
20.2.1.  Molar Mass
20.2.2.  Conversion Factors from Chemical Formulas/Subscripts
20.2.3.  Calculations
21.  Determining Formulas of Compounds
21.1. Percent Composition
21.2.  Empirical Formulas
21.3. Molecular Formulas
22.  Chemical Reactions
22.1.  Writing Equations
22.1.1.  Reactants and products
22.1.2.  States
22.2.  Balancing Reactions
23.  Moles and Chemical Reactions
23.1.  Conversion Factors from Balanced equations
23.1.1.  Coefficients
23.1.2.  Calculations
23.2.    Limiting Reactants
23.2.1.  Definition
23.2.2.  Determining which is the limiting reactant
23.2.3.  Calculations with limiting reactant
23.3. Percent Yield
23.3.1.  Definition
23.3.2.  Calculations
23.4.  Enthalpy
23.4.1.  Calculations
24.  Solubility of Ionic Compounds
24.1.   Solubility Table
25.  Types of Reactions
25.1.   Combination/Synthesis
252.  Decomposition
25.3.  Single Replacement
25.4.  Double Replacement
25.4.1.  Complete and Balance
26.  Types of Reactions 2
26.1.  Precipitation Reactions
26.1.1.  Identifying the Precipitate
26.1.2.  If no ppt, no reaction occurs
26.2.  Acid Base Reactions
26.2.1.  Complete and balance
26.3.   Gas Evolution Reactions
26.3.1.  Complete and balance
26.3.1.1.  H2S
26.3.1.2. H2CO3
26.4.   Redox Reaction
26.4.1.  Recognizing Redox Reaction
26.4.1.1. Combustion Reactions
26.4.2.  Oxidation and Reduction
26.4.2.1.  Definitions
26.4.2.2.  Identifying what species are Oxidized and Reduced
26.4.2.3. Identifying what species are the Oxidizing Agent and Reducing Agent
27.  Solutions
27.1.   Definitions
27.2.     Concentration
27.2.1.  Percent
27.2.2.  Molarity
27.2.2.1.  Dilutions
27.3.   Chemical Reactions and Molarity
27.3.1.  Calculations
27.3.2.  Titration
27.3.2.1. Indicators
27.3.2.2.  Calculations
28.  Gases
28.1.  Kinetic Molecular Theory
28.2.   Pressure
28.2.1.  Barometer
28.2.2.  Units
28.2.2.1.   Conversions
28.3.  Gas Laws
28.3.1.  Boyle's Law
28.3.2.  Charles's Law
28.3.2.1.  Kelvin Temperature
28.3.3.  Standard Temperature and Pressure
28.3.4.  Combined Gas Law
28.3.5.  Avogadro's Law
28.3.6.  Ideal Gas Law
28.3.6.1.  Molar Mass from the Ideal Gas Law
28.3.6.2. Relationship of MM to Density of Gases
28.4.  Mixtures of Gases
28.4.1.  Partial Pressure
28.4.2.  Dalton's Law
28.5.  Gases in Chemical Reactions
28.5.1.  Calculations
29.  Intermolecular Forces
29.1. Types
29.1.1.  H-Bond
29.1.2.  Dipole
29.1.3.  London
29.2.   Identifying types in Molecules
29.3.  Strength of IMFs
30.  Solids Liquids and Gases
30.1.   Properties
30.2.  Differences
31.  Physical Properties and IMF??????????
31.1. Surface Tension
31.2.  Viscosity
32.  Evaporation and Condensation
32.1.  Relationship with IMF
32.2. Relationship with Temperature
32.3.  Vapor Pressure
32.3.1.  Relationship with IMF
33.  Boiling
33.1.   Definition
33.2.   How to boil
33.3.   Relationship with IMF
34.  Melting, Freezing, and Sublimation?????????
34.1.  Energy associated with phase changes
34.2.  ΔHvap
34.3.    ΔHfus
34.4.    Calculations??????
35.  Colligitive Properties
35.1.   Melting Point Depression
35.2.   Freezing Point elevation
36.  Rates of Chemical Reactions
36.1.   Collision Theory
36.2.    Activation Energy
36.3.    Factors that affect the Rate
36.3.1.  Nature of Reactants
36.3.2.  Concentration of Reactants
36.3.3.  Temperature
36.3.4.  Size and Physical States of Reactants
36.3.5.  Catalyst
37.  Equilibrium
37.1.   Definition
37.2.  Properties of a Reaction at Equilibrium
37.3.  Equilibrium Constants
37.3.1.  Write Expressions
37.3.1.1.  States included
37.3.2.  Calculations
37.3.3.  Large or Small K - what does it "mean"
37.4.     Le Chatelier's Principle
37.4.1.  Changing amounts of reactants and products
37.4.2.  Temperature
37.4.3.  Pressure
38.  Acids and Bases
38.1. Properties of Acids
38.2. Property of Bases
38.3.  Arrhenious Theory
38.3.1.  Hydronium
38.4.  Bronsted-Lowry Theory
38.4.1.  Proton/H+
38.4.2.  Conjugate Acids and Bases
38.4.2.1.  Conjugate acid/base pairs
38.4.2.2.   Identifying in acid base reactions
38.5.   Strength of Acids
38.5.1.  Strong Acids
38.5.2.  Weak Acids
38.5.3.  Strong Bases
38.5.4.  Weak Bases
38.6.   Amphiprotic Water
38.6.1.  Kw
38.7.   pH
38.7.1.  Calculations of pH
38.7.2.  Calculations of [H3O+]
38.7.3.  Calculations of pOJ
38.7.4.  Calculations of [OH-]
38.7.5.  pH Scale
38.7.5.1. Calculations
38.8.    Buffers
38.8.1.  Definitions
38.8.2.  Examples
38.9.     Ka
38.9.1.  Writing Expressions