Irvington High School  AP Chemistry
Mr. Markic
Name _________________________________
Number ___ Date ___/___/___
Mid-Term Review
[Keep
1.
Chapter 1 – Introduction: Matter and
3.
Measurement
a.
b.
Properties of Matter

Physical and Chemical Changes
c.
Units of Measurement

SI Units

Length and Mass

Temperature

Derived SI Units

Volume

Density
d.
e.
2.
Classifications of Matter

States of Matter

Pure Substances and Mixtures

Separation of Mixtures

Elements

Compounds
Uncertainty in Measurement

Significant Figures

Significant Figures in Calculations
Dimensional Analysis

Using Two or More Conversion Factors
Chapter 2 – Atoms, Molecules, and Ions
a. The Atomic Theory of Matter
b.
The Discovery of the Atomic Structure

Cathode Rays and Electrons

Radioactivity

The Nuclear Atom
c.
The Modern View of Atomic Structure

Isotopes

Atomic Numbers

Mass Numbers
4.
Chapter 3 – Mass Relationships in Chemical Equations
a. Chemical Equations
b.
Patterns of Chemical Reactivity

Using the Periodic Table

Combustion in Air

Combination and Decomposition Reactions
c.
Atomic and Molecular Weights

The Atomic Mass Scale

Average Atomic Masses

Formula and Molecular Weights

Percentage Composition from Formulas
d.
The Mole

Molar Mass

Interconverting Masses, Moles, Number of
Particles, and Volume
e.
Empirical Formulas from Analyses

Molecular Formula from Empirical Formula

Combustion Analysis
f.
Quantitative Information from Balanced Equations
g.
Limiting Reactants

Theoretical Yields
Chapter 4 – Reactions in Aqueous Solutions
a. General Properties of Aqueous Solutions

Electrolytic Properties

Ionic Compounds in Water

Molecular Compounds in Water

Strong and Weak Electrolytes
b.
d.
The Periodic Table
e.
Molecules and Molecular Compounds

Molecules and Molecular Formulas

Molecular and Empirical Formulas
f.
Ions and Ionic Compounds

Predicting Ionic Charges

Ionic Compounds
g.
Naming Inorganic Compounds

Names and Formulas of Ionic Compounds

Names and Formulas of Acids

Names and Formulas of Binary Molecular
Compounds
AP Chemistry
Mr. Markic
for Reference]
c.
Precipitation Reactions

Solubility Guidelines for Ionic Compounds

Exchange (Metathesis) Reactions

Ionic equations
Acid-Base Reactions

Acids

Bases

Strong and Weak Acids and Bases

Identifying Strong and Weak Electrolytes

Neutralization Reactions and Salts

Acid-Base Reactions with Gas Formation
d.
Oxidation-Reduction Reactions

Oxidation and Reduction

Oxidation Numbers

Oxidation of Metals by Acids and Salts

The Activity Series
e.
Concentration of Solutions

Molarity

Expressing the Concentration of an Electrolyte

Interconverting Molarity, Moles, and Volume
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
Dilution
7.
f.
5.
Chapter 5– Gases
a. Characteristics of Gases
b.
c.
d.
e.
f.
6.
Solution Stoichiometry and Chemical Analysis

Titrations
Pressure

Atmospheric Pressure and the Barometer

Pressures of enclosed Gases and Manometers
The Gas Laws

The Pressure-Volume Relationship: Boyle’s Law

The Temperature-Volume Relationship: Charles’s
Law

The Quantity-Volume Relationship: Avogadro’s
Law
The Ideal-Gas Equation

Relating the Ideal-Gas Equation and the Gas
Laws
Chapter 7 – Electronic Structure of Atoms
a. The Wave Nature of Light
b.
Quantized Energy and Photons

The Photoelectric Effect
c.
Bohr’s Model of the Hydrogen Atom

Line Spectra

Bohr’s Model
d.
The Wave Behavior of Matter

The Uncertainty Principle
e.
Quantum Mechanics and Atomic Orbitals

Orbitals and Quantum Numbers
f.
Representations of Orbitals

The s Orbitals

The p Orbitals

The d and f Orbitals
Orbitals in Many-Electron Atoms

Effective Nuclear Charge

Energies of Orbitals

Electron Spin and the Pauli exclusion Principle
g.
Further Applications of the Ideal-Gas Equation

Gas Densities and Molar Mass

Volumes of Gases in Chemical Reactions
h.
Gas Mixtures and Partial Pressures

Partial Pressures and Mole Fractions

Collecting Gases Over Water
Electron Configurations

Periods 1, 2, and 3

Period 4 and Beyond
i.
Electron Configurations and the Periodic Table
g.
Kinetic-Molecular Theory

Application to the Gas Laws
8.
h.
Molecular Effusion and Diffusion

Graham’s Law of Effusion

Diffusion and Mean Free Path
b.
Electron Shells and the Sizes of Atoms

Electron Shells in Atoms

Atomic Sizes
i.
Real Gases: Deviations from Ideal Behavior

The van der Waals Equation
c.
Ionization Energy

Periodic Trends in Ionization Energies
d.
Electron Affinities
e.
Metals, Nonmetals, and Metalloids

Metals

Nonmetals

Metalloids
f.
Group Trends for the Active Metals

The Alkali Metals

The Alkaline Earth Metals
g.
Group Trends for Selected Nonmetals

Hydrogen

Group 6A: Chalcogens

The Halogens

The Noble Gases
Chapter 6 – Thermochemistry
a. The Nature of Energy

Kinetic Energy and Potential Energy

Units of Energy

System and Surroundings
b.
The First Law of Thermodynamics

Internal Energy

Endothermic and Exothermic Processes

State Functions
c.
Enthalpy
d.
Enthalpies of Reaction
e.
Calorimetry

Heat Capacity and Specific Heat
f.
Hess’s Law
g.
Enthalpies of Formation

Using Enthalpies of Formation to Calculate
Enthalpies of Reaction
9.
AP Chemistry
Mr. Markic
Chapter 8 – Periodic Properties of the Elements
a. Development of the Periodic Table
Chapter 9 – Basic Concepts of Chemical Bonding
a. Chemical Bonds, Lewis Symbols, and the Octet Rule

Lewis Symbols

The Octet Rule
b.
Ionic Bonding
Page 2 of 3


c.
Energies of Ionic Bond Formation
Electron Configuration of Ions of the
Representative Elements

Transition – Metal ions

Polyatomic Ions
Sizes of Ions
d.
Covalent Bonding

Lewis Structures

Multiple Bonds
e.
Bond Polarity and Electronegativity

Electronegativity

Electronegativity and Bond Polarity

Dipole Moments

Bond Types and Nomenclature
f.
Drawing Lewis Structures

Formal Charge
g.
Resonance Structures

Resonance in Benzene
h.
Exceptions to the Octet Rule

Odd Number of Electrons

Less than an Octet

More than an Octet
i.
Strengths of Covalent Bonds

Bond Enthalpies and the Enthalpies of Reactions

Bond Enthalpy and Bond Length
10. Chapter 10 – Molecular Geometry
a. Molecular Shapes
b.
c.
The VSEPR Model

The Effect of Nonbonding Electrons and Multiple
Bonds on Bond Angles

Molecules with Expanded Valence Shells

Molecules with more than One Central Atom
Polarity and Polyatomic Ions
d.
Covalent Bonding and Orbital Overlap
e.
Hybrid Orbitals

sp Hybrid Orbitals

sp2 and sp3 Hybrid Orbitals

Hybridization Involving d Orbitals
f.
Multiple Bonds

Delocalized  Bonding
g.
Molecular Orbitals

The Hydrogen Molecule
11.
a.
Chapter 11- IMF’s of Liquids and Solids
Intermolecular Forces

London dispersion forces

Dipole-dipole forces

Hydrogen bonding

Surface tension

Network covalent bonds

Metallic bonds

Phase diagrams

Phase changes
AP Chemistry
Mr. Markic
Page 3 of 3