Search this site
Embedded Files
Skip to main content
Skip to navigation
APChemwins
AP Chemistry Home
Lab Manual
Objectives
Resources
Summer Work
Summer Work 2013
10.1 Intermolecular Forces
14.1 The Nature of Acids and Bases
7.1 Electromagnetic Radiation
7.13 The Properties of a Group: The Alkali Metals
Calendar
Calendar Per 4/5
Calendar Per 6/5
Calendar 2013-2014
Calendar 2014-2015
Ch 01
1.1 Chemistry: An Overview
1.2 The Scientific Method
1.3 Units of Measurement
1.4 Uncertainty in Measurement
1.5 Significant Figures and Calculations
1.6 Dimensional Analysis
1.7 Temperature
1.8 Density
1.9 Classification of Matter
Ch 1 Blog
Caffeine Molecule
Significant figures
Ch 02
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
2.3 Dalton's Atomic Theory
2.4 Early Experiments to Charachterize the Atom
2.5 The Modern View of Atomic Structure: An Introduction
2.6 Molecules and Ions
2.7 An Introduction to the Periodic Table
2.8 Naming Simple Compounds
Ch 03
3.1 Counting by Weighing
3.10 Stoichiometric Calculations
3.11 The Concept of Limiting Reagent
3.2 Atomic Masses
3.3 The Mole
3.4 Molar Masses
3.5 Learning to Solve Problems
3.6 Percent Composition of Compounds
3.7 Determining the Formula of a Compound
3.8 Chemical Equations
3.9 Balancing Chemical Equations
Ch 04
4.1 Water Common Solvent
4.10 Balancing Oxidation Reduction Reactions
4.2 The Nature of Aqueous Solutions
4.3 The Composition of Solutions
4.4 Types of Chemical Reactions
4.5 Precipitation Reactions
4.6 Describing Reactions in Solutions
4.7 Stoichiometry of Precipitation Reactions
4.8 Acid-Base Reactions
4.9 Oxidation-Reduction Reactions
Ch 05
5.1 Pressure
5.2 Gas Laws of Boyle, Charles, & Avogadro
5.3 The Ideal Gas Law
5.4 Gas Stoichiometry
5.5 Dalton's Law of Partial Pressure
5.6 The Kinetic Molecular Theory of Gases
5.7 Effusion and Diffusion
5.8 Real Gases
5.9 Characteristics of Several Real Gases
Ch 06
6.1 The Nature of Energy
6.2 Enthalpy and Calorimetry
6.3 Hess's Law
6.4 Standard Enthalpies of Formation
6.5 Present Sources of Energy
6.6 New Energy Sources
Ch 07
7.1 Electromagnetic Radiation
7.10 The History of the Periodic Table
7.11 The Aufbau Principle and The Periodic Table
7.12 Periodic Trends in the Atomic Properties
7.13 The Properties of a Group: The Alkali Metals
7.2 The Nature of Matter
7.3 The Atomic Spectrum of Hydrogen
7.4 The Bohr Model
7.5 The Quantum Mechanical Model of the Atom
7.6 Quantum Numbers
7.7 Orbital Shapes and Energies
7.8 Electron Spin and the Pauli Principle
7.9 Polyelectronic Atoms
Ch 08
8.1 Types of Chemical Bonds
8.10 Lewis Structures
8.11 Exceptions to the Octet Rule
8.12 Resonance
8.13 Molecular Structure: The VSEPR Model
8.2 Electronegativity
8.3 Bond Polarity and Dipole Moments
8.4 Ions: Electron Configurations and Sizes
8.5 Energy Effects in Binary Ionic Compounds
8.6 Partial Ionic Character of Covalent Bonds
8.7 The Covalent Chemical Bond: A Model
8.8 Types of Chemical Bonds
8.9 The Localized Electron Bonding Model
Ch 09
9.1 Hybridization & Localized Electron Model
9.2 The Molecular Orbital Model
9.3 Bonding in Homonuclear Diatomic Molecules
9.4 Bonding in Heteronuclear Diatomic Molecules
9.5 Combining the Localized Electron and molecular Orbital Models
Ch 10
Ch 10
10.1 Intermolecular Forces
10.2 The Liquid State
10.3 Intro to the Structures & Types of Solids
10.4 Structure and Bonding in Metals
10.5 Carbon and Silicon: Network Atomic Solids
10.6 Molecular Solids
10.7 Ionic Solids
10.8 Vapor Pressure and Changes of State
10.9 Phase Diagrams
Ch 11
11.1 Solution Composition
11.2 The Energies of Solution Formation
11.3 Factors Affecting Solubility
11.4 The Vapor Pressure of Solutions
11.5 Boiling-Point Elevation and Freezing-Point Depression
11.6 Osmotic Pressure
11.7 Colligative Properties of Electrolyte Solutions
11.8 Colloids
Ch 12
12.1 Reaction Rates
12.2 Rate Laws: an Introduction
12.3 Determining the Form of the Rate Law
12.4 The Integrated Rate Law
12.5 Reaction Mechanisms
12.6 A Model for Chemical Kinetics
12.7 Catalysis
Ch 13
13.1 The Equilibrium Condition
13.2 The Equilibrium Constant
13.3 Equilibrium Expressions Involving Pressures
13.4 Heterogeneous Equilibria
13.5 Applications of the Equilibrium Constant
13.6 Solving Equilibrium Problems
13.7 Le Chateliers Principle
Ch 14
14.1 The Nature of Acids and Bases
14.1 The Nature of Acids and Bases
14.10 Acid-Base Properties of Oxides
14.11 The Lewis Acid-Base Model
14.12 Strategy for Solving Acid-Base Problems
14.2 Acid Strength
14.2 Acid Strength
14.3 The pH Scale
14.4 Calculating the pH of Strong Acid Solutions
14.5 Calculating the pH of Weak Acid Solutions
14.6 Bases
14.7 Polyprotic Acids
14.8 Acid-Base Properties
14.9 The Effect of Structure on Acid-Base Properties
Ch 15
15.1 Solutionsof Acids or Bases Containing a Common Ion
15.2 Buffered Solutions
15.3 Buffering Capacity
Ch 16
Ch 17
17.1 Spontaneous Processes and Entropy
17.2 Entropy and the Second Law of Thermodynamics
17.3 The Effect of Temperature on Spontaneity
17.4 Free Energy
17.5 Entropy Changes in Chemical Reactions
17.6 Free Energy and Chemical Reactions
17.7 The Dependence of Free Energy on Pressure
17.8 Free Energy and Equilibrium
17.9 Free Energy and Work
Ch 18
18.1 Balancing Oxidation-Reduction Equations
18.2 Galvanic Cells
18.3 Standard Reduction Potentials
18.4 Cell Potential, Electrical Work, and Free Energy
18.5 Dependence of Cell Potential on Concentration
18.6 Batteries
18.7 Corrosion
18.8 Electrolysis
18.9 Commercial Electrolytic Processes
Chapter Objectives
Summer Work 2021
Unit 1 Concepts
Ch 1 Chemical Foundations
Ch 2 Atoms, Molecules and Ions
Unit 2 Bonding
Unit 3 Reactions
Unit 4 Condensed States
Unit 5 Equilibrium
Unit 6 Thermodynamics
Unit 7 Topics
APChemwins
AP Chemistry Home
Lab Manual
Objectives
Resources
Summer Work
Summer Work 2013
10.1 Intermolecular Forces
14.1 The Nature of Acids and Bases
7.1 Electromagnetic Radiation
7.13 The Properties of a Group: The Alkali Metals
Calendar
Calendar Per 4/5
Calendar Per 6/5
Calendar 2013-2014
Calendar 2014-2015
Ch 01
1.1 Chemistry: An Overview
1.2 The Scientific Method
1.3 Units of Measurement
1.4 Uncertainty in Measurement
1.5 Significant Figures and Calculations
1.6 Dimensional Analysis
1.7 Temperature
1.8 Density
1.9 Classification of Matter
Ch 1 Blog
Caffeine Molecule
Significant figures
Ch 02
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
2.3 Dalton's Atomic Theory
2.4 Early Experiments to Charachterize the Atom
2.5 The Modern View of Atomic Structure: An Introduction
2.6 Molecules and Ions
2.7 An Introduction to the Periodic Table
2.8 Naming Simple Compounds
Ch 03
3.1 Counting by Weighing
3.10 Stoichiometric Calculations
3.11 The Concept of Limiting Reagent
3.2 Atomic Masses
3.3 The Mole
3.4 Molar Masses
3.5 Learning to Solve Problems
3.6 Percent Composition of Compounds
3.7 Determining the Formula of a Compound
3.8 Chemical Equations
3.9 Balancing Chemical Equations
Ch 04
4.1 Water Common Solvent
4.10 Balancing Oxidation Reduction Reactions
4.2 The Nature of Aqueous Solutions
4.3 The Composition of Solutions
4.4 Types of Chemical Reactions
4.5 Precipitation Reactions
4.6 Describing Reactions in Solutions
4.7 Stoichiometry of Precipitation Reactions
4.8 Acid-Base Reactions
4.9 Oxidation-Reduction Reactions
Ch 05
5.1 Pressure
5.2 Gas Laws of Boyle, Charles, & Avogadro
5.3 The Ideal Gas Law
5.4 Gas Stoichiometry
5.5 Dalton's Law of Partial Pressure
5.6 The Kinetic Molecular Theory of Gases
5.7 Effusion and Diffusion
5.8 Real Gases
5.9 Characteristics of Several Real Gases
Ch 06
6.1 The Nature of Energy
6.2 Enthalpy and Calorimetry
6.3 Hess's Law
6.4 Standard Enthalpies of Formation
6.5 Present Sources of Energy
6.6 New Energy Sources
Ch 07
7.1 Electromagnetic Radiation
7.10 The History of the Periodic Table
7.11 The Aufbau Principle and The Periodic Table
7.12 Periodic Trends in the Atomic Properties
7.13 The Properties of a Group: The Alkali Metals
7.2 The Nature of Matter
7.3 The Atomic Spectrum of Hydrogen
7.4 The Bohr Model
7.5 The Quantum Mechanical Model of the Atom
7.6 Quantum Numbers
7.7 Orbital Shapes and Energies
7.8 Electron Spin and the Pauli Principle
7.9 Polyelectronic Atoms
Ch 08
8.1 Types of Chemical Bonds
8.10 Lewis Structures
8.11 Exceptions to the Octet Rule
8.12 Resonance
8.13 Molecular Structure: The VSEPR Model
8.2 Electronegativity
8.3 Bond Polarity and Dipole Moments
8.4 Ions: Electron Configurations and Sizes
8.5 Energy Effects in Binary Ionic Compounds
8.6 Partial Ionic Character of Covalent Bonds
8.7 The Covalent Chemical Bond: A Model
8.8 Types of Chemical Bonds
8.9 The Localized Electron Bonding Model
Ch 09
9.1 Hybridization & Localized Electron Model
9.2 The Molecular Orbital Model
9.3 Bonding in Homonuclear Diatomic Molecules
9.4 Bonding in Heteronuclear Diatomic Molecules
9.5 Combining the Localized Electron and molecular Orbital Models
Ch 10
Ch 10
10.1 Intermolecular Forces
10.2 The Liquid State
10.3 Intro to the Structures & Types of Solids
10.4 Structure and Bonding in Metals
10.5 Carbon and Silicon: Network Atomic Solids
10.6 Molecular Solids
10.7 Ionic Solids
10.8 Vapor Pressure and Changes of State
10.9 Phase Diagrams
Ch 11
11.1 Solution Composition
11.2 The Energies of Solution Formation
11.3 Factors Affecting Solubility
11.4 The Vapor Pressure of Solutions
11.5 Boiling-Point Elevation and Freezing-Point Depression
11.6 Osmotic Pressure
11.7 Colligative Properties of Electrolyte Solutions
11.8 Colloids
Ch 12
12.1 Reaction Rates
12.2 Rate Laws: an Introduction
12.3 Determining the Form of the Rate Law
12.4 The Integrated Rate Law
12.5 Reaction Mechanisms
12.6 A Model for Chemical Kinetics
12.7 Catalysis
Ch 13
13.1 The Equilibrium Condition
13.2 The Equilibrium Constant
13.3 Equilibrium Expressions Involving Pressures
13.4 Heterogeneous Equilibria
13.5 Applications of the Equilibrium Constant
13.6 Solving Equilibrium Problems
13.7 Le Chateliers Principle
Ch 14
14.1 The Nature of Acids and Bases
14.1 The Nature of Acids and Bases
14.10 Acid-Base Properties of Oxides
14.11 The Lewis Acid-Base Model
14.12 Strategy for Solving Acid-Base Problems
14.2 Acid Strength
14.2 Acid Strength
14.3 The pH Scale
14.4 Calculating the pH of Strong Acid Solutions
14.5 Calculating the pH of Weak Acid Solutions
14.6 Bases
14.7 Polyprotic Acids
14.8 Acid-Base Properties
14.9 The Effect of Structure on Acid-Base Properties
Ch 15
15.1 Solutionsof Acids or Bases Containing a Common Ion
15.2 Buffered Solutions
15.3 Buffering Capacity
Ch 16
Ch 17
17.1 Spontaneous Processes and Entropy
17.2 Entropy and the Second Law of Thermodynamics
17.3 The Effect of Temperature on Spontaneity
17.4 Free Energy
17.5 Entropy Changes in Chemical Reactions
17.6 Free Energy and Chemical Reactions
17.7 The Dependence of Free Energy on Pressure
17.8 Free Energy and Equilibrium
17.9 Free Energy and Work
Ch 18
18.1 Balancing Oxidation-Reduction Equations
18.2 Galvanic Cells
18.3 Standard Reduction Potentials
18.4 Cell Potential, Electrical Work, and Free Energy
18.5 Dependence of Cell Potential on Concentration
18.6 Batteries
18.7 Corrosion
18.8 Electrolysis
18.9 Commercial Electrolytic Processes
Chapter Objectives
Summer Work 2021
Unit 1 Concepts
Ch 1 Chemical Foundations
Ch 2 Atoms, Molecules and Ions
Unit 2 Bonding
Unit 3 Reactions
Unit 4 Condensed States
Unit 5 Equilibrium
Unit 6 Thermodynamics
Unit 7 Topics
More
AP Chemistry Home
Lab Manual
Objectives
Resources
Summer Work
Summer Work 2013
10.1 Intermolecular Forces
14.1 The Nature of Acids and Bases
7.1 Electromagnetic Radiation
7.13 The Properties of a Group: The Alkali Metals
Calendar
Calendar Per 4/5
Calendar Per 6/5
Calendar 2013-2014
Calendar 2014-2015
Ch 01
1.1 Chemistry: An Overview
1.2 The Scientific Method
1.3 Units of Measurement
1.4 Uncertainty in Measurement
1.5 Significant Figures and Calculations
1.6 Dimensional Analysis
1.7 Temperature
1.8 Density
1.9 Classification of Matter
Ch 1 Blog
Caffeine Molecule
Significant figures
Ch 02
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
2.3 Dalton's Atomic Theory
2.4 Early Experiments to Charachterize the Atom
2.5 The Modern View of Atomic Structure: An Introduction
2.6 Molecules and Ions
2.7 An Introduction to the Periodic Table
2.8 Naming Simple Compounds
Ch 03
3.1 Counting by Weighing
3.10 Stoichiometric Calculations
3.11 The Concept of Limiting Reagent
3.2 Atomic Masses
3.3 The Mole
3.4 Molar Masses
3.5 Learning to Solve Problems
3.6 Percent Composition of Compounds
3.7 Determining the Formula of a Compound
3.8 Chemical Equations
3.9 Balancing Chemical Equations
Ch 04
4.1 Water Common Solvent
4.10 Balancing Oxidation Reduction Reactions
4.2 The Nature of Aqueous Solutions
4.3 The Composition of Solutions
4.4 Types of Chemical Reactions
4.5 Precipitation Reactions
4.6 Describing Reactions in Solutions
4.7 Stoichiometry of Precipitation Reactions
4.8 Acid-Base Reactions
4.9 Oxidation-Reduction Reactions
Ch 05
5.1 Pressure
5.2 Gas Laws of Boyle, Charles, & Avogadro
5.3 The Ideal Gas Law
5.4 Gas Stoichiometry
5.5 Dalton's Law of Partial Pressure
5.6 The Kinetic Molecular Theory of Gases
5.7 Effusion and Diffusion
5.8 Real Gases
5.9 Characteristics of Several Real Gases
Ch 06
6.1 The Nature of Energy
6.2 Enthalpy and Calorimetry
6.3 Hess's Law
6.4 Standard Enthalpies of Formation
6.5 Present Sources of Energy
6.6 New Energy Sources
Ch 07
7.1 Electromagnetic Radiation
7.10 The History of the Periodic Table
7.11 The Aufbau Principle and The Periodic Table
7.12 Periodic Trends in the Atomic Properties
7.13 The Properties of a Group: The Alkali Metals
7.2 The Nature of Matter
7.3 The Atomic Spectrum of Hydrogen
7.4 The Bohr Model
7.5 The Quantum Mechanical Model of the Atom
7.6 Quantum Numbers
7.7 Orbital Shapes and Energies
7.8 Electron Spin and the Pauli Principle
7.9 Polyelectronic Atoms
Ch 08
8.1 Types of Chemical Bonds
8.10 Lewis Structures
8.11 Exceptions to the Octet Rule
8.12 Resonance
8.13 Molecular Structure: The VSEPR Model
8.2 Electronegativity
8.3 Bond Polarity and Dipole Moments
8.4 Ions: Electron Configurations and Sizes
8.5 Energy Effects in Binary Ionic Compounds
8.6 Partial Ionic Character of Covalent Bonds
8.7 The Covalent Chemical Bond: A Model
8.8 Types of Chemical Bonds
8.9 The Localized Electron Bonding Model
Ch 09
9.1 Hybridization & Localized Electron Model
9.2 The Molecular Orbital Model
9.3 Bonding in Homonuclear Diatomic Molecules
9.4 Bonding in Heteronuclear Diatomic Molecules
9.5 Combining the Localized Electron and molecular Orbital Models
Ch 10
Ch 10
10.1 Intermolecular Forces
10.2 The Liquid State
10.3 Intro to the Structures & Types of Solids
10.4 Structure and Bonding in Metals
10.5 Carbon and Silicon: Network Atomic Solids
10.6 Molecular Solids
10.7 Ionic Solids
10.8 Vapor Pressure and Changes of State
10.9 Phase Diagrams
Ch 11
11.1 Solution Composition
11.2 The Energies of Solution Formation
11.3 Factors Affecting Solubility
11.4 The Vapor Pressure of Solutions
11.5 Boiling-Point Elevation and Freezing-Point Depression
11.6 Osmotic Pressure
11.7 Colligative Properties of Electrolyte Solutions
11.8 Colloids
Ch 12
12.1 Reaction Rates
12.2 Rate Laws: an Introduction
12.3 Determining the Form of the Rate Law
12.4 The Integrated Rate Law
12.5 Reaction Mechanisms
12.6 A Model for Chemical Kinetics
12.7 Catalysis
Ch 13
13.1 The Equilibrium Condition
13.2 The Equilibrium Constant
13.3 Equilibrium Expressions Involving Pressures
13.4 Heterogeneous Equilibria
13.5 Applications of the Equilibrium Constant
13.6 Solving Equilibrium Problems
13.7 Le Chateliers Principle
Ch 14
14.1 The Nature of Acids and Bases
14.1 The Nature of Acids and Bases
14.10 Acid-Base Properties of Oxides
14.11 The Lewis Acid-Base Model
14.12 Strategy for Solving Acid-Base Problems
14.2 Acid Strength
14.2 Acid Strength
14.3 The pH Scale
14.4 Calculating the pH of Strong Acid Solutions
14.5 Calculating the pH of Weak Acid Solutions
14.6 Bases
14.7 Polyprotic Acids
14.8 Acid-Base Properties
14.9 The Effect of Structure on Acid-Base Properties
Ch 15
15.1 Solutionsof Acids or Bases Containing a Common Ion
15.2 Buffered Solutions
15.3 Buffering Capacity
Ch 16
Ch 17
17.1 Spontaneous Processes and Entropy
17.2 Entropy and the Second Law of Thermodynamics
17.3 The Effect of Temperature on Spontaneity
17.4 Free Energy
17.5 Entropy Changes in Chemical Reactions
17.6 Free Energy and Chemical Reactions
17.7 The Dependence of Free Energy on Pressure
17.8 Free Energy and Equilibrium
17.9 Free Energy and Work
Ch 18
18.1 Balancing Oxidation-Reduction Equations
18.2 Galvanic Cells
18.3 Standard Reduction Potentials
18.4 Cell Potential, Electrical Work, and Free Energy
18.5 Dependence of Cell Potential on Concentration
18.6 Batteries
18.7 Corrosion
18.8 Electrolysis
18.9 Commercial Electrolytic Processes
Chapter Objectives
Summer Work 2021
Unit 1 Concepts
Ch 1 Chemical Foundations
Ch 2 Atoms, Molecules and Ions
Unit 2 Bonding
Unit 3 Reactions
Unit 4 Condensed States
Unit 5 Equilibrium
Unit 6 Thermodynamics
Unit 7 Topics
9.4 Bonding in Heteronuclear Diatomic Molecules
Objectives
: describe the bonding in heteronuclear diatomic molecules
Google Sites
Report abuse
Page details
Page updated
Google Sites
Report abuse
