普通化學

1.1 Classical Physics Does Not Adequately Describe the Interaction of Light with Matter1.2 The Bohr Model Was an Early Attempt to Formulate a Quantum Theory of Matter

1.1 Classical Physics Does Not Adequately Describe the Interaction of Light with Matter1.2 The Bohr Model Was an Early Attempt to Formulate a Quantum Theory of Matter

1.3 Matter Has Wavelike Properties 1.4 The Hydrogen Atom Is an Exactly Solvable Quantum- Mechanical System

1.3 Matter Has Wavelike Properties 1.4 The Hydrogen Atom Is an Exactly Solvable Quantum- Mechanical System

2.1 The Wavefunctions of Many-Electron Atoms Can Be Described to a Good Approximation Using Atomic Orbitals 2.2 Electron Configurations of Many-Electron Atoms Are Constructed Using the Aufbau (or ”Building-up”) Principle 2.3 The Periodic Table Predates Quantum Mechanics2.4 Elements Can Be Classified by Their Position in the Periodic Table

2.1 The Wavefunctions of Many-Electron Atoms Can Be Described to a Good Approximation Using Atomic Orbitals 2.2 Electron Configurations of Many-Electron Atoms Are Constructed Using the Aufbau (or ”Building-up”) Principle 2.3 The Periodic Table Predates Quantum Mechanics2.4 Elements Can Be Classified by Their Position in the Periodic Table

2.5 The Properties of the Elements Vary Periodically Across the Periodic Table3.1 Atoms in a Molecule Are Held Together by Chemical Bonds3.2 A Covalent Bond Involves the Sharing of Electrons Between Atoms in a Molecule

2.5 The Properties of the Elements Vary Periodically Across the Periodic Table3.1 Atoms in a Molecule Are Held Together by Chemical Bonds3.2 A Covalent Bond Involves the Sharing of Electrons Between Atoms in a Molecule

3.3 Electronegativity Differences Determine the Polarity of Chemical Bonds 3.4 Drawing Correct Lewis Structures Is an Invaluable Skill for a Chemist

3.3 Electronegativity Differences Determine the Polarity of Chemical Bonds 3.4 Drawing Correct Lewis Structures Is an Invaluable Skill for a Chemist

3.4 Drawing Correct Lewis Structures Is an Invaluable Skill for a Chemist 3.5 Molecular Orbital Theory Provides a Detailed Description of Chemical Bonding

3.4 Drawing Correct Lewis Structures Is an Invaluable Skill for a Chemist 3.5 Molecular Orbital Theory Provides a Detailed Description of Chemical Bonding

3.5 Molecular Orbital Theory Provides a Detailed Description of Chemical Bonding 4.1 The Basic Three-Dimensional Structure of a Molecule Can Be Predicted Using the VSEPR Model

3.5 Molecular Orbital Theory Provides a Detailed Description of Chemical Bonding 4.1 The Basic Three-Dimensional Structure of a Molecule Can Be Predicted Using the VSEPR Model

4.1 The Basic Three-Dimensional Structure of a Molecule Can Be Predicted Using the VSEPR Model4.2 The Polarity of a Molecule Can Be Described Quantitatively by Its Dipole Moment

4.1 The Basic Three-Dimensional Structure of a Molecule Can Be Predicted Using the VSEPR Model4.2 The Polarity of a Molecule Can Be Described Quantitatively by Its Dipole Moment

Midterm Exam

Midterm Exam

4.3 Valence Bond Theory for Polyatomic Molecules Requires the Use of Hybrid Orbitals4.4 Isomers Are Compounds That Have the Same Molecular Formula but Different Atomic Arrangements

4.3 Valence Bond Theory for Polyatomic Molecules Requires the Use of Hybrid Orbitals4.4 Isomers Are Compounds That Have the Same Molecular Formula but Different Atomic Arrangements

4.5 Bonding in Polyatomic Molecules Can Be Explained Using Molecular Orbitals4.6 The Interactions Between Molecules Greatly Affect the Bulk Properties of Materials

4.5 Bonding in Polyatomic Molecules Can Be Explained Using Molecular Orbitals4.6 The Interactions Between Molecules Greatly Affect the Bulk Properties of Materials

5.1 Pressure and Temperature Are Two Important Macroscopic Properties of Chemical Systems5.2 Substances and Mixtures Can Exist as Solid, Liquid, or Gas, Depending upon the External Conditions 5.3 The Ideal-Gas Equation Describes the Behavior of All Gases in the Limit of Low Pressure

5.1 Pressure and Temperature Are Two Important Macroscopic Properties of Chemical Systems5.2 Substances and Mixtures Can Exist as Solid, Liquid, or Gas, Depending upon the External Conditions 5.3 The Ideal-Gas Equation Describes the Behavior of All Gases in the Limit of Low Pressure

5.3 The Ideal-Gas Equation Describes the Behavior of All Gases in the Limit of Low Pressure5.4 The Kinetic Theory of Gases Provides a Molecular Explanation for the Behavior of Gases5.5 Real Gases Exhibit Deviations from Ideal Behavior at High Pressures

5.3 The Ideal-Gas Equation Describes the Behavior of All Gases in the Limit of Low Pressure5.4 The Kinetic Theory of Gases Provides a Molecular Explanation for the Behavior of Gases5.5 Real Gases Exhibit Deviations from Ideal Behavior at High Pressures

6.1 The Structure and Properties of Liquids Are Governed by Intermolecular Interactions6.2 Crystalline Solids Can Be Classified in Terms of Their Structure and Intermolecular Interactions

6.1 The Structure and Properties of Liquids Are Governed by Intermolecular Interactions6.2 Crystalline Solids Can Be Classified in Terms of Their Structure and Intermolecular Interactions

6.3 The Properties of Crystalline Solids Are Determined Largely by Intermolecular Interactions6.4 Band Theory Accurately Explains the Conductivity of Metals, Semiconductors, and Insulators7.1 Thermodynamics Is the Study of Energy and Its Transformations in Macroscopic Systems

6.3 The Properties of Crystalline Solids Are Determined Largely by Intermolecular Interactions6.4 Band Theory Accurately Explains the Conductivity of Metals, Semiconductors, and Insulators7.1 Thermodynamics Is the Study of Energy and Its Transformations in Macroscopic Systems

7.2 The Energy Absorbed by a System as Heat in a Constant-Pressure Process Is Equal to the Change in Enthalpy7.3 The Temperature Change of a System upon Heating Is Governed by Its Heat Capacity7.4 The Enthalpy Changes for any Reaction Can Be Calculated Using Standard Enthalpies of Formation

7.2 The Energy Absorbed by a System as Heat in a Constant-Pressure Process Is Equal to the Change in Enthalpy7.3 The Temperature Change of a System upon Heating Is Governed by Its Heat Capacity7.4 The Enthalpy Changes for any Reaction Can Be Calculated Using Standard Enthalpies of Formation

7.5 The Reaction Enthalpies Can Be Estimated from Bond Enthalpies7.6 Enthalpy Changes Also Accompany Physical Transformations7.7 The Temperature Dependence of Reaction Enthalpies Can Be Determined from Heat Capacity Data

7.5 The Reaction Enthalpies Can Be Estimated from Bond Enthalpies7.6 Enthalpy Changes Also Accompany Physical Transformations7.7 The Temperature Dependence of Reaction Enthalpies Can Be Determined from Heat Capacity Data

Final Exam

Final Exam