Sacramento City College
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- SCC: CHEM 300 - Beginning Chemistry
- SCC: CHEM 300 - Beginning Chemistry (Alviar-Agnew)
- 1: The Chemical World
- 2: Measurement and Problem Solving
- 2.1: Taking Measurements
- 2.2: Scientific Notation - Writing Large and Small Numbers
- 2.3: Significant Figures - Writing Numbers to Reflect Precision
- 2.4: Significant Figures in Calculations
- 2.5: The Basic Units of Measurement
- 2.6: Problem Solving and Unit Conversions
- 2.7: Solving Multistep Conversion Problems
- 2.8: Units Raised to a Power
- 2.9: Density
- 2.E: Measurement and Problem Solving (Exercises)
- 3: Matter and Energy
- 3.1: In Your Room
- 3.2: What is Matter?
- 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas
- 3.4: Classifying Matter According to Its Composition
- 3.5: Differences in Matter: Physical and Chemical Properties
- 3.6: Changes in Matter: Physical and Chemical Changes
- 3.7: Conservation of Mass: There is No New Matter
- 3.8: Energy
- 3.9: Energy and Chemical and Physical Change
- 3.10: Temperature: Random Motion of Molecules and Atoms
- 3.11: Temperature Changes: Heat Capacity
- 3.12: Energy and Heat Capacity Calculations
- 3.E: Exercises
- 4: Atoms and Elements
- 4.1: Experiencing Atoms at Tiburon
- 4.2: Indivisible: The Atomic Theory
- 4.3: The Nuclear Atom
- 4.4: The Properties of Protons, Neutrons, and Electrons
- 4.5: Elements: Defined by Their Numbers of Protons
- 4.6: Looking for Patterns: The Periodic Law and the Periodic Table
- 4.7: Ions: Losing and Gaining Electrons
- 4.8: Isotopes: When the Number of Neutrons Varies
- 4.9: Atomic Mass: The Average Mass of an Element’s Atoms
- 5: Molecules and Compounds
- 5.1: Sugar and Salt
- 5.2: Compounds Display Constant Composition
- 5.3: Chemical Formulas: How to Represent Compounds
- 5.4: A Molecular View of Elements and Compounds
- 5.5: Writing Formulas for Ionic Compounds
- 5.6: Nomenclature n- Naming Compounds
- 5.7: Naming Ionic Compounds
- 5.8: Naming Molecular Compounds
- 5.9: Naming Acids
- 5.10: Nomenclature Summary
- 5.11: Formula Mass: The Mass of a Molecule or Formula Unit
- 6: Chemical Composition
- 6.1: How Much Sodium?
- 6.2: Counting Nails by the Pound
- 6.3: Counting Atoms by the Gram
- 6.4: Counting Molecules by the Gram
- 6.5: Chemical Formulas as Conversion Factors
- 6.6: Mass Percent Composition of Compounds
- 6.7: Mass Percent Composition from a Chemical Formula
- 6.8: Calculating Empirical Formulas for Compounds
- 6.9: Calculating Molecular Formulas for Compounds
- 7: Chemical Reactions
- 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents
- 7.2: Evidence of a Chemical Reaction
- 7.3: The Chemical Equation
- 7.4: How to Write Balanced Chemical Equations
- 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water
- 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
- 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
- 7.8: Acid–Base and Gas Evolution Reactions
- 7.9: Oxidation–Reduction Reactions
- 7.10: Classifying Chemical Reactions
- 7.11: The Activity Series
- 8: Quantities in Chemical Reactions
- 8.1: Climate Change: Too Much Carbon Dioxide
- 8.2: Stoichiometry
- 8.3: Making Molecules: Mole-to-Mole Conversions
- 8.4: Making Molecules: Mass-to-Mass Conversions
- 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield
- 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
- 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
- 9: Electrons in Atoms and the Periodic Table
- 9.1: Blimps, Balloons, and Models of the Atom
- 9.2: Light: Electromagnetic Radiation
- 9.3: The Electromagnetic Spectrum
- 9.4: The Bohr Model: Atoms with Orbits
- 9.5: The Quantum-Mechanical Model: Atoms with Orbitals
- 9.6: Quantum-Mechanical Orbitals and Electron Configurations
- 9.7: Electron Configurations and the Periodic Table
- 9.8: The Explanatory Power of the Quantum-Mechanical Model
- 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
- 10: Chemical Bonding
- 10.1: Bonding Models and AIDS Drugs
- 10.2: Representing Valence Electrons with Dots
- 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred
- 10.4: Covalent Lewis Structures: Electrons Shared
- 10.5: Writing Lewis Structures for Covalent Compounds
- 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule
- 10.7: Predicting the Shapes of Molecules
- 10.8: Electronegativity and Polarity - Why Oil and Water Don’t Mix
- 11: Gases
- 11.1: Extra-Long Straws
- 11.2: Kinetic Molecular Theory: A Model for Gases
- 11.3: Pressure: The Result of Constant Molecular Collisions
- 11.4: Boyle’s Law: Pressure and Volume
- 11.5: Charles’s Law: Volume and Temperature
- 11.6: Gay-Lussac's Law: Temperature and Pressure
- 11.7: The Combined Gas Law: Pressure, Volume, and Temperature
- 11.8: Avogadro’s Law: Volume and Moles
- 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
- 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
- 11.11: Gases in Chemical Reactions
- 12: Liquids, Solids, and Intermolecular Forces
- 12.1: Interactions between Molecules
- 12.2: Properties of Liquids and Solids
- 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity
- 12.4: Evaporation and Condensation
- 12.5: Melting, Freezing, and Sublimation
- 12.6: Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
- 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic
- 12.8: Water: A Remarkable Molecule
- 13: Solutions
- 13.1: Prelude - Tragedy in Cameroon
- 13.2: Solutions: Homogeneous Mixtures
- 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy
- 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz
- 13.5: Solution Concentration: Mass Percent
- 13.6: Solution Concentration: Molarity
- 13.7: Solution Dilution
- 13.8: Solution Stoichiometry
- 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
- 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration
- 14: Acids and Bases
- 14.1: Sour Patch Kids and International Spy Movies
- 14.2: Acids: Properties and Examples
- 14.3: Bases: Properties and Examples
- 14.4: Molecular Definitions of Acids and Bases
- 14.5: Reactions of Acids and Bases
- 14.6: Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
- 14.7: Strong and Weak Acids and Bases
- 14.8: Water: Acid and Base in One
- 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity
- 14.10: Buffers: Solutions That Resist pH Change
- SCC: CHEM 300 - Beginning Chemistry (Faculty)
- 1: The Chemical World
- 2: Measurement and Problem Solving
- 2.1: Taking Measurements
- 2.2: Scientific Notation: Writing Large and Small Numbers
- 2.3: Significant Figures: Writing Numbers to Reflect Precision
- 2.4: Significant Figures in Calculations
- 2.5: The Basic Units of Measurement
- 2.6: Problem Solving and Unit Conversions
- 2.7: Solving Multistep Conversion Problems
- 2.8: Units Raised to a Power
- 2.9: Density
- 2.10: Numerical Problem-Solving Strategies and the Solution Map
- 2.E: Measurement and Problem Solving (Exercises)
- 3: Matter and Energy
- 3.1: In Your Room
- 3.2: What is Matter?
- 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas
- 3.4: Classifying Matter According to Its Composition
- 3.5: Differences in Matter: Physical and Chemical Properties
- 3.6: Changes in Matter: Physical and Chemical Changes
- 3.7: Conservation of Mass: There is No New Matter
- 3.8: Energy
- 3.9: Energy and Chemical and Physical Change
- 3.10: Temperature: Random Motion of Molecules and Atoms
- 3.11: Temperature Changes: Heat Capacity
- 3.12: Energy and Heat Capacity Calculations
- 3.E: Exercises
- 4: Atoms and Elements
- 4.1: Experiencing Atoms at Tiburon
- 4.2: Indivisible: The Atomic Theory
- 4.3: The Nuclear Atom
- 4.4: The Properties of Protons, Neutrons, and Electrons
- 4.5: Elements: Defined by Their Numbers of Protons
- 4.6: Looking for Patterns: The Periodic Law and the Periodic Table
- 4.7: Ions: Losing and Gaining Electrons
- 4.8: Isotopes: When the Number of Neutrons Varies
- 4.9: Atomic Mass: The Average Mass of an Element’s Atoms
- 5: Molecules and Compounds
- 5.1: Sugar and Salt
- 5.2: Compounds Display Constant Composition
- 5.3: Chemical Formulas: How to Represent Compounds
- 5.4: A Molecular View of Elements and Compounds
- 5.5: Writing Formulas for Ionic Compounds
- 5.6: Nomenclature: Naming Compounds
- 5.7: Naming Ionic Compounds
- 5.8: Naming Molecular Compounds
- 5.9: Naming Acids
- 5.10: Nomenclature Summary
- 5.11: Formula Mass: The Mass of a Molecule or Formula Unit
- 6: Chemical Composition
- 6.1: How Much Sodium?
- 6.2: Counting Nails by the Pound
- 6.3: Counting Atoms by the Gram
- 6.4: Counting Molecules by the Gram
- 6.5: Chemical Formulas as Conversion Factors
- 6.6: Mass Percent Composition of Compounds
- 6.7: Mass Percent Composition from a Chemical Formula
- 6.8: Calculating Empirical Formulas for Compounds
- 6.9: Calculating Molecular Formulas for Compounds
- 7: Chemical Reactions
- 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents
- 7.2: Evidence of a Chemical Reaction
- 7.3: The Chemical Equation
- 7.4: How to Write Balanced Chemical Equations
- 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water
- 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
- 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
- 7.8: Acid–Base and Gas Evolution Reactions
- 7.9: Oxidation–Reduction Reactions
- 7.10: Classifying Chemical Reactions
- 7.11: The Activity Series
- 8: Quantities in Chemical Reactions
- 8.1: Climate Change: Too Much Carbon Dioxide
- 8.2: Stoichiometry
- 8.3: Making Molecules: Mole-to-Mole Conversions
- 8.4: Making Molecules: Mass-to-Mass Conversions
- 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield
- 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
- 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
- 9: Electrons in Atoms and the Periodic Table
- 9.1: Blimps, Balloons, and Models of the Atom
- 9.2: Light: Electromagnetic Radiation
- 9.3: The Electromagnetic Spectrum
- 9.4: The Bohr Model: Atoms with Orbits
- 9.5: The Quantum-Mechanical Model: Atoms with Orbitals
- 9.6: Quantum-Mechanical Orbitals and Electron Configurations
- 9.7: Electron Configurations and the Periodic Table
- 9.8: The Explanatory Power of the Quantum-Mechanical Model
- 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
- 10: Chemical Bonding
- 10.1: Bonding Models and AIDS Drugs
- 10.2: Representing Valence Electrons with Dots
- 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred
- 10.4: Covalent Lewis Structures: Electrons Shared
- 10.5: Writing Lewis Structures for Covalent Compounds
- 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule
- 10.7: Predicting the Shapes of Molecules
- 10.8: Electronegativity and Polarity: Why Oil and Water Don’t Mix
- 11: Gases
- 11.1: Extra-Long Straws
- 11.2: Kinetic Molecular Theory: A Model for Gases
- 11.3: Pressure: The Result of Constant Molecular Collisions
- 11.4: Boyle’s Law: Pressure and Volume
- 11.5: Charles’s Law: Volume and Temperature
- 11.6: Gay-Lussac's Law: Temperature and Pressure
- 11.7: The Combined Gas Law: Pressure, Volume, and Temperature
- 11.8: Avogadro’s Law: Volume and Moles
- 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
- 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
- 11.11: Gases in Chemical Reactions
- 12: Liquids, Solids, and Intermolecular Forces
- 12.1: Interactions between Molecules
- 12.2: Properties of Liquids and Solids
- 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity
- 12.4: Evaporation and Condensation
- 12.5: Melting, Freezing, and Sublimation
- 12.6: Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
- 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic
- 12.8: Water: A Remarkable Molecule
- 13: Solutions
- 13.1: Prelude - Tragedy in Cameroon
- 13.2: Solutions: Homogeneous Mixtures
- 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy
- 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz
- 13.5: Solution Concentration: Mass Percent
- 13.6: Solution Concentration: Molarity
- 13.7: Solution Dilution
- 13.8: Solution Stoichiometry
- 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
- 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration
- 14: Acids and Bases
- 14.1: Sour Patch Kids and International Spy Movies
- 14.2: Acids: Properties and Examples
- 14.3: Bases: Properties and Examples
- 14.4: Molecular Definitions of Acids and Bases
- 14.5: Reactions of Acids and Bases
- 14.6: Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
- 14.7: Strong and Weak Acids and Bases
- 14.8: Water: Acid and Base in One
- 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity
- 14.10: Buffers: Solutions That Resist pH Change
- SCC: CHEM 300 - Beginning Chemistry (Alviar-Agnew)
- SCC: Chem 330 - Adventures in Chemistry (Alviar-Agnew)
- SCC: Chem 309 - General, Organic and Biochemistry (Bennett)
- AGENDA (Spring)
- AGENDA (Fall)
- Homework
- 1: Measurement of Matter & Energy
- 2: Atomic Structure
- 3: Nuclear Chemistry and Medicine
- 4: Ionic Bonding and Simple Ionic Compounds
- 5: Covalent Bonding & Simple Molecular Compounds: Questions
- 6: Quantities in Chemical Reactions
- 7: Solids, Liquids and Gases: Questions
- 8: Hydrocarbons Structure & Nomenclature: Questions
- 9: Organic Functional Groups Structure & Nomenclature: Questions
- 10: Organic Functional Groups Physical Properities and Intro to Acid Base Chemistry
- 11: Solutions, Colloids and Membranes: Questions
- 12: Acids, Bases, pH and Buffers: Questions
- 13: Reactions of Organic Functional Groups in Biochemistry: Questions
- 14: Carbohydrates (Structure and Function): Questions
- 15: Lipids (Structure and Function): Questions
- 16: Proteins: Structure and Function: Questions
- 17: Nucleic Acids: DNA and RNA
- 18: Metabolism and Bioenergetics: Questions
- Homework Solutions
- 1: Homework Solutions
- 2: Homework Solutions
- 3: Homework Solutions
- 4: Homework Solutions
- 5: Homework Solutions
- 6: Homework Solutions
- 7: Homework Solutions
- 8: Homework Solutions
- 9: Homework Solutions
- 10: Homework Solutions
- 11: Homework Solutions
- 12: Homework Solutions
- 13: Homework Solutions
- 14: Homework Solutions
- 15: Homework Solutions
- 16: Homework Solutions
- 17: Homework Solutions
- 18: Homework Solutions
- Chapters
- 1: Measuring Matter and Energy
- 1.1: What is Chemistry
- 1.2: Classification of Matter
- 1.3: Introduction to Kinetic and Potential Energy
- 1.4: Measurements
- 1.5: Expressing Numbers: Scientific Notation
- 1.6: Expressing Numbers: Significant Figures
- 1.7: The International System of Units
- 1.8: Converting Units
- 1.9: Temperature Conversions
- 1.10: Specific Heat
- 1.11: Dosage Calculations
- 1.12: Chapter Summary
- 2: Atomic Structure
- 3: Nuclear Chemistry
- 4: Ionic Bonding and Simple Ionic Compounds
- 5: Covalent Bonding and Simple Molecular Compounds
- 6: Quantities in Chemical Reactions
- 6.1: Formula Mass
- 6.2: The Mole
- 6.3: Atomic and Molar Masses
- 6.4: Mole-Mass Conversions
- 6.5: Mole-Mole Relationships in Chemical Reactions
- 6.6: The Law of Conservation of Matter
- 6.7: Balancing Chemical Equations
- 6.8: Bond Energies and Chemical Reactions
- 6.9: Energetics of Biochemical Reactions
- 6.10: Energies, Kinetics, and Catalysts
- 6.11: Equilbria and Le Châtelier's Principle
- 6.12: Chapter Summary
- 7: States of Matter and the Gas Laws
- 8: Organic Chemistry of Hydrocarbons
- 8.1: Introduction to Organic Chemistry
- 8.2: Organic Chemistry
- 8.3: Structures and Names of Alkanes
- 8.4: Branched-Chain Alkanes
- 8.5: Condensed Structural and Line-Angle Formulas
- 8.6: Cycloalkanes
- 8.7: IUPAC Nomenclature
- 8.8: Alkenes: Structure and Nomenclature
- 8.9: Alkenes: Cis-Tran Isomerization
- 8.10: Alkynes
- 8.11: Aromatic Compounds
- 8.12: Aromatic Compounds: Structure & Nomenclature
- 8.13: Physical Properties of Hydrocarbons
- 8.14: Chapter Summary
- 9: Organic Functional Groups: Structure and Nomenclature
- 9.1: Organic Compounds with Functional Groups
- 9.2 Alcohols and Phenols: Nomenclature and Classification
- 9.3: Glycols and Glycerol
- 9.4: Ethers
- 9.5: Aldehydes and Ketones: Structure and Names
- 9.6: Organic Sulfur Compounds
- 9.7: Carboxylic Acids: Structures and Names
- 9.8: Esters: Structures and Names
- 9.9: Phosphate Esters
- 9.10: Amines
- 9.11: Amides
- 10: Organic Functional Groups: Introduction to Acid-Base Chemistry
- 10.1: Physical Properties of Alcohols
- 10.2: Physical Properties of Aldehydes and Ketones
- 10.3: Physical Properties of Carboxylic Acids
- 10.4: Physical Properties of Esters
- 10.5: Physical Properties of Amines
- 10.6: Physical Properties of Amides
- 10.7: Ionization of Carboxylic Acids
- 10.8: Amines as Bases
- 10.9: Chirality
- 10.10: End-of-Chapter Material
- 11: Solutions
- 12: Acids and Bases
- 13: Functional Group Reactions
- 13.1: Oxidation-Reduction (Redox) Reactions
- 13.2: Redox Reactions in Organic Chemistry
- 13.3: Reactions that Form Alcohols
- 13.4: Reactions of Alcohols
- 13.5: The Formation of Carboxylic Acids
- 13.6: Properties of Esters
- 13.7: Hydrolysis of Esters
- 13.8: Formation of Amides
- 13.9: Hydrolysis of Amides
- 13.10: Phosphoester Formation
- 13.11: Summary
- 14: Carbohydrates
- 15: Lipids
- 16: Proteins and Enzymes
- 17: Nucleic Acids
- 18: Metabolism
- 1: Measuring Matter and Energy
- SCC: Chem 400 - General Chemistry I
- Chapters
- 1: Matter, Measurement, and Problem Solving
- 1.1: Atoms and Molecules
- 1.2: The Scientific Approach to Knowledge
- 1.3: The Classification of Matter
- 1.4: Physical and Chemical Changes and Properties
- 1.5: Energy: A Fundamental Part of Physical and Chemical Change
- 1.6: The Units of Measurement
- 1.7: The Reliability of a Measurement
- 1.8: Solving Chemical Problems
- 1.E: Matter, Measurement, and Problem Solving (Exercises)
- 2: Atoms and Elements
- 2.1: Brownian Motion: Evidence for Atoms
- 2.2: Early Ideas about the Building Blocks of Matter
- 2.3: Modern Atomic Theory and the Laws That Led to It
- 2.4: The Discovery of the Electron
- 2.5 The Structure of The Atom
- 2.6 Subatomic Particles: Protons, Neutrons, and Electrons in Atoms
- 2.7 Finding Patterns: The Periodic Law and the Periodic Table
- 2.8 Atomic Mass: The Average Mass of an Element’s Atoms
- 2.9 Molar Mass: Counting Atoms by Weighing Them
- 2.E : Atoms and Elements (Exercises)
- 3: Molecules, Compounds and Chemical Equations
- 3.1: Hydrogen, Oxygen, and Water
- 3.2: Chemical Bonds
- 3.3: Representing Compounds: Chemical Formulas and Molecular Models
- 3.4: An Atomic-Level Perspective of Elements and Compounds
- 3.5: Ionic Compounds: Formulas and Names
- 3.6: Molecular Compounds: Formulas and Names
- 3.7: Summary of Inorganic Nomenclature
- 3.9: Composition of Compounds
- 3.10: Determining a Chemical Formula from Experimental Data
- 3.11: Writing and Balancing Chemical Equations
- 3.12: Organic Compounds
- 3.E: Molecules, Compounds and Chemical Equations (Exercises)
- 4: Chemical Reactions and Aqueous Reactions
- 4.1: Global Warming and the Combustion of Fossil Fuels
- 4.2 Reaction Stoichiometry: How Much Carbon Dioxide?
- 4.3 Limiting Reactant, Theoretical Yield, and Percent Yield
- 4.4: Solution Concentration and Solution Stoichiomentry
- 4.5: Types of Aqueous Solutions and Solubility
- 4.6: Precipitation Reactions
- 4.7: Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
- 4.8: Acid-Base and Gas-Evolution Reactions
- 4.9: Oxidation-Reduction Reactions
- 5: Gases
- 5.1: Water from Wells: Atmospheric Pressure at Work
- 5.2: Pressure: The Result of Particle Collisions
- 5.3: The Simple Gas Laws: Boyle’s Law, Charles’s Law and Avogadro’s Law
- 5.4: The Ideal Gas Law
- 5.5: Applications of the Ideal Gas Law: Molar Volume, Density and Molar Mass of a Gas
- 5.6: Mixtures of Gases and Partial Pressures
- 5.7: Gases in Chemical Reactions: Stoichiometry Revisited
- 5.8: Kinetic Molecular Theory: A Model for Gases
- 5.9: Mean Free Path, Diffusion, and Effusion of Gases
- 5.10: Real Gases: The Effects of Size and Intermolecular Forces
- 5.E: Gases (Exercises)
- 6: Thermochemistry
- 6.1: Light the Furnace: The Nature of Energy and Its Transformations
- 6.3: The First Law of Thermodynamics
- 6.2: The Nature of Energy
- 6.4: Quantifying Heat and Work
- 6.4: Constant Volume Calorimetry: Measuring ΔU for Chemical Reactions
- 6.5: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
- 6.7: Constant Pressure Calorimetry: Measuring ΔH for Chemical Reactions
- 6.7: Relationships Involving Enthalpy of Reactions
- 6.8: Enthalpies of Reaction from Standard Heats of Formation
- 6.9: Energy Use and The Environment
- 7: The Quantum-Mechanical Model of the Atom
- 8: Periodic Properties of the Elements
- 8.1: Nerve Signal Transmission
- 8.2: The Development of the Periodic Table
- 8.3: Electron Configurations: How Electrons Occupy Orbitals
- 8.4: Electron Configurations, Valence Electrons, and the Periodic Table
- 8.5: The Explanatory Power of the Quantum-Mechanical Model
- 8.6: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
- 8.7: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
- 8.8: Electron Affinities and Metallic Character
- 8.9: Examples of Periodic Chemical Behavior
- 8.E: Periodic Properties of the Elements (Exercises)
- 9: Chemical Bonding I: Lewis Structures & Determining Molecular Shapes
- 9.1: Bonding Models and AIDS Drugs
- 9.2: Types of Chemical Bonds
- 9.3: Representing Valance Electrons with Dots
- 9.4: Ionic Bonding
- 9.5: Covalent Bonding: Lewis Structure
- 9.6: Electronegativity and Bond Polarity
- 9.7: Lewis Structures
- 9.8: Resonance and Formal Charge
- 9.9: Exceptions to the Octet Rule
- 9.10: Bond Energies and Bond Lengths
- 9.11: Bonding in Metals
- 9.E: Chemical Bonding I (Exercises)
- 10: Chemical Bonding II: Valance Bond Theory and Molecular Orbital Theory
- 10.1: Artificial Sweeteners
- 10.2: VSEPR Theory: The Five Basic Shapes
- 10.3: VSPER Theory: The Effect of Lone Pairs
- 10.4: VSPER Theory: Predicting Molecular Geometries
- 10.5: Molecular Shape and Polarity
- 10.6: Valence Bond Theory: Orbital Overlap as a Chemical Bond
- 10.7: Valence Bond Theory: Hybridization of Atomic Orbitals
- 10.8: Molecular Orbital Theory: Electron Delocalization
- 11: Liquids, Solids, and Intermolecular Forces
- 11.1: Water in Zero Gravity
- 11.2: Solids, Liquids, and Gases: A Molecular Comparison
- 11.3: Intermolecular Forces: The Forces that Hold Condensed Phases Together
- 11.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
- 11.5: Vaporization and Vapor Pressure
- 11.6: Sublimation and Fusion
- 11.7: Heating Curve for Water
- 11.8: Phase Diagrams
- 11.9: Water - An Extraordinary Substance
- 12: Solids and Modern Materials
- 12.1: Discovery of Graphene
- 12.2: X-Ray Crystallography
- 12.3: Unit Cells and Basic Structures
- 12.4: The Fundamental Types of Crystalline Solids
- 12.5: The Structure of Ionic Solids
- 12.6: Network Covalent Atomic Solids: Carbon and Silicates
- 12.7: Ceramics, Cement, and Glass
- 12.8: Crystalline Solids: Band Theory
- 12.9: Polymers and Plastics
- 13: Solutions
- 13.1: Thirsty Solutions: Why You Should Not Drink Seawater
- 13.2: Types of Solutions and Solubility
- 13.3: Energetics of Solution Formation
- 13.4: Solution Equilibrium and Factors Affecting Solubility
- 13.5: Expressing Solution Concentration
- 13.6: Colligative Properties: Freezing Point Depression, Boiling Point Elevation, and Osmosis
- 13.7: The Colligative Properties of Strong Electrolyte Solutions
- 13.8: Colloids
- 13.E: Solutions (Exercises)
- 14: Chemical Kinetics
- 15: Chemical Equilibrium
- 15.1: Fetal Hemoglobin and Equilibrium
- 15.2: The Concept of Dynamic Equilibrium
- 15.3: The Equilibrium Constant (K)
- 15.4: Expressing the Equilibrium Constant in Terms of Pressure
- 15.5: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
- 15.5: Heterogenous Equilibria: Reactions Involving Solids and Liquids
- 15.7: The Reaction Quotient: Predicting the Direction of Change
- 15.8: Finding Equilibrium Concentrations
- 15.9: Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
- 16: Acids and Bases
- 16.1: Heartburn
- 16.2: The Nature of Acids and Bases
- 16.3: Definitions of Acids and Bases
- 16.4: Acid Strength and the Acid Dissociation Constant (Ka)
- 16.5: Autoionization of Water and pH
- 16.6: Finding the [H3O+] and pH of Strong and Weak Acid Solutions
- 16.7: Base Solutions
- 16.8: The Acid-Base Properties of Ions and Salts
- 16.9: Polyprotic Acids
- 16.10: Acid Strength and Molecular Structure
- 16.11: Lewis Acids and Bases
- 16.12: Acid rain
- 17: Aqueous Ionic Equilibrium
- 17.1: The Danger of Antifreeze
- 17.2: Buffers: Solutions That Resist pH Change
- 17.3: Buffer Effectiveness: Buffer Capacity and Buffer Range
- 17.4: Titrations and pH Curves
- 17.5: Solubility Equilibria and the Solubility Product Constant
- 17.6: Precipitation
- 17.7: Qualitative Chemical Analysis
- 17.8: Complex Ion Equilibria
- 17.E: Aqueous Ionic Equilibrium (Exercises)
- 18: Gibbs Energy and Thermodynamics
- 18.1: Nature’s Heat Tax: You Can’t Win and You Can’t Break Even
- 18.2: Spontaneous and Nonspontaneous Processes
- 18.3: Entropy and the Second Law of Thermodynamics
- 18.4: Entropy Changes Associated with State Changes
- 18.5: Heat Transfer and Changes in the Entropy of the Surroundings
- 18.6: Gibbs Energy
- 18.7: Entropy Changes in Chemical Reactions
- 18.8: Gibbs Energy Changes in Chemical Reactions
- 18.9: Gibbs Energy Changers for Non-Standard States
- 18.10: Gibbs Energy and Equilibrium
- 19: Electrochemistry
- 19.1: Pulling the Plug on the Power Grid
- 19.2: Balancing Oxidation-Reduction Equations
- 19.3: Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
- 19.4: Standard Reduction Potentials
- 19.5: Cell Potential, Gibbs Energy, and the Equilibrium Constant
- 19.6: Cell Potential and Concentration
- 19.7: Batteries: Using Chemistry to Generate Electricity
- 19.8: Electrolysis: Driving Non-spontaneous Chemical Reactions with Electricity
- 19.9: Corrosion: Undesirable Redox Reactions
- 20: Radioactivity and Nuclear Chemistry
- 20.1: Diagnosing Appendicitis
- 20.2: The Discovery of Radioactivity
- 20.3: Types of Radioactivity
- 20.4: The Valley of Stability: Predicting the Type of Radioactivity
- 20.5: Detecting Radioactivity
- 20.6: The Kinetics of Radioactive Decay and Radiometric Dating
- 20.7: The Discovery of Fission: The Atomic Bomb and Nuclear Power
- 20.8: Converting Mass to Energy: Mass Defect and Nuclear Binding Energy
- 20.9: Nuclear Fusion: The Power of the Sun
- 20.10: Nuclear Transmutation and Transuranium Elements
- 20.11: The Effects of Radiation on Life
- 20.12: Radioactivity in Medicine and Other Applications
- 21: Organic Chemistry
- 21.1: Fragrances and Odor
- 21.2: Carbon: Why It Is Unique
- 21.3: Hydrocarbons: Compounds Containing Only Carbon and Hydrocarbon
- 21.4: Alkanes: Saturated Hydrocarbons
- 21.5: Alkenes and Alkynes
- 21.6: Hydrocarbon Reactions
- 21.7: Aromatic Hydrocarbons
- 21.8: Functional Groups
- 21.9: Alcohols
- 21.10: Aldehydes and Ketones
- 21.11: Carboxylic Acids and Esters
- 21.12: Ethers
- 21.13: Amines
- 22: Biochemistry
- 23: Chemistry of the Nonmetals
- 23.1: Insulated Nanowires
- 23.2: The Main-Group Elements: Bonding and Properties
- 23.3: The Most Common Matter: Silicates
- 23.4: Boron and Its Amazing Structures
- 23.5: Carbon, Carbides, and Carbonates
- 23.6: Nitrogen and Phosphorus: Essential Elements for Life
- 23.7: Oxygen
- 23.8: Sulfur: A Dangerous and Useful Element
- 23.9: Halogens: Reactive Chemicals with High Electronegativity
- 23.E: Chemistry of the Nonmetals (Exercises)
- 24: Metals and Metallurgy
- 25: Transition Metals and Coordination Compounds
- 1: Matter, Measurement, and Problem Solving
- Chapters
- SCC: Chem 401 - General Chemistry II
- SCC: Chem 420 - Organic Chemistry I
Sacramento City College is a two-year community college located in Sacramento, California and is part of the Los Rios Community College District.