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Chem 400: General Chemistry I

This is the Textmap constructed to follow the organization of Nivaldo Tro's "Chemistry: A Molecular Approach" general chemistry textbook.

Chemistry

Publisher: Sacramento City College
Source: LibreTexts
License: CC BY-NC-SA
Language: EN
Category: Basic Sciences

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Contents· 260 sections

01: 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)
02: Atoms and ElementsEdit section
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)
03: Molecules, Compounds and Chemical Equations
3.01: Hydrogen, Oxygen, and Water
3.02: Chemical Bonds
3.03: Representing Compounds: Chemical Formulas and Molecular Modelspounds: Chemical Formulas and Molecular Models
3.04: An Atomic-Level Perspective of Elements and Compounds
3.05: Ionic Compounds: Formulas and Names
3.06: Molecular Compounds: Formulas and Names
3.07: Formula Mass and The Mole Concept for Compounds
3.08: 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)
04: 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
05: Gases
5.02: Pressure: The Result of Particle Collisions
5.03: The Simple Gas Laws: Boyle’s Law, Charles’s Law and Avogadro’s Law
5.04: The Ideal Gas Law
5.05: Applications of the Ideal Gas Law: Molar Volume, Density and Molar Mass of a Gas
5.06: Mixtures of Gases and Partial Pressures
5.07: Gases in Chemical Reactions: Stoichiometry Revisited
5.08: Kinetic Molecular Theory: A Model for Gases
5.09: Mean Free Path, Diffusion, and Effusion of Gases
5.10: Real Gases: The Effects of Size and Intermolecular Forces
5.E: Gases (Exercises)
11.01: Water from Wells: Atmospheric Pressure at Work
06: Thermochemistry
6.01: Light the Furnace: The Nature of Energy and Its Transformations
6.02: The First Law of Thermodynamics
6.02: The Nature of Energy
6.03: Quantifying Heat and Work
6.04: Measuring ΔE for Chemical Reactions: Constant-Volume Calorimetry
6.05: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
6.06" Constant Pressure Calorimetry: Measuring DHrxn
6.07 Relationships Involving DHrxn
6.08: Enthalpies of Reaction from Standard Heats of Formation
6.09 Energy Use and The Environment
07: The Quantum-Mechanical Model of the Atom
7.1: Schrödinger's Cat
7.2: The Nature of Light
7.3: Atomic Spectroscopy and The Bohr Model
7.4: The Wavelength Nature of Matter
7.5: Quantum Mechanics and The Atom
7.6: The Shape of Atomic Orbitals
7.E: The Quantum-Mechanical Model of the Atom (Exercises)
08: 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)
09: Chemical Bonding I: Drawing Lewis Structures
9.01: Bonding Models and AIDS Drugs
9.02: Types of Chemical Bonds
9.03: Representing Valance Electrons with Dots
9.04: Ionic Bonding
9.05: Covalent Bonding: Lewis Structure
9.06: Electronegativity and Bond Polarity
9.07: Lewis Structures
9.08: Resonance and Formal Charge
9.09: 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: Molecular Shapes, 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
11.01: Water in Zero Gravity
11.02: Solids, Liquids, and Gases: A Molecular Comparison
11.03: Intermolecular Forces: The Forces that Hold Condensed Phases Together
11.04: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
11.05: Vaporization and Vapor Pressure
11.06: Sublimation and Fusion
11.07: Heating Curve for Water
11.08: Phase Diagrams
11.09: 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
14.1: Catching Lizards
14.2: Rate of a Chemical Reaction
14.3: The Rate Law: The Effect of Concentration on Reaction Rate
14.4: The Integrated Rate Law: The Dependence of Concentration on Time
14.5: The Effect of Temperature on Reaction Rate
14.6: Reaction Mechanisms
14.7: Catalysis
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
16.01: Heartburn
16.02: The Nature of Acids and Bases
16.03: Definitions of Acids and Bases
16.04: Acid Strength and the Acid Dissociation Constant (Ka)
16.05: Autoionization of Water and pH
16.06: Finding the [H3O ] and pH of Strong and Weak Acid Solutions
16.07: Base Solutions
16.08: The Acid-Base Properties of Ions and Salts
16.09: 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
18.01: Nature’s Heat Tax: You Can’t Win and You Can’t Break Even
18.02: Spontaneous and Nonspontaneous Processes
18.03: Entropy and the Second Law of Thermodynamics
18.04: Entropy Changes Associate with State Changes
18.05: Heat Transfer and Changes in the Entropy of the Surroundings
18.06: Gibbs Energy
18.07: Entropy Changes in Chemical Reactions
18.08: Gibbs Energy Changes in Chemical Reactions
18.09: 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
20.01: Diagnosing Appendicitis
20.02: The Discovery of Radioactivity
20.03: Types of Radioactivity
20.04: The Valley of Stability: Predicting the Type of Radioactivity
20.05: Detecting Radioactivity
20.06: The Kinetics of Radioactive Decay and Radiometric Dating
20.07: The Discovery of Fission: The Atomic Bomb and Nuclear Power
20.08: Converting Mass to Energy: Mass Defect and Nuclear Binding Energy
20.09: 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
21.01: Fragrances and Odor
21.02: Carbon: Why It Is Unique
21.03: Hydrocarbons: Compounds Containing Only Carbon and Hydrocarbon
21.04: Alkanes: Saturated Hydrocarbons
21.05: Alkenes and Alkynes
21.06: Hydrocarbon Reactions
21.07: Aromatic Hydrocarbons
21.08: Functional Groups
21.09: Alcohols
21.10: Aldehydes and Ketones
21.11: Carboxylic Acids and Esters
21.12: Ethers
21.13: Amines
22: Biochemistry
22.1: Diabetes and the Synthesis of Human Insulin
22.2: Lipids
22.3: Carbohydrates
22.4: Proteins and Amino Acids
22.5: Protein Structure
22.6: Nucleic Acids: Blueprints for Proteins
22.7: DNA Replication, the Double Helix, and Protein Synthesis
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
24.1: Vanadium: A Problem and an Opportunity
24.2: The General Properties and Natural Distribution of Metals
24.3: Metallurgical Processes
24.4: Metal Structures and Alloys
24.5: Sources, Properties, and Products of Some of the 3d Transition Metals
25: Transition Metals and Coordination Compounds
25.1: The Colors of Rubies and Emeralds
25.2: Properties of Transition Metals
25.3: Coordination Compounds
25.4: Structure and Isomerization
25.5: Bonding in Coordinate Compounds
25.6: Applications of Coordination Compounds
25.E: Transition Metals and Coordination Compounds (Exercises)