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CHEM100: Fundamentals of Chemistry

This Textmap is an introductory chemistry text aimed for a single semester or quarter beginning experience to the chemistry field. This Textmap surveys some of the basic topics of chemistry and should give students enough knowledge to appreciate the impact of chemistry in everyday life and, if necessary, prepare students for additional instruction in chemistry.

Chemistry

Tác giả: Brent Hamaoka
Nhà xuất bản: Palomar College
Nguồn: LibreTexts
Giấy phép: CC BY-NC-SA
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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01: The Chemical World
1.1: The Scope of Chemistry
1.2: Chemicals Compose Ordinary Things
1.3: Hypothesis Theories and Laws
1.4: The Scientific Method - How Chemists Think
1.5: A Beginning Chemist - How to Succeed
1.6: Solid Liquid and Gas
1.7: Physical and Chemical Changes
1.8: Classification of Matter
1.7: Classification of Matter
02: Measurement and Problem Solving
2.01: Measuring Global Temperatures
2.02: Scientific Notation: Writing Large and Small Numbers
2.03: Significant Figures: Writing Numbers to Reflect Precision
2.04: Significant Figures in Calculations
2.05: The Basic Units of Measurement
2.06: Problem Solving and Unit Conversions
2.07: Solving Multistep Conversion Problems
2.08: Units Raised to a Power
4.9: Density
4.10: Energy and Heat Capacity Calculations
2.4: Solid Liquid and Gas
3: Introduction to Energy
3.1: Conservation of Mass - There is No New Matter
3.2: Energy
3.3: Energy and Chemical and Physical Change
3.4: Temperature: Random Motion of Molecules and Atoms
3.5: Temperature Changes - Heat Capacity
03: Matter and Energy
2.4: Density and its Applications
3.01: In Your Room
3.02: What Is Matter
3.03: Classifying Matter According to Its State: Solid Liquid and Gas
3.04 Classifying Matter According to Its Composition
3.05: Differences in Matter: Physical and Chemical Properties
3.06: Changes in Matter: Physical and Chemical Changes
04: Atoms and Elements
5.1: Cutting Alumimun until you get Atoms
5.2: Indivisible: The Atomic Theory
5.3: The Nuclear Atom
5.4: The Properties of Protons, Neutrons, and Electrons
5.5: Elements: Defined by Their Number of Protons
5.6: Looking for Patterns: The Periodic Table
5.7: Ions - Losing and Gaining Electrons
5.8: Isotopes - When the Number of Neutrons Varies
5.9: Atomic Mass: The Average Mass of an Element’s Atoms
05: Molecules and Compounds
5.01: Sugar and Salt
5.02: Compounds Display Constant Composition
5.03: Chemical Formulas: How to Represent Compounds
5.04: A Molecular View of Elements and Compounds
5.05: Writing Formulas for Ionic Compounds
5.06: Nomenclature: Naming Compounds
5.07: Naming Ionic Compounds
5.08: Naming Molecular Compounds
5.09: Naming Acids
6.10: Nomenclature Summary
6.11: Formula Mass: The Mass of a Molecule or Formula Unit
06: Chemical Composition
7.1: How Much Sodium?
7.2: Counting Nails by the Pound
7.3: Counting Atoms by the Gram
7.4: Counting Molecules by the Gram
7.5: Chemical Formulas as Conversion Factors
7.6: Mass Percent Composition of Compounds
7.7: Mass Percent Composition from a Chemical Formula
7.8: Calculating Empirical Formulas for Compounds
7.9: Calculating Molecular Formulas for Compounds
07: Chemical Reactions
7.02: Evidence of a Chemical Reaction
7.03: The Chemical Equation
7.04: How to Write Balanced Chemical Equations
8.4: Classifying Chemical Reactions
08: Quantities in Chemical Reactions
12.1: Climate Change - Too Much Carbon Dioxide
12.2: Stoichiometry
12.3: Mole-to-Mole Conversions
12.4: Making Molecules: Mole to Mass (or vice versa) and Mass-to-Mass Conversions
12.5: Limiting Reactant and Theoretical Yield
12.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
12.7: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
9: Chemical Reactions
7.05: Aqueous Solutions and Solubility: Compounds Dissolved in Water
7.06: Precipitation Reactions
7.06: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
09: Electrons in Atoms and the Periodic Table
14.1: The Perioidic Table
14.2: Electron Configurations
14.3: Electron Configurations and the Periodic Table (The Block Method)
14.4: Electron Configurations of Ions
14.5: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
10: Acid-Base and Gas Evolution Reactions
10.1: Acids: Properties and Examples
10.2: Bases: Properties and Examples
10.3: Molecular Definitions of Acids and Bases
10.4: Reactions of Acids and Bases
10.5: Acid–Base and Gas Evolution Reactions
11: Redox Reactions
11.1: Oxidation and Reduction - Some Definitions
11.2: Electronegativity
11.3: Oxidation States: Electron Bookkeeping
11.4: Oxidation States and Redox Reactions
11.5: Half-Reactions
11.6: The Activity Series: Predicting Spontaneous Redox Reactions
11.7: Combustion Reactions
13: Solutions
13.01: Tragedy in Cameroon
13.02: Solutions: Homogeneous Mixtures
13.03: Solutions of Solids Dissolved in Water: How to Make Rock Candy
13.04: Solutions of Gases in Water: How Soda Pop Gets Its Fizz
13.05: Specifying Solution Concentration: Mass Percent
13.06: Specifying Solution Concentration: Molarity
13.07: Solution Dilution
13.08: Solution Stoichiometry
13.9: Acid–Base Titration
13.10: Water - Acid and Base in One
13.11: The pH and pOH Scales - Ways to Express Acidity and Basicity
15: Chemical Bonding
15.1: Representing Valence Electrons with Dots
15.2: Electrons are Transferred in Ionic Compounds
15.3: Lewis Structures: Electrons Shared
15.4: Lewis Structures: Counting Valence Electrons
15.5: Predicting the Shapes of Molecules
15.6: Electronegativity and Polarity - Why Oil and Water Don’t Mix
16: Gases
11.01: Extra-Long Straws
11.02: Kinetic Molecular Theory: A Model for Gases
11.03: Pressure: The Result of Constant Molecular Collisions
11.04: Boyle’s Law: Pressure and Volume
11.05: Charles’s Law: Volume and Temperature
11.05A: Gay-Lussac's Law: Temperature and Pressure
11.07: The Combined Gas Law: Pressure, Volume, and Temperature
11.08: Avogadro’s Law: Volume and Moles
11.09: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
Chapter 3: Introduction to Energy