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  • Chapters Part 1
    • Chapter 1
    • Chapter 2>
      • 2.1 Scientific Notation
      • 2.2 Units
      • 2.3 Measurements of Length, Volume, and Mass
      • 2.4 Uncertainty in Measurement
      • 2.5 Significant Figures
      • 2.6 Problem Solving and Dimensional Analysis
    • Chapter 3>
      • 3.1 Matter
      • 3.2 Physical and Chemical Properties and Changes
      • 3.3 Elements and Compounds
      • 3.4 Mistures and Pure Substances
      • 3.5 Separation of Mixtures
    • Chapter 4>
      • 4.1 The Elements
      • 4.2 The Symbols
      • 4.3 Dalton's Atomic Theory
      • 4.4 Formulas of Compounds
      • 4.5 The Structure of The Atom
      • 4.6 Introduction to the Modern Concept of Atomic Structure
      • 4.7 Isotopes
    • Chapter 11>
      • 11.1 Rutherford's Atom
      • 11.2 Electromagnetic Radiation
      • 11.3 Emission of Energy by Atom
      • 11.4 The Energy Levels of Hydrogen
      • 11.5 The Bohr Model of the Atom
      • 11.6 The Wave Mechanical Model of the Atom
      • 11.7 The Hydrogen Orbitals
      • 11.8 The Wave Mechanical Model: Further Development
      • 11.9 Electron Arrangements in the First Eighteen Atoms on the Periodic Table
      • 11.10 Electron Configuration and the Periodic Table
      • 11.11 Atomic Properties and the Periodic Table
    • Chapter 12>
      • 12.1 Types of Chemical Bonds
      • 12.2 Electronegativity
      • 12.3 Bond Polarity and Dipole Moments
      • 12.4 Stable Electron Configurations and Charges on Ions
      • 12.5 Ionic Bonding and Structures of Ionic Compounds
      • 12.6 Lewis Structures
      • 12.7 Lewis Structures of Molecules with Multiple Bonds
      • 12.8 Molecular Structure
      • 12.9 Molecular Structure: The VSEPR Model
      • 12.10 Molecular Structure: Molecules with Double Bonds
    • Chapter 5>
      • 5.1 Naming Compounds
      • 5.2 Naming Binary Compounds That Contain a Metal and a Nonmetal (Types I and II)
      • 5.3 Naming Binary Compounds That Contain Only Nonmetals (Type III)
      • 5.5 Naming Compounds That Contain Polyatomic Ions
      • 5.6 Naming Acids
      • 5.7 Writing Formulas from Names
    • Chapter 6>
      • 6.1 Evidence for a Chemical Reaction
      • 6.2 Chemical Equations
      • 6.3 Balancing Chemical Equations
    • Chapter 7>
      • 7.1 Predicting Whether a Reaction Will Occur
      • 7.2 Reactions in Which a Solid Forms
      • 7.3 Describing Reactions in Aqueous Solutions
      • 7.4 Reactions That Form Water: Acids and Bases
      • 7.5 Reactions of Metals with Nonmetals (Oxidation-Reduction)
  • Chapters Part 2
    • Chapter 8>
      • 8.1 Counting by Weighing
      • 8.2 Atomic Masses: Counting Atoms by Weighing
      • 8.3 The Mole
      • 8.4 Learning to Solve Problem
      • 8.5 Molar Mass
      • 8.6 Percent Composition of Compound
      • 8.7 Formulas of Compound
      • 8.8 Calculation of Empirical Formulas
      • 8.9 Calculation of Molecular Formulas
    • Chapter 9>
      • 9.1 Information Given by Chemical Equations
      • 9.2 Mole-Mole Relationships
      • 9.3 Mass Calculations
      • 9.4 The Concept of Limiting Reactants
      • 9.5 Calculations Involving a Limiting Reactant
      • 9.6 Percent Yield
    • Chapter 13>
      • 13.1 Pressure
      • 13.2 Pressure and Volume: Boyle's Law
      • 13.3 Volume and Temperature: Charles's Law
      • 13.4 Volume and Moles: Avogadro's Law
      • 13.5 The Ideal Gas Law
      • 13.6 Dalton's Law of Partial Pressures
      • 13.8 The Kinetic Molecular Theory of Gases
      • 13.10 Gas Stoichiometry
    • Chapter 15>
      • 15.1 Solubility
      • 15.2 Solution Composition: An Introduction
      • 15.3 Solution Composition: Mass Percent
      • 15.4 Solution Composition: Molarity
      • 15.5 Dilution
      • 15.6 Stoichiometry of Solution Reactions
      • 15.7 Neutralization Reactions
      • 15.8 Solution Composition: Normality
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OBJECTIVE: To understand some important features of subatomic particles.
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The space in which the electrons move accounts for most of the atomic volume. The electrons are the parts of atoms that “intermingle” when atoms combine to form molecules. Therefore, the number of electrons a given atom possesses greatly affects the way it can interact with other atoms. As a result, atoms of different elements, which have different numbers of electrons, show different chemical behavior. Although the atoms of different elements also differ in their numbers of protons, it is the number of electrons that really determines chemical behavior.
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    • Atoms are classified by their atomic number, which is the number of protons in the nucleus.
    • The nucleus of a hydrogen atom has one proton, so its atomic number is 1. 
    • Helium has two protons, so its atomic number is 2. 
    • Lithium has three protons, so its atomic number is 3.
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