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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 learn how a formula describes a compound’s composition.
A compound is a distinct substance that is composed of the atoms of two or more elements and always contains exactly the same relative masses of those elements. 

The types of atoms and the number of each type in each unit (molecule) of a given compound are conveniently expressed by a chemical formula. In a chemical formula the atoms are indicated by the element symbols, and the number of each type of atom is indicated by a subscript, a number that appears to the right of and below the symbol for the element.

Following are some general rules for writing formulas: 
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Write the formula for each of the following compounds, listing the elements in the order given.

  1. Each molecule of a compound that has been implicated in the formation of acid rain contains one atom of sulfur and three atoms of oxygen.

  2. Each molecule of a certain compound contains two atoms of nitrogen and five atoms of oxygen.

  3. Each molecule of glucose, a type of sugar, contains six atoms of carbon, twelve atoms of hydrogen, and six atoms of oxygen. 
                                                         S O L U T I O N   
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