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Chapter 7: Chemical Formulas and Chemical Compounds

Chapter 7: Chemical Formulas and Chemical Compounds. Section 1: Chemical Names and Formulas. Overview. We will explain the significance of a chemical formula. We will again look at how to determine the formula unit of an ionic compound.

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Chapter 7: Chemical Formulas and Chemical Compounds

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  1. Chapter 7: Chemical Formulas and Chemical Compounds Section 1: Chemical Names and Formulas

  2. Overview • We will explain the significance of a chemical formula. • We will again look at how to determine the formula unit of an ionic compound. • We will name an ionic compound based on its formula unit. • We will use prefixes to name binary molecular compounds based on its formula. • We will write the name of a binary molecular compound based on its name.

  3. Significance of Formulas • A chemical formula indicates what elements there are in the compound. • It also says by the subscripts how many atoms of that element are needed. • Fe2O3 – 2 Iron Atoms, 3 Oxygen Atoms • Al2(SO4)3 – 2 Aluminum Atoms, 3 Sulfur Atoms, and 12 Oxygen Atoms • Nomenclature – A naming system.

  4. Naming Monatomic Ions • Monatomic ions are made of only one charged atom. • Naming Cations • Barium → Barium cation or Barium ion • Cesium → Cesium cation or Cesium ion • Naming Anions • Sulfur → Sulfide anion or Sulfide ion • Oxygen → Oxide anion or Oxide ion

  5. Naming Binary Ionic Compounds • If needed, solve for the formula unit. (pg 222) • Naming the formula unit: Al2O3 • Aluminum Oxide • Work it backward: Iron (II) Oxide • FeO • Stock system of nomenclature: Al2O3 • Aluminum (III) Oxide

  6. Naming Polyatomic Ion Compounds • Naming Polyatomic ion compounds: Al(NO3)3 • Aluminum Nitrate • Aluminum (III) Nitrate • See page 226 or your Mastery Manual for a list of Polyatomic ions and their names. • Oxyanions – Anions that contain oxygens.

  7. Naming Binary Molecular Compounds • See Table 7-3 on page 228 for a list of prefixes. • This nomenclature is for covalent compounds only, not for ionic compounds. • Still use the –ide suffix for nonmetals. • H2O • Dihydrogen oxide • Carbon tetrachloride • CCl4

  8. Naming Acids • See table 7-5 on page 230 for a list of common acids and their names. • Salt – An ionic compound made of a cation and anion that formed from and acid-base reaction. • Most common: • H2SO4 – Sulfuric Acid • HNO3 – Nitric Acid • HCl – Hydrochloric Acid • CH3COOH – Acetic Acid

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