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  • 71.

    List and compare the distinctive properties of ionic and molecular compounds.

  • 72.

    Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate information.

  • 73.

    Describe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors.

  • 74.

    Explain why metal surfaces are shiny.

  • 75.

    Explain why metals are malleable and ductile but ionic-crystalline compounds are not.

  • 76.

    Explain VSEPR theory.

  • 77.

    Predict the shapes of molecules or polyatomic ions using VSEPR theory.

  • 78.

    Explain how the shapes of molecules are accounted for by hybridization theory.

  • 79.

    Describe dipole-dipole forces, hydrogen bonding, induced dipoles, and London dispersion forces.

  • 80.

    Explain what determines molecular polarity.

Chapter 7 Chemical Formulas and Chemical Compounds

  • 81.

    Explain the significance of a chemical formula.

  • 82.

    Determine the formula of an ionic compound formed between two given ions.

  • 83.

    Name an ionic compound given its formula.

  • 84.

    Using prefixes, name a binary molecular compound from its formula.

  • 85.

    Write the formula of a binary molecular compound given its name.

  • 86.

    Give the oxidation number for each element in the formula of a chemical compound.

  • 87.

    Calculate the formula mass or molar mass of any given compound.

  • 88.

    Use molar mass to convert between mass in grams and amount in moles of a chemical compound.

  • 89.

    Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical


  • 90.

    Calculate the percentage composition of a given chemical compound.

  • 91.

    Define empirical formula, and explain how the term applies to ionic and molecular compounds.

  • 92.

    Determine an empirical formula from either a percentage or a mass composition.

  • 93.

    Explain the relationship between the empirical formula and the molecular formula of a given compound.

  • 94.

    Determine a molecular formula from an empirical formula.

Chapter 8 Chemical Equations and Reactions

  • 95.

    List three observations that suggest that a chemical reaction has taken place.

  • 96.

    List three requirements for a correctly written chemical equation.

  • 97.

    Write a word equation and a formula equation for a given chemical reaction.

  • 98.

    Balance a formula equation by inspection.

  • 99.

    Define and give general equations for synthesis, decomposition, single-replacement, and double-

replacement reactions.

  • 100.

    Classify a reaction as synthesis, decomposition, single-replacement, double-replacement, or combustion.

  • 101.

    List three types of synthesis reactions and six types of decomposition reaction.

  • 102.

    List four types of single-replacement reactions and three types of double-replacement reactions.

  • 103.

    Predict the products of simple reactions given the reactants.

  • 104.

    Explain the significance of an activity series.

  • 105.

    Use an activity series to predict whether a given reaction will occur and what the products will be.

Chapter 9 Stoichiometry

  • 106.

    Define stoichiometry.

  • 107.

    Describe the importance of the mole ratio in stoichiometric calculations.

  • 108.

    Write a mole ratio relating two substances in a chemical equation.

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