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Chapter 9: Problem 9
Name one ionic compound that contains only nonmetallic elements.
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Specify which compound in the following pairs of ionic compounds has the higher lattice energy: (a) \(\mathrm{KCl}\) or \(\mathrm{MgO},\) (b) \(\mathrm{LiF}\) or \(\mathrm{LiBr}\) (c) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}\) or \(\mathrm{NaCl}\). Explain your choice.
True or false: (a) Formal charges represent actual separation of charges; (b) \(\Delta H_{\mathrm{rxn}}^{\circ}\) can be estimated from bond enthalpies of reactants and products; (c) all second-period elements obey the octet rule in their compounds; (d) the resonance structures of a molecule can be separated from one another.
Define bond enthalpy. Bond enthalpies of polyatomic molecules are average values. Why?
Arrange these bonds in order of increasing ionic character: carbon to hydrogen, fluorine to hydrogen, bromine to hydrogen, sodium to chlorine, potassium to fluorine, lithium to chlorine.
Classify these bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (b) the \(\mathrm{SiCl}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (c) the CaF bond in \(\mathrm{CaF}_{2},\) (d) the \(\mathrm{NH}\) bond in \(\mathrm{NH}_{3}\).
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