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Chapter 9: Problem 23

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.

Short Answer

Expert verified
(a) MgO has the higher lattice energy. (b) LiF has the higher lattice energy. (c) Mg3N2 has the higher lattice energy.

Step by step solution

01

Identify Charges and Sizes of Ions

Identify the charges and sizes of the ions in the compounds. K+ and Cl- in KCl, Mg2+ and O2- in MgO, Li+ and F- in LiF, Li+ and Br- in LiBr, Mg2+ and N3- in Mg3N2, Na+ and Cl- in NaCl.
02

Compare the Lattice Energy

Compare the lattice energy using the Lattice Energy Law: Higher the charges of the ions and smaller the sizes of ions, higher the lattice energy. Thus, (a) MgO has a higher lattice energy than KCl because Mg2+ and O2- result in a higher lattice energy than K+ and Cl-. (b) LiF has a higher lattice energy than LiBr because F- being smaller in size than Br-, it forms a more energetically stable ionic compound. (c) Mg3N2 has a higher lattice energy than NaCl because Mg2+ and N3- result in a higher lattice energy than Na+ and Cl-.

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Most popular questions from this chapter

Classify these bonds as ionic, polar covalent, or \(\mathrm{co}-\) valent, and give your reasons: (a) the CC bond in \(\mathrm{H}_{3} \mathrm{CCH}_{3},\) (b) the KI bond in \(\mathrm{KI},(\mathrm{c})\) the \(\mathrm{NB}\) bond in \(\mathrm{H}_{3} \mathrm{NBCl}_{3},\) (d) the \(\mathrm{ClO}\) bond in \(\mathrm{ClO}_{2}\).

The term "molar mass" was introduced in Chapter 3 What is the advantage of using the term "molar mass" when we discuss ionic compounds?

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Draw Lewis structures of these organic molecules: (a) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right) ;\) (b) ethanol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right)\); (c) tetraethyllead \(\left[\mathrm{Pb}\left(\mathrm{CH}_{2} \mathrm{CH}_{3}\right)_{4}\right]\), which was used in "leaded" gasoline; (d) methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\) (e) mustard gas \(\left(\mathrm{ClCH}_{2} \mathrm{CH}_{2} \mathrm{SCH}_{2} \mathrm{CH}_{2} \mathrm{Cl}\right)\), a poison- ous gas used in World War I; (f) urea \(\left[\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\right]\), a fertilizer; (g) glycine \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{COOH}\right)\), an amino acid.

Explain how the lattice energy of an ionic compound such as \(\mathrm{KCl}\) can be determined using the Born-Haber cycle. On what law is this procedure based?
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