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Chapter 8: Problem 41

Predict the empirical formulas of the ionic compounds formed from the following pairs of elements. Name each compound. a. \(\mathrm{Li}\) and \(\mathrm{N}\) c. \(\mathrm{Rb}\) and \(\mathrm{Cl}\) b. Ga and \(\mathrm{O}\) d. \(\mathrm{Ba}\) and \(\mathrm{S}\)

Short Answer

Expert verified
The empirical formulas and names of the ionic compounds are: a. \(\mathrm{Li_3N}\): Lithium nitride c. \(\mathrm{RbCl}\): Rubidium chloride b. \(\mathrm{Ga_2O_3}\): Gallium oxide d. \(\mathrm{BaS}\): Barium sulfide

Step by step solution

01

Identify the charges of the ions

Find the charges of the ions formed by the given elements. Elements in group 1 form +1 ions, group 2 form +2 ions, group 13 form +3 ions, group 15 form -3 ions, group 16 form -2 ions, and group 17 form -1 ions. a. Li is in group 1 (+1 ion) and N is in group 15 (-3 ion) c. Rb is in group 1 (+1 ion) and Cl is in group 17 (-1 ion) b. Ga is in group 13 (+3 ion) and O is in group 16 (-2 ion) d. Ba is in group 2 (+2 ion) and S is in group 16 (-2 ion)
02

Determine the empirical formula based on ion charges

Determine the ratio of cations to anions to create a neutral compound. The compound's empirical formula will have the lowest whole-number ratio of elements. a. Li (+1) and N (-3): We need three Li ions to balance one N ion, so the formula is \(\mathrm{Li_3N}\). c. Rb (+1) and Cl (-1): We need one Rb ion to balance one Cl ion, so the formula is \(\mathrm{RbCl}\). b. Ga (+3) and O (-2): We need two Ga ions to balance three O ions, so the formula is \(\mathrm{Ga_2O_3}\). d. Ba (+2) and S (-2): We need one Ba ion to balance one S ion, so the formula is \(\mathrm{BaS}\).
03

Name each compound

Following the IUPAC naming rules, name each compound, using the names of the cation followed by the anion. For the anion, use the ending -ide. a. \(\mathrm{Li_3N}\): Lithium nitride c. \(\mathrm{RbCl}\): Rubidium chloride b. \(\mathrm{Ga_2O_3}\): Gallium oxide d. \(\mathrm{BaS}\): Barium sulfide

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Most popular questions from this chapter

Arrange the following molecules from most to least polar and explain your order: \(\mathrm{CH}_{4}, \mathrm{CF}_{2} \mathrm{Cl}_{2}, \mathrm{CF}_{2} \mathrm{H}_{2}, \mathrm{CCl}_{4}\), and \(\mathrm{CCl}_{2} \mathrm{H}_{2}\).

Think of forming an ionic compound as three steps (this is a simplification, as with all models): (1) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three processes? d. Given your answer to part \(\mathrm{c}\), why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not \(\mathrm{Na}_{2} \mathrm{Cl} ? \mathrm{NaCl}_{2} ?\) What about \(\mathrm{MgO}\) compared to \(\mathrm{MgO}_{2} ?\) \(\mathrm{Mg}_{2} \mathrm{O} ?\)

Use the formal charge arguments to rationalize why \(\mathrm{BF}_{3}\) would not follow the octet rule.

For each of the following groups, place the atoms and/or ions in order of decreasing size. a. \(\mathrm{Cu}, \mathrm{Cu}^{+}, \mathrm{Cu}^{2+}\) b. \(\mathrm{Ni}^{2+}, \mathrm{Pd}^{2+}, \mathrm{Pt}^{2+}\) c. \(\mathrm{O}, \mathrm{O}^{-}, \mathrm{O}^{2-}\) d. \(\mathrm{La}^{3+}, \mathrm{Eu}^{3+}, \mathrm{Gd}^{3+}, \mathrm{Yb}^{3+}\) e. \(\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}, \mathrm{La}^{3+}\)

For each of the following, write an equation that corresponds to the energy given. a. lattice energy of \(\mathrm{NaCl}\) b. lattice energy of \(\mathrm{NH}_{4} \mathrm{Br}\) c. lattice energy of \(\mathrm{MgS}\) d. \(\mathrm{O}=\mathrm{O}\) double bond energy beginning with \(\mathrm{O}_{2}(g)\) as a reactant
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