Problem 49
Write electron configurations for a. the cations \(\mathrm{Mg}^{2+}, \mathrm{K}^{+},\) and \(\mathrm{Al}^{3+}\) . b. the anions \(\mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^{-},\) and \(\mathrm{Te}^{2-}\)
Problem 50
Write electron configurations for a. the cations \(\mathrm{Sr}^{2+}, \mathrm{Cs}^{+}, \mathrm{In}^{+},\) and \(\mathrm{Pb}^{2+} .\) b. the anions \(\mathrm{P}^{3-}, \mathrm{S}^{2-},\) and \(\mathrm{Br}^{-}\)
Problem 52
What noble gas has the same election configuration as each of the ions in the following compounds? a. cesium sulfide \(\quad\) c. calcium nitride b. strontium fluoride \(\quad\) d. aluminum bromide
Problem 53
Give the formula of a negative ion that would have the same number of electrons as each of the following positive ions. a. \(\mathrm{Na}^{+} \quad\) c. \(\mathrm{Al}^{3+}\) b. \(\mathrm{Ca}^{2+} \quad\) d. \(\mathrm{Rb}^{+}\)
Problem 54
Give an example of an ionic compound where both the anion and the cation are isoelectronic with each of the following noble gases. a. \(\mathrm{Ne} \quad\) c. \(\mathrm{Kr}\) b. \(\mathrm{Ar} \quad\) d. \(\mathrm{Xe}\)
Problem 55
Give three ions that are isoelectronic with krypton. Place these ions in order of increasing size.
Problem 57
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. \(\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}, \mathrm{La}^{3+}\)
Problem 58
For each of the following groups, place the atoms and/or ions in order of decreasing size. a. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}, \mathrm{V}^{5+}\) b. \(\mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Cs}^{+}\) c. \(\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}\) d. \(\mathrm{P}, \mathrm{P}^{-}, \mathrm{P}^{2-}, \mathrm{P}^{3-}\) e. \(\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}, \mathrm{Te}^{2-}\)
Problem 59
Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl} \quad\) d. Fe \((\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) b. \(\mathrm{LiF}, \mathrm{LiCl} \quad\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO} \quad\) f. \(\mathrm{MgO}, \mathrm{BaS}\)
Problem 60
Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers a. \(\mathrm{LiF}, \mathrm{CsF} \quad\) d. \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{CaSO}_{4}\) b. \(\mathrm{NaBr}, \mathrm{Nal} \quad\) e. \(\mathrm{KF}, \mathrm{K}_{2} \mathrm{O}\) c. \(\mathrm{BaCl}_{2}, \mathrm{BaO} \quad\) f. \(\mathrm{Li}_{2} \mathrm{O}, \mathrm{Na}_{2} \mathrm{S}\)
