Problem 61
Name the ions with three charges that have the following electron configurations: (a) [Ar]3d^{3} , ( b ) \text { [Ar], } (c) \([\mathrm{Kr}] 4 d^{6}\) (d) \([\operatorname{Xe}] 4 f^{14} 5 d^{6}\)
Problem 62
Which of the following species are isoelectronic with each other: \(\mathrm{C}, \mathrm{Cl}^{-}, \mathrm{Mn}^{2+}, \mathrm{B}^{-}, \mathrm{Ar}, \mathrm{Zn}, \mathrm{Fe}^{3+}, \mathrm{Ge}^{2+} ?\)
Problem 63
Define ionic radius. How does the size of an atom change when it is converted to (a) an anion and (b) a cation?
Problem 64
Explain why, for isoelectronic ions, the anions are larger than the cations.
Problem 65
Indicate which one of the two species in each of the following pairs is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-}\). (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+}\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\)
Problem 66
$$ \begin{aligned} &\text { List the following ions in order of increasing ionic }\\\ &\text { radius: } \mathrm{N}^{3-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{Mg}^{2+}, \mathrm{O}^{2-} \end{aligned} $$
Problem 67
$$ \begin{aligned} &\text { Explain which of the following cations is larger, and }\\\ &\text { why: } \mathrm{Cu}^{+} \text {or } \mathrm{Cu}^{2+} \end{aligned} $$
Problem 68
$$ \begin{aligned} &\text { Explain which of the following anions is larger, and }\\\ &\text { why: } \mathrm{Se}^{2-} \text { or } \mathrm{Te}^{2-} \text { . } \end{aligned} $$
Problem 69
Why do members of a group exhibit similar chemical properties?
Problem 72
Give the physical states (gas, liquid, or solid) of the main group elements in the fourth period \((\mathrm{K}, \mathrm{Ca}, \mathrm{Ga},\) Ge, As, Se, Br) at room temperature.
