91Ó°ÊÓ

Write the electron configuration for each ion. $$ \text { a. } \mathrm{Cl}^{-} \quad \text { b. } \mathrm{P}^{3-} \quad \text { c. } \mathrm{K}^{+} \quad \text { d. } \mathrm{Mo}^{3+} \quad \text { e. } \mathrm{V}^{3+} $$

Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. $$ \text { a. } \mathrm{Cd}^{2+} \quad \text { b. } \mathrm{Au}^{+} \quad \text { c. } \mathrm{Mo}^{3+} \quad \text { d. } \mathrm{Zr}^{2+} $$

Which is the larger species in each pair? $$ \text { b. Li or Li}^{+} \quad \text { b. } I^{-} \text { or } C s^{+} \quad \text { c. Cr or } C r^{3+} \quad \text { d. } \text { O or } O^{2-} $$

Which is the larger species in each pair? $$ \text { a. Sr or }\mathrm{Sr}^{2+} \quad \text { b. N} \text { or N} ^{3-} \quad \text { c. Ni or }\mathrm{Ni}^{2+} \quad \text { d. } \mathrm{S}^{2-} \text { or } \mathrm{Ca}^{2+} $$

Arrange this isoelectronic series in order of decreasing radius: \(\mathbf{F}^{-}, \mathrm{Ne}\) \(\mathrm{O}^{2}, \mathrm{Mg}^{2+}, \mathrm{Na}^{+} .\)

Arrange this isoelectronic series in order of increasing atomic radius: \(\mathrm{Se}^{2-}, \mathrm{Kr}, \mathrm{Sr}^{2+}, \mathrm{Rb}^{+}, \mathrm{Br}^{-} .\)

Choose the element with the higher first ionization energy in each pair. $$ \text {a. Br or Bi} \quad \text {b. Na or Rb} \quad \text {c. As or At} \quad \text {d. P or Sn} $$

Choose the element with the higher first ionization energy in each pair. $$ \text {a. P or I} \quad \text {b. Si or Cl} \quad \text {c. P or Sb} \quad \text {d. Ga or Ge} $$

Arrange these elements in order of increasing first ionization energy: \(\mathrm{Si,}\) \(\mathrm{F,}\) \(\mathrm{In,}\) \(\mathrm{N.}\)

Arrange these elements in order of decreasing first ionization energy: \(\mathrm{Cl}\) , \(\mathrm{S}, \mathrm{Sn}, \mathrm{Pb} .\)