Potassium iodide (KI) exhibits predominantly ionic bonding. The \(\mathrm{K}^{+}\)and \(\mathrm{I}^{-}\)ions have electron structures that are identical to which two inert gases?

Before calculating the ion's electron configurations, we need the electron configurations for potassium (K) and iodine (I). Potassium has 19 electrons \((\mathrm{Z} = 19)\) and it is located in Group 1 and Period 4, while iodine has 53 electrons \((\mathrm{Z} = 53)\) and it is located in Group 17 and Period 5. Their electron configurations are as follows: Potassium (K): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^1\) Iodine (I): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^2 3\mathrm{d}^{10} 4\mathrm{p}^6 5\mathrm{s}^2 4\mathrm{d}^{10} 5\mathrm{p}^5\)

When potassium forms the \(\mathrm{K}^{+}\) ion, it loses one electron from its outermost shell. The electron configuration of \(\mathrm{K}^{+}\) ion will be: \(\mathrm{K}^{+}\): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6\) When iodine forms the \(\mathrm{I}^{-}\) ion, it gains one electron in its outermost shell. The electron configuration of \(\mathrm{I}^{-}\) ion will be: \(\mathrm{I}^{-}\): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^2 3\mathrm{d}^{10} 4\mathrm{p}^6 5\mathrm{s}^2 4\mathrm{d}^{10} 5\mathrm{p}^6\)

Now, let's compare the electron configurations of the \(\mathrm{K}^{+}\) and \(\mathrm{I}^{-}\) ions with the electron configurations of inert gases. Inert gases have full outer electron shells, giving them a stable configuration. There are six inert gases: helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). Their electron configurations are: Helium (He): \(1\mathrm{s}^2\) Neon (Ne): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6\) Argon (Ar): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6\) Krypton (Kr): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^2 3\mathrm{d}^{10} 4\mathrm{p}^6\) Xenon (Xe): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^2 3\mathrm{d}^{10} 4\mathrm{p}^6 5\mathrm{s}^2 4\mathrm{d}^{10} 5\mathrm{p}^6\) Radon (Rn): \(1\mathrm{s}^2 2\mathrm{s}^2 2\mathrm{p}^6 3\mathrm{s}^2 3\mathrm{p}^6 4\mathrm{s}^2 3\mathrm{d}^{10} 4\mathrm{p}^6 5\mathrm{s}^2 4\mathrm{d}^{10} 5\mathrm{p}^6 6\mathrm{s}^2 4\mathrm{f}^{14} 5\mathrm{d}^{10} 6\mathrm{p}^6\) Comparing the electron configurations, we find that: - \(\mathrm{K}^{+}\) ion has the same electron configuration as Argon (Ar) - \(\mathrm{I}^{-}\) ion has the same electron configuration as Xenon (Xe)

The electron structures of \(\mathrm{K}^{+}\) and \(\mathrm{I}^{-}\) ions are identical to the electron structures of the inert gases Argon (Ar) and Xenon (Xe), respectively.