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# Write the ground-state electron configurations of the following transition metal ions: (a) $\mathrm{Sc^{3+}}$, (b) $\mathrm{Ti^{4+}}$, (c) $\mathrm{V^{5+}}$, (d) $\mathrm{Cr^{3+}}$, (e) $\mathrm{Mn^{2+}}$, (f) $\mathrm{Fe^{2+}}$, (g) $\mathrm{Fe^{3+}}$, (h) $\mathrm{Co^{2+}}$, (i) $\mathrm{Ni^{2+}}$, (j) $\mathrm{Cu^{+}}$, (k) $\mathrm{Cu^{2+}}$, (l) $\mathrm{Ag^{+}}$, (m) $\mathrm{Au^{+}}$, (n) $\mathrm{Au^{3+}}$, (o) $\mathrm{Pt^{2+}}$.

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PART A:

Write the electron configuration for an uncharged scandium atom using noble gas notation. By inspection of the periodic table, the noble gas preceding scandium is argon. Use brackets to denote these filled inner subshells. Then write the remaining subshells in the order in which they are filled.

$\mathrm{Sc}$: $\left[\text{Ar}\right]4s^23d^1$

Write the electron configuration for the $\mathrm{Sc^{3+}}$ ion. For transition metals, the charge of the cation indicates the number of electrons (three) that must be removed from the uncharged atom. This is done by first removing electrons from the outermost $s$ subshell before removing electrons from the outermost $d$ subshell.

$\mathrm{Sc^{3+}}$: $\left[\text{Ar}\right]$

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