Give the oxidation number for the central atom or ion in...

Give the oxidation number for the central atom or ion in each of the following complexes. (a) $\mathrm{K}_{2}\left[\mathrm{Pt}\left(\mathrm{NO}_{2}\right)_{4}\right]$ (b) $\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]$ (c) $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{I}$ (d) $\mathrm{K}_{4}\left[\mathrm{Ni}(\mathrm{CN})_{6}\right]$ (e) $\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{2}$ (f) $\mathrm{Na}\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{OH})_{4}\right]$

Give the oxidation number for the central atom or ion in each of the following complexes.
(a) $\mathrm{K}_{2}\left[\mathrm{Pt}\left(\mathrm{NO}_{2}\right)_{4}\right]$
(b) $\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]$
(c) $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{I}$
(d) $\mathrm{K}_{4}\left[\mathrm{Ni}(\mathrm{CN})_{6}\right]$
(e) $\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{2}$
(f) $\mathrm{Na}\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{OH})_{4}\right]$

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Key Concepts

Ligand Charges

Ligands can be neutral, anionic, or cationic, and their inherent charges play a critical role in determining the oxidation state of the central metal atom. Understanding whether a ligand donates a neutral or charged entity helps in calculating the overall charge of the complex.

Charge Balance

To determine the oxidation number of the central metal atom in a coordination complex, one must account for the charges on all the ligands and any external counter ions. The sum of these charges, combined with the metal’s oxidation state, should equal the overall charge of the complex.

Oxidation Number

This is the hypothetical charge that an atom would have if all bonds to atoms of different elements were completely ionic. It is a useful bookkeeping tool used to keep track of electron transfers in redox reactions, as well as to compare and balance chemical equations.

Coordination Complexes

These are compounds formed when a metal ion binds to a group of atoms or molecules called ligands, which donate electron pairs to the metal. Studying the oxidation state of the central metal ion is crucial in coordination chemistry as it influences the structure, reactivity, and properties of the complex.

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