Provide the IUPAC names for the following coordination compounds: i. [CrCl2(H2O)4]NO3 ii. [Pd(ONO)2(H2O)2I2] iii. (NH4)3[Fe(CN)6]

Chloro ($\text{Cl}^-$) has a -1 charge, aqua ($\text{H}_2\text{O}$) is neutral. The counter ion is nitrate ($\text{NO}_3^-$), which has a -1 charge.

Ligands are named alphabetically: aqua, chloro.
Name: Dichlorotetraaquachromium(III) nitrate

Nitrito-O ($\text{ONO}^-$) has a -1 charge, aqua ($\text{H}_2\text{O}$) is neutral, iodo ($\text{I}^-$) has a -1 charge. This is a neutral complex.

Ligands are named alphabetically: aqua, iodo, nitrito-O.
Name: Diaquadiododinitrito-O-palladium(IV)

The cation is ammonium ($\text{NH}_4^+$). The ligand is cyano ($\text{CN}^-$), which has a -1 charge.

Since there are three $\text{NH}_4^+$ ions, the complex anion must have a -3 charge.

The metal in an anionic complex ends with "-ate".
Name: Ammonium hexacyanoferrate(III)

The cation is ammonium ($\text{NH}_4^+$). The ligand is cyano ($\text{CN}^-$), which has a -1 charge.

Since there are four $\text{NH}_4^+$ ions, the complex anion must have a -4 charge.

The metal in an anionic complex ends with "-ate".
Name: Ammonium hexacyanoferrate(II)

The ligand is ammine ($\text{NH}_3$), which is neutral. The counter ion is bromide ($\text{Br}^-$), which has a -1 charge.

Since there are three $\text{Br}^-$ ions, the complex cation must have a +3 charge.

Name: Hexaamminechromium(III) bromide

Cyano ($\text{CN}^-$) has a -1 charge, nitrito-O ($\text{ONO}^-$) has a -1 charge, ammine ($\text{NH}_3$) is neutral. This is a neutral complex.