Question

The Correct name of \[[Pt{(N{H_3})_4}C{l_2}][PtC{l_4}]\]

1. tetraamminedichloroplatinum(IV) tetrachloroplatinate(II)
2. dichlorotetraammineplatinum(IV) tetrachloroplatinate(II)
3. tetrachloroplatinate(II) tetraammineplatinum(IV)
4. tetrachloroplatinate(II) dichloro tetraamine platinum(IV)

Answer 1

Hint: Write the name of the double complex salt as cation first and then anion. The ligand names are written in alphabetical order. The total charge on the cation should be neutralised by the total charge on the anion.

Complete step by step answer:
Let us break down the complex \[[Pt{(N{H_3})_4}C{l_2}][PtC{l_4}]\] into its corresponding anion and cation.

Cation: ${[Pt{(N{H_3})_4}C{l_2}]^{ + 2}}$
We have two ligands in this complex; one is chlorine and the other one is Ammine
These ligands will be named in alphabetical order and the prefix used will be the number of those species in the complex. The last would be the name of the metal followed by its oxidation state.
$\therefore $The name of this complex will be:
tetraamminedichloroplatinum(IV) ion

Anion: ${[PtC{l_4}]^{ - 2}}$
The naming of the anion complex is the same as that of the cation complex. The only difference is that in the anion, the name of the metal is written in its Latin origin and with the “ate” suffix. For example: Platinum becomes Platinate, Silver becomes Argentate.
$\therefore $The name of this complex will be tetrachloroplatinate(II) ion

Hence, the name of the double complex salt will be: tetraamminedichloridoplatinum(IV) tetrachloridoplatinate(II)

Note:
The oxidation number of platinum cannot be determined by only considering individual ions. This will lead to calculation error. Since the complex is electrically neutral, it means the anion complex and the cation complex have a charge which is equal in magnitude and opposite electrically.
Do not forget to mention the ion when mentioning individual cationic and anionic species.