In the complex $[P t {(p y)}_{4}] [P t C l_{4}],$ the oxidation numbers of Pt atom in former and later part of the compound are respectively :

0 and 0

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+4 and +2

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+2 and +2

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0 and +4

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Solution

The correct option is C +2 and +2
To balance the -4 charges of chloride ions each platinum atom will exhibit +2 oxidation state as $(p y)_{4}$ has no charge.
Let the charge of Pt is $x$ . As the compound is neutral, therefore, total charge is 0. Chlorine has -1 charge.
$2 x - 4 = 0$
$⟹ x = + 2$
IUPAC name of the given complex tetrapyridineplatinum(II) tetrachloroplatinate(II).

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