The hybridization involved in complex `[Ni(CN)_(4)]^(2-)` is `(At. No . Ni = 28)`

Options

A. `d^(2)sp^(2)`
B. `d^(2)sp^(3)`
C. `dsp^(2)`
D. `sp^(3)`

Answer

C

Explanation

Here nickel is in `+2` oxidation state has the electronnc configuration `3d^(8)` . Since `CN^(-)` ion is a strong field lignd, the electronic configuration is reshuffled to pair up all the electrons so as to provide one empty orbital for `dsp^(2)` hybrization.


`[Ni(CN)_(4)]^(2-)`

Four pairs of form `4CN^(-)` ligands electrons
Each of the hybridised orbitals receives a pair of electrons form a cyanide ion.