Analysis show that nickel oxide consists of nickel ion with `96%` ions having `d^(8)` configuration and `4%` having `d^(7)` configuration. Which amongst the following best represents the formula of the oxide?

Options

A. `Ni_(1.02)O_(1.00)`
B. `Ni_(0.96)O_(1.00)`
C. `Ni_(0.98)O_(0.98)`
D. `Ni_(0.98)O_(1.00)`

Explanation

`Ni=3d^(8)4s^(2)` (At.no.=28)
`therefore Ni^(2+)=3d^(8)` and `Ni^(3+)=3d^(7)`
Hence, 96^ ion of `Ni^(2+)` and 4% ions of `Ni^(3+)` are present,
Let number of `O^(2-)` ion present in the crystal =x. Applying electroneutraility rule,
Total positive charge =Total negative charge `96xx2` (+ve charge)`+4xx3`(+ve charge)`=x xx 2`(-ve charge)
`therefore 96xx2+4xx3-2x=0rArrx=1.02`
So formula of crystal
`Ni_(1.00)O_(1.02)` or `Ni_(1.00)` or `Ni_(0.98)O_(1.00)`.