Which of the following statement is incorrect according to crystal field theory?

The

N i^{2 +} (a q)

cation is coloured because

N i^{2 +}

ion can absorb light, which promotes electrons from the low energy d-orbitals to high energy d-orbitals.

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The

Z n^{2 +} (a q)

cation is colourless because the d-orbitals are completely filled and no electrons can be promoted, so on light is absorbed.

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A complex which has just one absorption band at

455 n m

, must be blue coloured.

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A complex which has just one absorption band at

425 n m

, must be yellow coloured.

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Solution

The correct option is C A complex which has just one absorption band at $455 n m$ , must be blue coloured.
$N i^{2 +}$ ion is coloured because it has unpaired electrons.
$Z n^{2 +}$ ion is colourless because it lacks unpaired electrons.
Complementary colour of the wavelength is observed for a complex.

Wavelength $425 n m$ corresponds to violet colour. Thus, its complement colour is yellow. Hence, compound appears as yellow colour.

The wavelength $455 n m$ corresponds to blue light. When a complex absorbs blue light, the colour observed is orange.
Thus, the complex appears orange. So, the statement in option $C$ is incorrect.

Hence, the correct option is $C$ .

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