A copper complex crystallising in a CCP lattice with a cell edge of 0.4518 nm has been revealed by employing X-ray diffraction studies. The density of a copper complex is found to be 7.62 g cm^–3. The molar mass of copper complex is _____g mol^–1. [Given: NA = 6.022 × 1023 mol^–1]

Given, CCP lattice with a cell edge of 0.4518 nm
We need to find the molar mass of copper complex.

A copper complex's density is equal to= 7.62gcm⁻³, N_A= 6.022×10²³ mol⁻¹,a=0.4518 nm, Z=4
Knowing the d = $\frac{\mathrm{Z}\times \mathrm{M}}{\mathrm{a}\times {\mathrm{N}}_{\mathrm{A}}}$
fcc structure of the CCP lattice:
Atoms are present at the corners and face centres of a fcc unit cell:
Quantity of atoms in a single cell is $\left(8\times \frac{1}{8}\right)+\left(6\times \frac{1}{2}\right)=4$
$7.62=\frac{4\times \mathrm{M}}{{\left(0.4518\times {10}^{-7}\right)}^3\times 6.022\times {10}^{23}}=\mathrm{M} = 105.8 \simeq 106 \mathrm{g}/\mathrm{mol}$

Therefore the correct answer is 106