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Q.
Aluminium metal has a density of $2.72\, g\, cm ^{-3}$ and crystallizes in a cubic lattice with an edge of $404\, pm$. Which is/are correct?
The Solid State
Solution:
Use any relation:
$\rho=\frac{Z_{ eff } \times A w}{N_{ A } \times a^3} \text { orp }=\frac{Z_{ eff } \times A w \times 1.67 \times 10^{-24} g }{a^3} $
$\therefore 2.72\, g\, cm ^{-3}=\frac{Z_{ eff } \times 27 \times 1.67 \times 10^{-24} g }{\left(404 \times 10^{-10}\right)^3 cm ^3}$
$\therefore Z_{ eff } \approx 4$
a. $Z_{ eff }=4$, means fcc structure
d. CN of fcc structure $=12$