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Density of a unit cell is represented as
\( \rho=\frac{\text { Effective no. of atom }(\mathrm{s}) \times \text { Atomic mass } / \text { formula mass }}{\text { Volume of a unit cell }}=\frac{Z . M .}{N_{A} \cdot a^{3}} \)
where, mass of unit cell = mass of effective no. of atom(s) or ion(s).
\( M= \) At. mass/formula mass
\( \begin{aligned} N_{A} &=\text { Avogadro's no. } \Rightarrow 6.023 \times 10^{23} \\ a &=\text { edge length of unit cell } \end{aligned} \)
The density of \( \mathrm{KBr} \) is \( 2.75 \mathrm{~g} / \mathrm{cm}^{-3} \). The length of the edge of the unit cell is \( 654 \mathrm{pm} \). To which type of cubic crystal, KBr belongs?
(a) simple cubic
(b) bcc
(c) fcc
(d) none of these
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