The cubic unit cell of a metal (molar mass = | vedclass

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(B) The density formula is given by $d = \frac{Z M}{N_A a^3}$,where $Z$ is the number of atoms per unit cell,$M$ is the molar mass,$N_A$ is Avogadro's

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face centred

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(B) The density formula is given by $d = \frac{Z M}{N_A a^3}$,where $Z$ is the number of atoms per unit cell,$M$ is the molar mass,$N_A$ is Avogadro's constant $(6.022 	imes 10^{23} \ mol^{-1})$,and $a$ is the edge length.Rearranging for $Z$: $Z = \frac{d N_A a^3}{M}$.Given: $d = 8.92 \ g \ cm^{-3}$,$M = 63.55 \ g \ mol^{-1}$,$a = 362 \ pm = 362 	imes 10^{-10} \ cm$.Substituting the values: $Z = \frac{8.92 	imes 6.022 	imes 10^{23} 	imes (362 	imes 10^{-10})^3}{63.55}$.$Z \approx \frac{8.92 	imes 6.022 	imes 10^{23} 	imes 47.458 	imes 10^{-24}}{63.55} \approx 4.01$.Since $Z = 4$,the unit cell is face-centred cubic $(FCC)$.

The cubic unit cell of a metal (molar mass $= 63.55 \ g \ mol^{-1}$) has an edge length of $362 \ pm$. Its density is $8.92 \ g \ cm^{-3}$. The type of unit cell is

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