The formula for the determination of the density of a unit cell is:
- A$\frac{a^3 \times N_A}{Z \times M} \ g \ cm^{-3}$
- B$\frac{Z \times M}{a^3 \times N_A} \ g \ cm^{-3}$
- C$\frac{a^3 \times M}{Z \times N_A} \ g \ cm^{-3}$
- D$\frac{M \times N_A}{a^3 \times Z} \ g \ cm^{-3}$
Explore More
Similar Questions
$CsBr$ has $b.c.c.$ structure with edge length $4.3 \ \mathring{A}$. The shortest inter-ionic distance between $Cs^{+}$ and $Br^{-}$ is ........... $\mathring{A}$.
Medium
View Solution$A$ metal crystallizes in two phases,one as $fcc$ and another as $bcc$ with unit cell edge lengths of $3.5 \mathring{A}$ and $3.0 \mathring{A}$,respectively. The ratio of density of $fcc$ and $bcc$ phases approximately is
Nickel crystallises in a $fcc$ type of unit cell,with edge length $0.3524 \ nm$. Calculate the radius of nickel atom. (in $nm$)
Calculate the number of atoms in $5 \ g$ of a metal that crystallises in a simple cubic unit cell structure with an edge length of $336 \ pm$. (Density of the metal $= 9.4 \ g \ cm^{-3}$)
How many unit cells are present in a $1.00 \ g$ cube of ideal $NaCl$ crystal?
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo