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The Solid State

Question

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A metal (at. mass = 50) has a bcc crystal structure. The density of the metal is 5.96 g cm^–3. Find the volume of its unit cell?

Solution

Solution:
We have given that
Atomic mass of the metal = 50g
bcc unit cell, Z = 2
Density of metal = 5.96 g/cm³Therefore, volume of the unit,

a^{3} = \frac{M \times Z}{N_{A} \times d} = \frac{50 \times 2}{6.02 \times 10^{23} \times 5.96} = 2.787 \times 10^{- 23} {cm}^{3}

Some More Questions From The Solid State Chapter

Give the significance of a 'lattice point'.

Name the parameters that characterize a unit cell.

Distinguish between Hexagonal and monoclinic unit cells.

Distinguish between Face-centred and end-centred unit cells.

What is the two-dimensional coordination number of a molecule in square close packed layer ?

A compound is formed by two elements M and N. The element N forms ccp and atoms of M occupy 1/3 of tetrahedral voids. What is the formula of the compound?

Which of the following lattices has the highest packing efficiency:

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