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The Solid State

Question

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An element (At. mass 60) have face centred cubic structure has a density of 6.23 g cm^–3. What is the edge length of the unit cell?

Solution

Solution:
we have given that
Atomic mass of element = 60.
Number of atoms per fcc unit cell = 4
Density of the element = 6.23 g/cm³

= \frac{6.23}{10^{23}} g / (pm)^{3}

Density,

d = \frac{N \times M}{N_{A} \times a^{3}}

or

a^{3} = \frac{N \times M}{d \times N_{A}} = \frac{60 \times 4 \times 10^{30}}{6.23 \times 6.02 \times 10^{23}} = 64 \times 10^{6} (pm)^{3}

Therefore, edge of unit cell, a = 400 pm.

Some More Questions From The Solid State Chapter

What type of solids are electrical conductors, malleable and ductile?

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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