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The Solid State

Question

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An element with molar mass 2.7 x 10^–2kg mol^–1 form a cubic unit cell with edge length 405 pm. If its density is 2.7 x 10³ kg m^–3. What is the nature of the cubic unit cell?

Solution

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

Hence, the nature of the cubic unit cell is ccp.

Some More Questions From The Solid State Chapter

Ionic solids conduct electricity in liquid state but not in solid state. Explain.

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?

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