The cell edge of a fcc element of atomic mass 108 is 409 pm. Calculate its density.

Solution

we have given,.
mass =108 g
edge (a) = 409pm
a³ = 6.84 x10²³ cm³N_a =6.023 x10^-233Z =4

Apply formula

$d = \frac{Z xM}{a^{3} x N_{A}} d = \frac{4 x 108}{6.84 x 10^{23} x 6.02 x 10^{- 23}} = 10.98 g {cm}^{- 3}$

density = 10.98 g cm^–3

Some More Questions From The Solid State Chapter

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The Solid State

The cell edge of a fcc element of atomic mass 108 is 409 pm. Calculate its density.

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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