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Question
An element has atomic mass 93 g mol–1 and density 11.5 g cm–3. If the edge length of its unit cell is 300 pm, identify the type of unit cell
Solution
Given;
M = 93 g mol-1
d = 11.5 g cm-3
a = 300 pm = 300×10-10cm = 3×10-8 cm
We know that
`d = (Z XX M)/(N_A xx a^3)`
`Z = (d xx N_A xx a^3)/M = (11.5 xx 6.022 xx 10^23 (3 xx 10^(-8))^3)/93`
= 2.01 (approx)
As the number of atoms present in given unit cells are coming nearly equal to 2, hence the given unit cell is body centred cubic unit cell (BCC).
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