﻿ An element X with an atomic mass of 60 g/mol has density of 6.23 g/cm–3. If the edge length of its cubic unit cell is 400 pm, identify the type of cubic unit cell. Calculate the radius of an atom of this element. from Chemistry The Solid State Class 12 Nagaland Board

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Class 10 Class 12
An element X with an atomic mass of 60 g/mol has density of 6.23 g/cm–3. If the edge length of its cubic unit cell is 400 pm, identify the type of cubic unit cell. Calculate the radius of an atom of this element.

Solution:
we have given that
Density, d = 6.23 g/cm3
a = 400 pm
M = 60g/mol-1

Volume  = (a3)

$\mathrm{Z}=\frac{\mathrm{d}×{\mathrm{a}}^{3}×{\mathrm{N}}_{\mathrm{A}}}{\mathrm{M}}$

Hence, the type of cubic unit cell is FCC

So radius of element is 141.4 pm

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