An element X with an atomic mass of `60g mol^-1` 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.

Explanation

`M=60 g mol^-1` density `d=6.23 g cm^-3`, edge length, a = 400 pm
`Z=dxa^3xxN_A//M=4`
Since z is 4 it means the element crystallizes in fcc lattice, radius of atom, `r=a//2(2)^(1//2)=141.4 "pm"`.