Chromium crystallizes in bcc structure if its edgelength is 300 picometre find its density atomic mass of chromium is 52 you
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In a BCC lattice, The atoms touch each other along with there body-diagonal of the cube.
Hence
The BCC crystal atomic radius r = √3a/4
Where a= edge
density= Mass per unit cell/Volume of Unit Cell
= z*atomic mass/NA x a3
Where as z=2
NA = Avogadro constant = 6.022x10²³
On Substituting the values
Volume of unit cell = a³ = (300 pm³)
= (300*10-10 cm³)³
Density = 2*52/6.022x10²³× (3.00*10-10 cm³)³
=10.0 g cm³
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