An element with cell edge of 288 pm has a density of 7.2 g cm^-3. What type of structure does the element have if it’s atomic mass M=51.8 g mol^-1?(a) Body-Centred Cubic (BCC)(b) Face-Centred Cubic (FCC)(c) Simple Cubic(d) Hexagonal Closed Packing (HCP)The question was asked during an internship interview.The doubt is from Solid State topic in portion Solid State of Chemistry – Class 12

An element with cell edge of 288 pm has a density of 7.2 g cm^-3. What

1.	An element with cell edge of 288 pm has a density of 7.2 g cm^-3. What type of structure does the element have if it’s atomic mass M=51.8 g mol^-1?(a) Body-Centred Cubic (BCC)(b) Face-Centred Cubic (FCC)(c) Simple Cubic(d) Hexagonal Closed Packing (HCP)The question was asked during an internship interview.The doubt is from Solid State topic in portion Solid State of Chemistry – Class 12
Answer» Correct answer is (a) Body-Centred Cubic (BCC) For explanation I would say: Given, Edge length (a) = 288 pm Density (ρ) =7.2 g cm^-3 Atomic mass (M) = 51.8 g mol^-1 Avogadro’s number (N0) = 6.02 X 10^23 We know, (ρ) = (Z x M)/(a^3 x N0) Or Z =(ρ x a^3 x N0)/M = (7.2 x (288 x 10^-10) ^3 x 6.02 x 10^23)/51.8 Z = 2 Therefore, the ELEMENT has Body-Centred Cubic (BCC) type of structure.

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