If the edge length of its unit cell is 3...

If the edge length of its unit cell is 300 pm, determine the type of unit cell when an element has atomic mass `93 g mol^(-1) ` and density `11.5 g cm^(-3)` .

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Silver has atomic mass 108 a.m.u. and density 10.5 g cm^(-3) . If the edge length of its unit cell is 409 pm, identify the type of unit cell. Also calculate the radius of an atom of silver.

(a) 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. (b) Write any two differences between amorphous solids and crystalline solids.

Sodium crystallises in a cubic lattice and the edge length of the unit cell is 430 pm. Calculate the number of atoms in the unit cell. (Atomic mass Na = 23 amu, Density of Na = 0.9623 g cm^(-3) )

The edge length of NaCl unit cell is 564 pm. What is the density of NaCl in g/ cm^(3) ?

A element X with atomic mass 60 g/mol has a density of 6.23"g cm"^(-3) . If the edge length of the unit cell is 400 pm, identify the type of the cubic unit cell. Calculate the radius of the atoms of the element.

The density of chromium metal is 7.2 g cm^(-3) . If the unit cell is cubic with edge length of 289 pm, determine the type of unit cell (simple , body centred or face centred) [Atomic mass of Cr = 52 a.m.u., N_A = 6.02 xx 10^(23) mol^(-1)] .

Density of KBr is 2.75 g//cm^3 . The edge length of unit cell is 654pm. Find the type of unit cell of KBr (At.mass of K=39 and Br=80)

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