Aluminium crystallizes in a cubic close packed structure . Its metallic radius is 125 pm .
What is the length of the side of the unit cell .

Aluminium crystallizes in a cubic close packed structure . Its metallic radius is 125 pm . How many unit cells are there in 1.00 cm^(3) of aluminium.

Density of a unit cell is represented as rho=("Effectiveno.ofatom(s)x Mass of a unit cell")/("Volume of a unit cell")=(Z.M.)/(N_(A).a^(3)) Where, mass of unit cell = mass of effective no. of atom(s) or ion(s). M = At. wt./formula wt. N_(A)="Avogadro’s no. "rArr 6.023xx10^(23) a = edge length of unit cell Silver crystallizes in a foc lattice and has a density of 10.6g//cm^(3) ? What is the length of an edge of the unit cell?

The number of octahedral voids in a unit cell of cubic close packed structure is

Gold (atomic radius = 0.144 nm) crystallizes in a face centered unit cell . What is the length of a side of the unit cell ?

In a cubic close packed structure the number of nearest neighbours for a given lattice point is

In a cubic close packed structure the number of nearest neighbours for a given lattice point is

A substance forms f.c.c. crystal structure. Its density is 1.984 gm cm^(-1) and the length of the edge of the unit cell is 630 pm. Calculate the molar mass.

AgI crystallises in the cubic close-packed zinc blend structure. Assuming that the iodide ions occupy the lattice points, fraction of the tetrahedral sites occupies by sliver ions are