Calculate the efficiency of packing in case of a metal crystal for face centred cubic lattice.

Calculate the efficiency of packing in case of a metal crystal for body centred cubic lattice.

Calculate the efficiency of packing in case of a metal crystal for: body-centred cubic

Calculate the efficiency of packing in case of a metal crystal for: face-centred cubic (with the assumptions that atoms are touching each other).

Calculate the efficiency of packing in case of a metal crystal for: Simple cubic

Calculate tbe packing efficiency of a metal crystal for a simple cubic lattice.

Calculate the atomic radius of elementary silver which crsytallises in face centred cubic lattice with unit cell edge length 4.086xx10^-10m .

Calculate the density of silver which crystallines in the face centred cubic structure. The distance between the nearest silver atoms in this structure is 287 pm. ( Molar mass of silver=107.87 g mol^-1 ).

CsCl has body centred cubic lattice with the lengh of a side of a unit cell 412.1 pm and aluminium is face centred cubic lattice with length of the side of unit cell 405 pm. Which of the two larger density? (Atomic mass of Cs=132.9, Cl=29.9).

The well known mineral fluorite is chemically clacium fluoride. Its is known that in one unit cell of this mineral there are 4 Ca^(2+) ions and 8 F^- ions and that of Ca^(2+) ions are arranged in a fcc lattice. The F^- ions fill all the tetrahedral holes in the face centred cubic lattice of Ca^(2+) ions. the edge of hte unit cell is 5.46xx10^-8 cm in length. the density of the solid is 3.18 gcm^-3 . use this information to calculate the Avagadro's number. (Molar mass of CaF_2=70.08 g mol^-1 ).