A cubic unit cell contains manganese ions \(Mn^{+3}\) at the corners and fluoride ions at the centre of each edge. If the radius of \(Mn^{+3}\) ion is 0.65 \(A^{o}\) and that of \(F^{-}\) ion is 1.35 \(A^{o}\). The density of solid is [(Mn=55,F=19,\(N_{A}=6\times10^{23}\)

A cubic unit cell contains manganese ions at the corners and fluoride ions at the centre of each face. (a) What is the empirical formula ? (b) What is the C.N. of Mn^(2+) ion ? (c) Calculate the edge length of the unit cell if the radius of Mn^(2+) ion is 0.65Å and that of F^(-) ion is 1.36Å .

If the length of the body for CaCl which crystallizes into a cubic strructure with Cl^(Θ) ions at the corners and Cs^(o+) ions at the centre of the unit cell is 7 Å and the radius of he Cs^(o+) ions is 1.69Å , what is the radius of Cl^(ɵ) ions?

The number of manganeses ions in tetrahedral and octahedral sites respectively in Mn_3O_4 are

BaTiO_(3) has perovskite structure with Ba^(2+) ions at the corners O^(2-) ions at the center of each face and Ti^(4) ions at the center of a cubic unit cell.What is the number of Ti^(4+) ions nearest to Ba^(2+) ion?

Write electronic configuration of Fe^(2+) , Mn^(4+) , n^(3-) and O^(2-) ions .

The well know mineral flourite is chemically calcium fluoride. It is a well known fact that in one unit cell of this mineral, there are four Ca^(2+) ions and eight F^(-) ions and Ca^(2+) ions are arranged in f.c.c. lattice. The F^(-) ions fill all the tetrahedral holes in the face centred cubic lattice of Ca^(2+) ions. The edge length of the unit cell is 5.46xx10^(-8) cm. The density of the solid is 3.18"g cm"^(-3) . Use this information to calculate Avogadro's number (Molar mass of CaF_(2)=78.0"g mol"^(-1) )

In CsCl with cubic structure, Cl^(-) ions are located at each corner and Cs^(+) ions at the centre of the unit cell. If r_(Cs^(+)) and r_(Cl^(-)) and 1.69Å and 1.81Å respectively. Find the value of edge length of cube.