Solid State Tes...

A compound $$AB$$ has rock salt type structure. The formula weight of $$AB$$ is $$6.023 \ Y$$ amu, and closest $$A-B$$ distance is $$Y^{1/3}$$ nm, where $$Y$$ is an arbitrary number, find the density of the lattice.

Potassium has a bcc structure wit nearest neighbour distance $$4.52A^0$$, its atomic weight is $$39$$. Its density (in kg $$m^{-1}$$) will be:

The maximum radius of sphere that can be fitted in the octahedral hole of cubical closed packing of sphere of radius $$r$$ is:

A solid $$X^+Y^-$$ has a bcc structure. If the distance of closest approach between the two atoms is $$173$$ pm, the edge length of the cell is:

The unit cell length of $$NaCl$$ is observed to be $$0.5627$$ nm by X-ray difference studies; the measured density of $$NaCl$$ is $$2.164$$g $$cm^{-3}$$/ Calculate the difference of observed and calculated density. lso calculate $$\%$$ is missing $$Na^+$$ and $$Cl^-$$ ions:

The number of unit cells in $$58.5$$ g of $$NaCl$$ is nearly ?

A crystalline solid $$AB$$ adopts sodium chloride type structure with edge length of the unit cell as 745 pm and formula mass of 74.5 a.m.u. The density of the crystalline compound is:

The fraction of octahedral voids filled by $$A{l^{3 + }}$$ ions in $$A{l_2}{O_3}\left( {{r_{Al^{3 \oplus }}}}/r_{O^{2 - }} = 0.43 \right)$$ is:

Polonium crystallizes in a simple cubic structure. The edge of the unit cell is $$0.236$$ nm. What is the radius of the polonium atom?

In the crystal $$A^{2+}B^{2-}$$, having anions in the face centred cubic packing if the radius of the anion if $$1.84A^0$$, ideal radius of the cation present in the tetrahedral hole will be: