In a hexagonal-close-pack (hcp) unit cell, the ratio of lattice points to octahedral holes to tetrahedral holes is 1: 1: 2. what is the general formula for a compound if anions occupy the hcp lattice points and cations occupy half of the tetrahedral holes? ab a3b ab2 a2b what is the general formula for a compound if anions occupy the hcp lattice points and cations occupy all the tetrahedral holes? ab a2b ab2 a3b

Explanation:

In a hexagonal-close-pack (HCP) unit cell, the ratio of lattice points to octahedral holes to tetrahedral holes =  1 : 1 : 2

let the :

Number of lattice point = 1x.

Number of octahedral points = 1x

Number of tetrahedral  points = 2x

If anions occupy the HCP lattice points and cations occupy half of the tetrahedral holes.

Number of anions occupying the HCP lattice points, A= 1x

Number of cations occupying the tetrahedral points, B =  

The formula of the compound will be =

If anions occupy the HCP lattice points and cations occupy all of the tetrahedral holes.

Number of anions occupying the HCP lattice points, A= 1x

Number of cations occupying the tetrahedral points, B =  2x

The formula of the compound will be =

it is a good conductor

explanation:

your answer would be “dry”