In a solid, oxide ions are arrnged in ccp, cations A occupy A occupy `(1/8)^th` of the tetrahedral voids and cation B occupy `(1/4)^(th)` of the octahedral voids. The formula of the compound is:

In certain solid, the oxide ions are arranged in ccp. Cations A occupy (1)/(6) of the tetrahedral voids and cations B occupy one third of the octahedral voids. The probable formula of the compound is

In certain solid, the oxide ions are arranged in ccp. Cations A occupy (1)/(6) of the tetrahedral voids and cations B occupy one third of the octahedral voids. The probable formula of the compound is

In a solid, oxide ions are arranged in ccp. Cations 'A' occupy one - sixth of the tetrahedral voids and cations 'B' occupy one - third of the octahedral voids. Which of the following is the correct formula of the oxide?

In a solid ,oxide (O^(2-)) ions are arranged in ccp, cations (A^(3+)) occupy one -fourth of tetrahedral void and cations (B^(3+)) occupy half of the octahedral voids . What is the formula of the compound?

In a compound,oxide ions are arranged in cubic close packing arrangement. Cations A occupy one-sixth of the tetrahdral voids and cations B occupy one-third of the octahedral voids. The formula of the compound is

In a compound,oxide ions are arranged in cubic close packing arrangement. Cations A occupy one-sixth of the tetrahdral voids and cations B occupy one-third of the octahedral voids. The formula of the compound is

In a solid ,oxide (O^(2-)) ions are arranged in ccp, cations (A^(3+)) occupy one -sixth of tetrahedral void and cations (B^(3+)) occupy one -third of the octahedral voids . What is the formula of the compound?

In a solid ,oxide (O^(2-)) ions are arranged in ccp, cations (A^(3+)) occupy one -sixth of tetrahedral void and cations (B^(3+)) occupy one -third of the octahedral voids . What is the formula of the compound?