A) \[A{{B}_{3}}\]
B) \[{{A}_{2}}B\]
C) \[{{A}_{3}}{{B}_{4}}\]
D) \[{{A}_{4}}{{B}_{3}}\]
Correct Answer: D
Solution :
[d]| The element B forms ccp lattice which means the number of atom \[B=4\] |
| Also, A occupies 2/3rd of tetrahedral voids. So, the number of tetrahedral voids formed in any unit cell \[=2\,Z\] (where, \[Z=\] number of atoms in unit cell) \[=2\times 4=8\] |
| Since, A occupies 2/3rd of tetrahedral voids, the number of atom \[A=\frac{2}{3}\times 8=\frac{16}{3}.\] |
| So, \[A=\frac{16}{3}\] and \[B=4\] |
| The formula of the compound \[={{A}_{4}}{{B}_{3}}.\] |
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