The electronic configuration of two neutral elements A and B are
`A= 1s^(2) 2s^(2) 2p^(6) 3s^(2)`
`B=1s^(2) 2s^(2) 2p^(5)`
Which of the following represents the structure of the compound formed by them ?

Options

A. `A ^(2+) B ^(2-)`
B. `B^(2-) (A ^(-))_(2)`
C. `A^(2+) (B^(-))_(2)`
D. `A^(+)B^(-)`

Answer

C

Explanation

A loses two electrons to form `A^(2+)` while two atoms of B lose one electron each to from `2B^(-).` Therefore, the formula of the compound is `A^(2+)(B^(-))_(2).`