while aluminium can form the ion (AlF6)3-, boron is unable to form (BF6)3- ion

Open in App

Solution

The electronic config. of B is 1s² 2s² 2p¹ whereas Al has electronic config. 1s² 2s² 2p⁶ 3s² 3p¹
As the valence shell in B is L shell it can accommodate a maximum of 8 (2x2²) electrons, whereas in case of (BF₆)^3- the no. of electrons around central atom is 12 which is not possible.

In case of Al the valence electron is in the M shell and can accommodate a maximum of 18 electrons (2x3²) hence (AlF₆)^3- can exist.

Suggest Corrections

Similar questions

{B F}_{6}^{3 -}

{[S i F_{6}]}^{2 -}

{[S i {C l}_{6}]}^{2 -}

{[{B F}_{6}]}^{3 -}

H {N O}_{3}

B^{3 +}

M F_{6}^{3 -}

Join BYJU'S Learning Program