The shapes of BF3 and [BH4^(-)] are resp...

The shapes of `BF_3` and `[BH_4^(-)]` are respectively

planar, tetrahedral

tetrahedral, planar

planar, planar

tetrahedral, tetrahedral

Text Solution

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The correct Answer is:

In `BF_3`, boron is `sp^2`-hybridised as it contains three bond pairs and therefore, `BF_3` molecule is trigonal planar in shape. On the other hand, in `[BH_4]^(-)` boron is `sp^3`-hybridised because of the presence of four bond pairs and hence, `[BH_4]^(-)` species is tetrahedral in shape.

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The hybridisation of boron in 'B F_3' and 'BF_4' respectively is sp^2, sp^3' sp^3, sp^3' s p^3, s p^3 d'. sp^2, sp^2'

sp^2, sp^3'

sp^3, sp^3'

s p^3, s p^3 d'.

sp^2, sp^2'

Hybridization, shape and number of t bonds in XeOF_2 molecule are respectively,

`sp^3` , pyramidal,1

`sp^3d`, trigonäl bipyramidal, 2

`sp^3d` , T-shaped, 1

`sp^3,d` , square pyramidal, 1

The geometries of the molecules BF_3 and NF_3 are riigonal planarand trigonal pyramidal, respectively. Which statement best accounts for the difference?

N is more electronegative than B

`BF_3` is ionic, `NF_3` is covalent

B utilise `sp^2` hybridization, while N does not

N is `sp^3` hybridised and has non-bonding pair of valence electrons, while B does not