Question

Why NF3 is pyramidal but BF3 is triangular planar?​

Answer 1

Explanation:

In BF3 there are three bond pairs which are shared in between two atoms resulting in the triangular planar structure while in case of NF3 there is sharing of three bond pairs plus one lone pair. Because of the lone pair sharing the structure get distorted and resulting structure is pyramidal.....

Answer 2

$NF_3$ has one lone pair of electrons whereas $BF_3$ does not have any lone pair of electrons

Explanation:

According to VSEPR theory:

Number of electron pairs =$\frac{1}{2}[V+N-C+A]$

For $NF_3$

where,

V = number of valence electrons present in central nitrogen atom = 5

N = number of monovalent atoms = 3

C = charge of cation = 0

A = charge of anion = 0

Number of electron pairs =$\frac{1}{2}[5+3-0+0]=4$

The number of electron pairs is 4 that means the hybridization will be $sp^3$  but as only 3 atoms are present , one position will be occupied by a lone pair thus electronic geometry is tetrahedral and the molecular geometry will be trigonal pyramidal.

For $BF_3$

where,

V = number of valence electrons present in central boron atom = 3

N = number of monovalent atoms = 3

C = charge of cation = 0

A = charge of anion = 0

Number of electron pairs =$\frac{1}{2}[3+3-0+0]=3$

The number of electron pairs is 3 that means the hybridization will be $sp^2$ thus electronic geometry and the molecular geometry will be trigonal planar.

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