Question

show BF4 Bond formation.​

Answer 1

Answer:

Use VSEPR theory (valence shell electron pair repulsion)

Boron has 3 valence electrons, and each of the four fluorides contributes one electron to each covalent bond. The overall negative charge of the molecule contributes another electron, so overall we have 3 + 4 + 1 = 8 valence electrons which form 4 electron pairs.

The pairs arrange themselves in space to maximise the distance between them, thereby reducing the electronic repulsion between them to a minimum. The shapes for various numbers of electron pairs are:

2 - linear

3 - trigonal planar

4 - tetrahedral

5 - trigonal bipyramidal

6 - octahedral

7 and above - Google!

And hence BF4- would be tetrahedral.

Explanation:

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