Question

What is the molecular geometry (shape) for F2?

Answer 1

Linear.

This is because Fluorine has seven valence electrons, pairing the odd one out in the middle will solve this problem.

It can't be pyrimidal or bent as it doesn't have any lone (unpaired) valence electrons. It can't be a tettrahedral as there aren't four other elements. It couldn't be a planar as there isn't a total of four elements to pair with a central atom.

Hope this helps!

Answer 2

Answer : The molecular geometry for $F_2$ is linear.

Explanation :

Formula used  :

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

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

Now we have to determine the hybridization of the $F_2$  molecules.

The given molecule is, $F_2$

$\text{Number of electrons}=\frac{1}{2}\times [7+1]=4$

The number of electron pair are 4 that means the hybridization will be $sp^3$ and the electronic geometry of the molecule will be tetrahedral.

But as there are 1 atom around the central fluorine atom, the second, third and fourth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be linear.

Hence, the molecular geometry for $F_2$ is linear.