# Question #d2d69

Oct 27, 2015

Here's how you can do that.

#### Explanation:

The first thing to do here is determine the total number of valence electrons you have in a fluorine molecule, ${\text{F}}_{2}$.

The fluorine molecule is composed of two fluorine atoms. Each fluorine atom has $7$ valence electrons, which means that the molecule will have a total of

${\text{valence e}}^{-} = 7 + 7 = 14$

Now, these two fluorine atoms have seven electrons in their outermost shells, which means that they only need one more to complete their octet.

They will thus form one single bond to which each of the two atoms contributes one electron.

This bond will take up $2$ of the $14$ valence electrons of the molecule. The remaining $12$ valence electrons will be placed as lone pairs on the fluorine atoms, three lone pairs of electrons on each, to be precise.

SIngle bonds are drawn using a single horizontal dash between the two atoms. Lone pairs are represented using dots, each dot being equivalent to one electron.

The Lewis structure of the ${\text{F}}_{2}$ molecule will thus be