Here’s how you can do that.

The first thing to do here is determine the total number of you have in a fluorine molecule, ##”F”_2##.

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

##”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 .

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## 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 of the ##”F”_2## molecule will thus be