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QUESTION

# How to draw lewis structure F2?

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

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