Problem: Although I3- is known, F3- is not.Another classmate says F3-– does not exist because F is too small to make bonds to more than one atom. Is this classmate possibly correct?

FREE Expert Solution

Let us start this problem by drawing the Lewis structure of F3-.

Step 1: The steps that are required to be taken:

  1. Firstly, we need to calculate the total number of valence electrons that would be present in the structure. The number of valence electrons per atom of each element will be based on its group number. F is in group 7A so it has 7 valence electrons.
  2. One extra electron should be added for the negative charge present.


Atom               Valence Electrons

           Fluorine       7 e- x 3 = (21 e) + 1 

                                                = 22 valence e- 

   A total of 22 valence electrons are present.  

Step 2 : The Lewis structures have to be drawn.

  • All the atoms in F3are equivalent; therefore, they can be drawn next to each other. 
  • You will then need to subtract two electrons for each bond. 
  • Then place the rest of the electrons in each fluorine atom to make sure the atom fulfills the octet
  • Finally, the two remaining electrons are placed in the central atom.
  • The formal charge for each atom is then calculated using the equation 

Formal Charge = group number – (bonds the element is making + non-bonding electrons)

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Problem Details

Although I3- is known, F3- is not.

Another classmate says F3-– does not exist because F is too small to make bonds to more than one atom. Is this classmate possibly correct?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Hybridization concept. You can view video lessons to learn Hybridization. Or if you need more Hybridization practice, you can also practice Hybridization practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hampton's class at UCF.