Question

Consider the sulfur difluoridemolecule.What is the central atom? Enter its chemical symbol.How many lone pairs are around the central atom?What is the ideal angle between the sulfur-fluorine bonds?Compared to the ideal angle, you would expect the actual angle between the sulfur-fluorine bonds to be ...

Answer 1

Step-by-step explanation:

Question #1: What is the central atom?

The central atom of this molecule is Sulfur, S.

Question #2: Enter its chemical symbol.

The chemical symbol of the molecule is SF2 but the chemical symbol of the central atom is S.

Question #3: How many lone pairs are around the central atom?

There are two lone pairs around the central atom of Sulfur.

Question #4: What is the ideal angle between the sulfur-fluorine bonds?

The ideal angle between the Sulfur-Fluorine bonds is 109.5 degrees.

Question #5: Compared to the ideal angle, you would expect the actual angle between the sulfur-fluorine bonds to be.

I would expect the actual angle between the Sulfur-Fluorine bonds to be less than 109.5 degrees since the unbonded pairs have a greater repulsion with bonded pairs than the repulsion that happens between two bonded pairs. Therefore, the bonds would be closer to each other causing a smaller angle.

Answer 2

a. The central atom is sulfur

b. SF2

c. The central atom has two lone pairs

d. The ideal angle between the sulfur-fluorine bonds is 109.5°

e. I expect the actual angle between the sulfur-fluorine bonds to be less than 109.5° because unbonded pairs repel bonded pairs more than bonded pairs repel other bonded pairs. So the bonds here will be pushed closer than normal