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

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.

the answer is 75.0%.