If your're ANY good in CHemistry, PLEASE look at this....?

Question

For sulfur dioxide, Use VSPER to predict the underlying gemotery for the valence electrom domains and the molecular geometry. Give approximate bond angles

I know the angle is 120 degrees. and thats about it...can u help me?

Answer 1

Sulfur dioxide is SO2, so total valence electrons is 18.

Trigonal planar parent shape (electron group geometry of 3)
VESPR predicts a bent shape, which agrees with your prediction of a 120 degree angle (more accurately, 119 degrees).

:O:
//
S: (SO2-VESPR model)
\\
:O:

Answer 2

Righto... step by step

(a) Sulfur and oxygen both have six electrons in the valence shell. That means there's a total of 18 electrons to distribute (6 from sulfur, 6 from each of the oxygens) or 9 pairs.

(b) Each of the three atoms tries to capture four electron pairs to make up the eight electrons in its valence shell. That means that the atoms "want" 3 * 4 = 12 electron pairs. There are only nine available pairs available, meaning that three are shared. Six electron pairs are unshared.

(c) We know from (b) that the sulfur is sharing three electron pairs with the oxygen. That means that it only has one pair all to itself to make up the total of four pairs.

(d) The structure of the molecule (as far as sulfur is concerned) therefore involves two clouds of electrons bonding with the two oxygen atoms, and one unshared electron pair.

(e) The three clusters of electrons are the farthest apart if they organize themselves as a planar structure with 120 degree bond angles. This is the structure for SO2

The link below describes the structure with some diagrams. Hard to visualize in text-only format

Answer 3

The sulfur atom is sp2 hybridized: an unshared pair, a double bond to one oxygen atom and a single bond to the other: a resonance structure --
.. .. ..
:O::S:O:
" (quote marks = electron pair under O on the right)

bond angle is 120°. Electrons has trigonal pyramidal geometry; the molecule is angular. Bond order is one and a half -- two sigma bonds and one pi. All bonds actually identical -- in between double and single in length and strength.

Answer 4

Oh jeez..That equation makes me nervous just reading it..
I'm taking college chemistry in a week and I'm just sweating already

Answer 5

I thought I was good in chemistry until I looked at your question. lol