Question

sulfur has several different alloys. draw the lewis structure for each. using a thermochemical cycle, determine which compound in the pair is more stable. Show youre work

a) S2 vs S3

b) S2 vs S8

Answer 1

Now, the thermochemical cycle, I don't know much about that, but here's your lewis structures:

  

Now according to these structures:

S2 vs S3:

S2 is more stable, cause it has more electrons available thant S3. S2 is a linear molecuel while S3 it's not, so the stability is better if it's linear.

S2 vs S8

In this case, a single bond gives more stability than a double bond. So S8 is more stable, and has more available electrons than S2. In general terms S8 is the most stable alloys from sukphur.

EDIT:

For S2, it has one pi bonds and one sigma bonds.

For S3 it has two pi bonds and two sigma bonds.

For S8, all of it's bond are sigma.

Hope this helps