Question

HELP: MODELING MOLECULES!!!!!!!!!!!!!!!!

Answer 1

How do I solve the electron dot structure, structure formula, and drawing for the following molecules:

Sulfur Hexachloride
Carbon Dioxide
Methyl Cyclohexane
Propane
Ethene
Phenol

(I have the chemical formulas for all)

Answer 2

I believe the chemical formulas are:
(in order as the molecules from above)
SCl6
CO2
C7H14
C3H8
C2H4
C6H6O

Answer 3

I know how to do a few. I had to do a lab on this the other day.

Answer 4

I only have Carbon dioxide and Ethane

Answer 5

Oh you said Ethene. Sorry. The second one on the picture now does not apply to you.

Answer 6

Sulfur Hexachloride
SCl6 So now we count the number of valence electrons each has by seeing what column it's in, (1-8) not counting the columns of the transition metals.

Since Sulfur is in the 6th and Chlorine is in the 7th, and there are 6 chlorines, we can add up all their valence electrons:

6*1+7*6=48 valence electrons.

But remember that electrons come in pairs, either in bonds or as lone pairs. So I usually divide the valence electron number by 2 and just think about placing pairs. It's up to you, but I think it's convenient since we can count "1" in our mind each time we place a bond or a electron pair. So we need to place 24 pairs/bonds.

So we can guess that sulfur is a central atom and draw out a bond from sulfur to each chlorine. Since Sulfur is in the 3rd row it can use d-orbitals to break the octet rule. So when we bond all the chlorines onto sulfur we get:



So we made 6 bonds, that means we used up 12 electrons, so if you're counting (AND YOU SHOULD BE!) you have 36 electrons or simply 18 electron pairs left to place. Now let's give chlorine a neutral charge.

Answer 7

So now if you count up all the pairs we used up 6 each, or 3 pairs each, we can multiply it by 6 to find that we have used up the remaining 36 (18 pairs) of electrons with none leftover! Problem pretty much solved. Keep in mind that all of the atoms need to have a complete octet, no more and no less (Except for some exceptions, like sulfur). If you count them up you'll see chlorine has 8, 6 in lone pairs, 2 in the bond. Sulfur as 12, which is allowed since it's an exception.

Now if your professor cares about the structure you can say that it's octahedral with this sort of shape:

Try the same sort of method.

Count all the valence electrons. Make sure there's at least one bond between everything. Attempt to make all the atoms in the molecule neutral and have a complete octet.

Methyl Cyclohexane
Propane
Ethene
Phenol

None of those have exceptions to the octet rule, so don't worry about that so much. Determining the structures is kind of hard, but you can just look them up and after you see them a couple times, you should have no problem with structures like Phenol, which is the simplest of the benzene alcohol derivatives.

Answer 8

Thanks so much....I finally understand it now lol!!!!