So basically we have three types of bonds.
You have single, double and triple.
And what we need to know is just a few facts about each.
The first thing is composition.
Composition deals with are they made out of sigma bonds, pi bonds, a combination.
We need to know this.
I already told you guys what single bonds were.
Do you guys remember?
It's just made out of one sigma.
So whenever I say sigma, it means single.
Single means sigma.
They're the same thing if it's just one sigma, that's a single.
Now, double and triple get a little bit more complicated because remember that I said that
it's actually more than one orbital combining.
So for a double bond, it's actually going to be one sigmas always because there's still
one region of overlap in the middle from the s orbitals.
But, there are also these p orbitals.
And the p orbitals have two regions of overlap, so that means that a double bond is made out
of a pi and a sigma or a sigma and a pi.
Overall that kind of makes sense because a double bond has two orbitals that are overlapping.
Then finally, a triple bond you could guess, now this one is going to have three orbitals
overlapping.
What's that going to be is still that one sigma from the s's, but for a triple bond
now you have two sets of p orbitals on both sides that are overlapping, one up and down
and one side to side.
What that means is that a triple bond is made out of one sigma and two pi.
Cool.
That's the first thing.
Now I want to talk about free rotation.
Why?
Because this has a lot to do with composition.
So remember that I said that a bond is just a region of shared space with electrons.
So if I just have one interaction in the middle, where they're overlapping, is it possible
to rotate one of the atoms like I'm doing right now and keep the bond intact?
The answer is yes.
If I rotate this atom, I can still keep this bond together.
It turns out that for a single bond, since they have one region of overlap, we're just
going to write a big yes right here.
Yes, I have free rotation there because I can rotate one of the atoms as much as I want.
It's always going to have that bond present.
Now let's look at double bonds.
Double bonds, they do have that region of overlap in the middle, that one area, but
they also have the region at the top and the region at the bottom from the pi bonds.
So it's going to look something like this, where you have basically electrons overlapping
at the top, electrons overlapping at the bottom.
If I try to rotate one of the atoms, is that going to break or change my bond at all?
Actually, yeah.
It will.
What's going to happen is this top orbital or this top region is going to break and this
bottom region is going to break.
That's really unfavorable and really unlikely to happen.
The reason is because remember that I said that when you form bonds, that saves a ton
of energy, so what that means is that I'm going to have to spend a lot of energy in
order to rotate and break this bond.
That's energy that these atoms don't have most of the time.
What that means is that these double bonds are not going to be able to break.
Actually, that's what I want you guys to write for double and triple.
They're both not going to be able to rotate because of the fact that if you rotate them,
you're going to have to break them and it's very difficult to break the bonds just to
rotate.
Good.
Now you guys understand the only ones that rotate are the single bonds.
Now let's talk about length.
Hopefully, you guys should remember what I talked about with sigma versus pi, which one
was the longer one?
Do you guys remember?
Sigma is the longest.
So single bond would be my longest.
It actually turns out that because the triple bond is made out of one sigma and two pi,
this one's going to be the shortest.
Then you could guess that the double bond is going to be like the middle child, so just
right in the middle.
Going to be in the middle, not quite as long, but not quite as short.
Now let's go onto strength.
So I already talked to you guys about this earlier, which of these is going to be the
weakest overall, in terms of single, double or triple?
The answer is that the single bond is the weakest.
The reason for that is that there's only one region of overlap that is saving energy.
Now the triple bond is actually going to be the strongest.
The reason for that is that it has three orbitals that are overlapping and each one is saving
a little bit more energy.
That means that once again, my double bond is going to be in the middle.
Now I want to ask you guys a question though, which of the orbitals is the strongest?
Is the sigma orbital the strongest or is the pi orbital the strongest?
The answer is that the sigma bond, not orbital, the sigma bond is the strongest because the
sigma bond saves the most energy of the three bonds for the triple.
Then the next pi bond would save a little bit less energy.
Then the last pi bond would not save that much energy at all, but it would still be
a little bit more.
You know what, I can tell that this is a little bit confusing, so I'm just going to give you
numbers like before.
Imagine that your single bond is saving 436 and then your double bond is saving 599 and
then imagine that your triple bond is saving like 650.
By the way, I'm just making that number up, but it's pretty accurate.
So what that means is that the single bond is saving a ton of energy, but as I go up
and make these bonds a little stronger, each pi bond is going to get weaker and weaker
and weaker.
So by the end, I'm only saving like 50 kJ per mole by adding another pi bond.
Does that make sense?
I hope that that distinction is clear to you guys.
Professors love to trick you on that.