Let's think about what might happen if we had a molecule of
butanoyl chloride.
So one, two, three, four carbons.
That's where the but- comes in, and then
it's a butanoyl chloride.
So it's an acyl halide or it's an acyl chloride.
Let me write this down just to give us some
practice with namings.
This is butanoyl chloride.
We saw a couple of videos ago that acyl halides, you just
count the main number of carbons.
One, two, three, four carbons.
That's where butan- comes from.
And then this is an acyl chloride, so the acyl chloride
part, this part, gives us the -oyl.
Or I guess you could look at even the carbonyl.
We could even say this whole part over here, we know it's a
carboxylic acid derivative.
It's in an acyl chloride.
So that's why we have the -oyl here and the chloride.
So let's think about what would happen if we have a
molecule of butanoyl chloride or if we had a solution, even
better, of butanoyl chloride, and for every molecule of
butanoyl chloride, we had two molecules of dimethylamide, or
sorry, dimethylamine.
Let me draw that.
So dimethyl, so two methyl groups.
One, two, and then we have one hydrogen, and then we're going
to have two molecules of this for every one molecule of our
butanoyl chloride.
So let me copy and paste this.
So edit, copy.
And edit, paste.
So let's think about what would happen in a solution
with these reactants in this ratio right here.
And just as a bit of review, this right here is dimethyl.
We kind of have a tie for our longest chain attached to the
nitrogen: dimethylamine.
You could pick one of these as the longest chain and then it
would actually be N-methylmethylamine.
Either one, this is the one that you're
more likely to see.
But this video isn't about naming, this video is to think
about what's likely to happen.
So what are we dealing with?
We have amine here and then we have an acyl chloride.
And if we look at our hierarchy of stability that we
looked at in the last video, we saw that when an amine
reacts or a carboxylic derivative from an amine,
which is an amide, is much more stable
than an acyl chloride.
This is the least stable.
So if we're starting with an acyl chloride and we have the
ingredients for an amide, this reaction will probably end up
with amide.
So let's see how we can get there.
What we know from previous videos when we studied amines,
that they are pretty good nucleophiles, so they could
have a nucleophile attack on this carbonyl
carbon right over here.
So you can imagine this amine right here, this nitrogen,
gives an electron to this carbonyl carbon.
This carbonyl carbon can then let go of this electron to
this top oxygen over here.
It was already hogging it to begin with.
And so the next step of our reaction would look like this.
What was the butanoyl chloride will now look like one, two,
three, four carbons.
Now you only have a single bond.
This oxygen up here now has a negative charge.
Since it took an electron from this central carbon right over
here, you are still bonded to this chlorine.
And actually let me do that in a different color so we can
keep track of it.
You are still bonded to this chlorine atom and then the
nitrogen has been bonded.
So this bond I'll drawn green because we're giving this
green electron to form the bond, and then the rest of the
dimethylamine is still over there.
Let me do it in that same color.
The rest of the dimethylamine, so you have CH3, CH3 and then
you just have your hydrogen.
And then this nitrogen gave away an electron, so it has a
positive charge.
Now, the next step, and this is chlorine, it's fairly
electronegative.
It's a not-so-bad leaving group.
It will want to hog this electron that is on the
central carbon.
So you can imagine in the next step that this oxygen gives
back an electron to reform the carbonyl group at the exact
same time that this chlorine takes an electron and forms a
chloride anion.
So the next step in this will look like-- so the molecules
will now look like-- you have there one,
two, three, four carbons.
That's one of the bonds to that oxygen, but now you've
now formed another bond.
That electron was given back to that central atom and now
you have the bond to the nitrogen, this bond right
here, and then the nitrogen is bound to one methyl group, two
methyl groups, and a hydrogen.
And it had given away an electron so it has a positive
charge, and the chloride anion has been bumped off.
The chloride anion, it took an electron from that central
carbon, so now it has a negative charge.
Now, we still have that other dimethylamine molecule, or for
every one of these, we should have two of these.
We've only use one of them, so let me bring the other one
into the mix, and this one could just be in the mix to
make this other molecule neutral now, and this could go
in either direction.
This part right here could go in either direction.
This guy's not so weak or it's not a bad base, so this guy
could give an electron to this hydrogen proton, and then the
hydrogen proton's electron, or that hydrogen atom's electron,
can be taken back by this nitrogen to make it neutral.
And I'll make this go in both directions.
So this could go in both directions.
So then this molecule over here will look like one, two,
three, four carbonyl group.
And let me color code it the same way just so we know what
parts are which parts.
We have this green bond to this nitrogen, which has now
lost a proton.
It was able to take back an electron,
so it is now neutral.
It is bonded to one, two methyl groups.
This dimethylamine took a hydrogen.
So let me draw it over here.
So it's nitrogen one, two, and then it already had one
hydrogen and now it's gaining another hydrogen.
It's gaining this hydrogen right over here.
So now it's bound to that hydrogen.
It gave an electron to get that hydrogen nucleus so it
now has a positive charge.
And, of course, we can't forget about that chloride
anion that's floating around.
And these might be attracted to each other.
One's positive, one's negative, form a salt.
So what are we left with?
And then once again, this is a little bit
of practice of naming.
We started with an acyl chloride and we ended with an
amide because we now have this nitrogen group attached.
So what is this?
This has one, two, three, four carbons so it's butan-, but
it's an amide.
So this part tells us that we're dealing with an amide.
It's butanamide, but to specify what type of amide, we
see that we have two methyl groups attached to the
nitrogen there, so we would call this-- let me put another
color here.
We have one, two methyl groups attached to the nitrogen, so
we would call this N comma N-dimethylbutanamide.
This N comma N let's us know that the methyl groups are
attached here as opposed to on the butyl group, I guess we
could view it this way.
So we end up with N,N-dimethylbutanamide, which
is an amide, one of the most stable carboxylic acid
derivatives.
And then this right here, this salt, what is this?
This right here is dimethyl, and this is now no longer
dimethylamine.
We now are a positively charged cation, so this is
dimethylammonium.
We get that from the fact that we have four bonds.
We have a positive charge.
This dimethylammonium, and then we have this negative
anion, dimethylammonium chloride.
I'll just go to the next line.
Dimethylammonium chloride.
But I really just wanted to show you a mechanism here of
how you could go from a less stable or one of the least
stable carboxylic acid derivatives to one of the most
stable, going from an acyl chloride, which butanoyl
chloride was, to an amide.