The one thing that probably causes some of the most pain
in chemistry, and in organic chemistry, in particular, is
just the notation and the nomenclature or the naming
that we use.
And what I want to do here in this video and really the next
few videos is to just make sure we have a firm grounding
in the notation and in the nomenclature or how we name
things, and then everything else will
hopefully not be too difficult.
So just to start off, and this is really a little bit of
review of regular chemistry, if I just have a chain of
carbons, and organic chemistry is dealing
with chains of carbons.
Let me just draw a one-carbon chain, so it's really kind of
ridiculous to call it a chain, but if we have one carbon over
here and it has four valence electrons, it
wants to get to eight.
That's the magic number we learned in
just regular chemistry.
For all molecules, that's the stable valence structure, I
guess you could say it.
A good partner to bond with is hydrogen.
So it has four valence electrons and then hydrogen
has one valence electron, so they can each share an
electron with each other and then they
both look pretty happy.
I said eight's the magic number for everybody except
for hydrogen and helium.
Both of them are happy because they're only trying to fill
their 1s orbital, so the magic number for
those two guys is two.
So all of the hydrogens now feel like
they have two electrons.
The carbon feels like it has eight.
Now, there's several ways to write this.
You could write it just like this and you can see the
electrons explicitly, or you can draw little lines here.
So I could also write this exact molecule, which is
methane, and we'll talk a little bit more about why it's
called methane later in this video.
I can write this exact structure like this: a carbon
bonded to four hydrogens.
And the way that I've written these bonds right here you
could imagine that each of these bonds consists of two
electrons, one from the carbon and one from the hydrogen.
Now let's explore slightly larger chains.
So let's say I have a two-carbon chain.
Well, let me do a three-carbon chain so it really
looks like a chain.
So if I were to draw everything explicitly it might
look like this.
So I have a carbon.
It has one, two, three, four electrons.
Maybe I have another carbon here that has-- let me do the
carbons in slightly different shades of yellow.
I have another carbon here that has one,
two, three, four electrons.
And then let me do the other carbon in that first yellow.
And then I have another carbon so we're going to have a
three-carbon chain.
It has one, two, three, four valence electrons.
Now, these other guys are unpaired, and if you don't
specify it, it's normally going to be hydrogen, so let
me draw some hydrogens over here.
So you're going to have a hydrogen there, a hydrogen
over there, a hydrogen over here, a hydrogen over here, a
hydrogen over there, a hydrogen over here, almost
done, a hydrogen there, and then a hydrogen there.
Now notice, in this molecular structure that I've drawn, I
have three carbons.
They were each able to form four bonds.
This guy has bonds with three hydrogens and another carbon.
This guy has a bond with two hydrogens and two carbons.
This guy has a bond with three hydrogens and then this carbon
right here.
And so this is a completely valid molecular structure, but
it was kind of a pain to draw all of these
valence electrons here.
So what we typically would want to do is, at least in
this structure, and we're going to see later in this
video there's even simpler ways to write it, so if we
want at least do it with these lines, we can
draw it like this.
So you have a carbon, carbon, carbon, and then they are
bonded to the hydrogens.
So you'll almost never see it written like this because this
is just kind of crazy.
Hyrdrogen, hydrogen-- at least crazy to write.
It takes forever.
And it might be messy, like it might not be clear where these
electrons belong.
I didn't write it as clearly as I could.
So they have two electrons there.
They share with these two guys.
Hopefully, that was reasonably clear.
But if we were to draw it with the lines, it
looks just like that.
So it's a little bit neater, faster to draw, same exact
idea here and here.
And in general, and we'll go in more detail on it, this
three-carbon chain, where everything is a single bond,
is propane.
Let me write these words down because it's helpful to get.
This is methane.
And you're going to see the rhyme-- you're going to see
the reason to this naming soon enough.
This is methane; this is propane.
And there's an even simpler way to write propane.
You could write it like this.
Instead of explicitly drawing these bonds, you could say
that this part right here, you could write that that part
right there, that is CH3, so you have a CH3, connected to
a-- this is a CH2, that is CH2 which is then connected to
another CH3.
And the important thing is, no matter what the notation, as
long as you can figure out the exact molecular structure, as
long as you can-- so there's this last CH3.
Whether you have this, this, or this, you know what the
molecular structure is.
You could draw any one of these given any of the others.
Now, there's an even simpler way to write this.
You could write it just like this.
Let me do it in a different color.
You literally could write it so we have three carbons.
So one, two, three.
Now, this seems ridiculously simple and you're like, how
can this thing right here give you the same information as
all of these more complicated ways to draw it?
Well, in chemistry, and in organic chemistry in
particular, any of these-- let me call it a line diagram or a
line angle diagram.
It's the simplest way and it's actually probably the most
useful way to show chains of carbons or to
show organic molecules.
Once they start to get really, really complicated, because
then it's a pain to draw all of the H's, but when you see
something like this, you assume that the end points of
any lines have a carbon on it.
So if you see something like that, you assume that there's
a carbon at that end point, a carbon at that end point, and
a carbon at that end point.
And then you know that carbon makes four bonds.
There are no charges here.
All the carbons are going to make four bonds, and each of
the carbons here, this carbon has two bonds, so the other
two bonds are implicitly going to be with hydrogens.
If they don't draw them, you assume that they're going to
be with hydrogens.
This guy has one bond, so the other three
must be with hydrogen.
This guy has one bond, so the other three must be hydrogens.
So just drawing that little line angle thing right there,
I actually did convey the exact same information as this
depiction, this depiction, or this depiction.
So you're going to see a lot of this.
This really simplifies things.
And sometimes you see things that are in between.
You might see someone draw it like this, where they'll write
CH3, and then they'll draw it like that.
So that's kind of combining this way of writing the
molecule where you write the CH3's for the end points, but
then you implicitly have the CH2 on the inside.
You assume that this end point right here is a C and it's
bonded to two hydrogens.
So these are all completely valid ways of drawing the
molecular structures of these carbon chains or of these
organic compounds.