00:01
So I talked earlier on
about the importance
of having a full outer shell in order to achieve
stability. And this applies to all elements:
not just those in the first three groups and
the last two groups, but also those within
the middle. And whereas I talked before about
the formal transfer of electrons from one
atom to another, now I'd just like to briefly
introduce you to the idea of covalent bonds—that
is, where you have electrons which are shared.
So rather than formally transferred, they're
shared in order for both species to obtain
a full outer shell and the stability that
comes with that. Let's take, for example,
methane. This consists of two elements: one
carbon and four hydrogen atoms. Let's consider
those individual atoms in isolation. If we
look at carbon (again, we're using the abbreviated
form, so the helium nucleus followed by 2s2,
2p2) we can see that it needs, or requires,
four additional electrons to complete its
valence shell. If, on the other hand, we look
at hydrogen (which, as you should recall,
has the electron configuration 1s1), it needs
to gain one additional valence electron in
order to complete its outer shell.
So if carbon shares all four of its valence
electrons with four hydrogen atoms, such as
this shown, this enables the completion of
the outer shell for both atoms, or both sets
of atoms. The hydrogen gains the electron
it requires to create 1s2, and the carbon
can share the four electrons from the hydrogen
to create the 2s2, 2p6 outer shell. So hopefully,
you can appreciate in this scenario, where
the actual loss of individual electrons is
not energetically preferable, sharing, or
covalent bond formation (which is what I'm
showing you here), is the preferred way in
which atoms can achieve the energetic stability
associated with a full outer shell. The bonds
between the carbon and the hydrogen are covalent
bonds. And I'll just want to briefly draw
your attention to the shape of the molecule,
as I've shown here. If you recall, if we look
back at the anionic and ionic systems, I talked
about the idea that they form these crystal
lattices, or structures, where you have multiple
ions all able to interact with each other
electrostatically. However, in the case of
covalent bonds—and this is very important
for macroscopic properties—the bonds are
directional. The carbon is bound to the hydrogen
and nothing else. And so therefore, you don't
have the same macroscopic interactions, which
means that the methane exists as a gas rather
than as a crystal structure.
03:22
So due to their electron requirements, hydrogen
will always form one covalent bond and is
said, formally, to have a valency of 1. Carbon
will always form four covalent bonds and therefore
has a valency of 4. And as we will see when
we actually start looking at things like hybridization,
it'll make you realize the importance of the
carbon in organic chemistry. Because whilst
it's possible to form many thousand formula
units, compounds, and molecules and so forth
from other parts of the periodic table from
different elements, carbon in itself is directly
related to the millions and millions of different
compounds which exist on this planet and is
therefore one of the most—or the most—important
compound because of its diversity.
04:22
So, question for you now:
• Ammonia is a molecule that contains a
single nitrogen covalently bound to hydrogen
atoms. So what will the molecular formula
for ammonia be?
• What, therefore, is the valency of nitrogen?
• And a follow-up: Hydrazine, which is a
related molecule, contains two nitrogen atoms
and hydrogen atoms. The nitrogen atoms are
joined by a covalent bond. What you should
do as an exercise is draw the bonding and
give the molecular formula for hydrazine.