- [Instructor] Let's talk a little bit about metallic solids. And here is an example of what a metallic solid might look like. They tend to be shiny like this. Some would say lustrous. Some of you might be guessing
maybe this is some type of aluminum or silver. It actually turns out that this is sodium. Our same friend sodium that
we saw bonding with chlorine to form sodium chloride
and form ionic solids, it can actually bond with
itself with metallic bonds. This right over here, you might guess is silver or something. It actually turns out this is calcium. And I know what you're thinking. Isn't calcium kind of
this chalky white powder? Well no, those are compounds
formed with calcium, things like calcium oxide. But this right over here is pure calcium. And the reason why it has
to be in this container, it is highly reactive with oxygen. So that's not oxygen that
is in this container. It's some form of inert gas. But calcium when it just bonds to itself with metallic bonds, which we'll
talk about in a little bit, it also looks kind of similar. It's this shiny, metallic,
or lustrous look to it. And what do you think this is? Well this is something
we're used to associating with metals, this is gold. But once again, you can see
it has this lustrous property. So what is it about
metals or metallic solids that allow them to be lustrous in this way and have other properties
that we're about to see? And to understand that,
we just have to look at the periodic table of elements. And that most of the
periodic table of elements is actually some form of metal. You have in red right over
here, this group one elements, not including hydrogen. Those are your alkali metals, and you have your alkaline earth metals, your transition metals, your post-transition
metals, your metalloids. It's really only what you
see in yellow and blue here that are not your metals. So how do metals form
solids when you just have a pure sample of them? Well the general idea, you can
look at your alkali metals, they all have that one valence electron. And to get to that stable outer shell, it's much easier for them to
give away a valence electron. And that's why we often see
these folks are dissipating in ionic bonds. They can be ionized quite easily. But if you have a pure sample of them, they can contribute electrons to a sea of electron, one each. These alkaline earth metals, they have two valence electrons. They too can be ionized or
if you have a pure sample like in a calcium, they can
contribute two valence electrons to a sea of electrons. And the transition metals
here have a similar ability to contribute valence electrons. And so in general, we
can view metallic solids as having cations, these
positively charged cations in a sea of electrons. So you have all these electrons here. I'll just draw all these
minus charges that they're in. Where do those electrons come from? Well if you're looking
at the alkali metals, each of those atoms could
give one electron to that sea because it doesn't really
want that valence electron. If you're talking about
alkaline earth metals, they could each donate
two electrons to that sea. Now given that you have
this positive charge in this sea of electrons, what are you think of the properties? How good do you think this will be at conducting electricity or heat? And many of you might guessed,
if you looked at a wire, wires are made out of metals,
because they are excellent at conducting electricity,
or they tend to be excellent at conducting electricity,
because you have all of these electrons
that can move around. And so if you apply a voltage,
they will start moving and conduct electricity. And those electrons can
also be good at conducting thermal energy or heat. Now what would be, we
already talked about them having the shiny, lustrous property, but how easy would it be to bend them? Ionic solids, we talked about they can be strong but brittle. As soon as you try to shift
them around a little bit, they can break. But what do you think
is going to happen here? If let's say right over here,
I were to push really hard and on the top I would have
pushed really hard to the left. Do you think this will be brittle? Or do you think it will be malleable? It's easy to bend. Well if you have a pure metallic solid, it's actually quite malleable. If you just took this
top part and pushed it to the left like this, no big deal. You have those cations
that are still in those that sea of electrons. And that's generally
true of metallic solids. They're very malleable. They are not brittle. In fact, so much so that
often times we want them to be a little bit more rigid. We want them to be a little bit harder. And that's why we might do
things like add other elements into the metallic solid. For example, pure iron
is reasonably malleable. But if you wanna make it stronger, you could stick carbon atoms in between. For example, you could
put a carbon atom there, or carbon atom over there. And that way, it kind of disrupts this electron sea a little bit. So it's not quite as malleable. It'll be stronger and more rigid. So I'll leave you here. This is just an extension of
what we've already learned about metals and metallic bonds. To just realize why most of
the periodic table of elements that we're familiar with
has some of these properties when they are, when you
have pure solids of them.