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And we have this general notion, and I think water is the example that always comes to at least my mind. Is that solid happens when things are colder, relatively colder. And then as you warm up, you go into a liquid state.
And as your warm up even more you go into a gaseous state. So you go from colder to hotter. And in the case of water, when you're a solid, you're ice. When you're a liquid, some people would call ice water, but let's call it liquid water. I think we know what that is. And then when it's in the gas state, you're essentially vapor or steam. So let's think a little bit about what, at least in the case of water, and the analogy will extend to other types of molecules.
But what is it about water that makes it solid, and when it's colder, what allows it to be liquid. And I'll be frank, liquids are kind of fascinating because you can never nail them down, I guess is the best way to view them. Or a gas. So let's just draw a water molecule. So you have oxygen there. You have some bonds to hydrogen. And then you have two extra pairs of valence electrons in the oxygen. And a couple of videos ago, we said oxygen is a lot more electronegative than the hydrogen.
It likes to hog the electrons. So even though this shows that they're sharing electrons here and here. At both sides of those lines, you can kind of view that hydrogen is contributing an electron and oxygen is contributing an electron on both sides of that line.
But we know because of the electronegativity, or the relative electronegativity of oxygen, that it's hogging these electrons. And so the electrons spend a lot more time around the oxygen than they do around the hydrogen. And what that results is that on the oxygen side of the molecule, you end up with a partial negative charge.
And we talked about that a little bit. And on the hydrogen side of the molecules, you end up with a slightly positive charge.
Now, if these molecules have very little kinetic energy, they're not moving around a whole lot, then the positive sides of the hydrogens are very attracted to the negative sides of oxygen in other molecules. Let me draw some more molecules. When we talk about the whole state of the whole matter, we actually think about how the molecules are interacting with each other. Not just how the atoms are interacting with each other within a molecule.
I just drew one oxygen, let me copy and paste that. But I could do multiple oxygens. And let's say that that hydrogen is going to want to be near this oxygen. Because this has partial negative charge, this has a partial positive charge. And then I could do another one right there.
And then maybe we'll have, and just to make the point clear, you have two hydrogens here, maybe an oxygen wants to hang out there. So maybe you have an oxygen that wants to be here because it's got its partial negative here. And it's connected to two hydrogens right there that have their partial positives.
But you can kind of see a lattice structure. Let me draw these bonds, these polar bonds that start forming between the particles. These bonds, they're called polar bonds because the molecules themselves are polar. And you can see it forms this lattice structure. And if each of these molecules don't have a lot of kinetic energy. Or we could say the average kinetic energy of this matter is fairly low.
And what do we know is average kinetic energy? Well, that's temperature. Then this lattice structure will be solid. These molecules will not move relative to each other. I could draw a gazillion more, but I think you get the point that we're forming this kind of fixed structure.
And while we're in the solid state, as we add kinetic energy, as we add heat, what it does to molecules is, it just makes them vibrate around a little bit. If I was a cartoonist, they way you'd draw a vibration is to put quotation marks there. That's not very scientific.
But they would vibrate around, they would buzz around a little bit. I'm drawing arrows to show that they are vibrating. It doesn't have to be just left-right it could be up-down. But as you add more and more heat in a solid, these molecules are going to keep their structure.
So they're not going to move around relative to each other. But they will convert that heat, and heat is just a form of energy, into kinetic energy which is expressed as the vibration of these molecules. Now, if you make these molecules start to vibrate enough, and if you put enough kinetic energy into these molecules, what do you think is going to happen? Well this guy is vibrating pretty hard, and he's vibrating harder and harder as you add more and more heat. This guy is doing the same thing.
At some point, these polar bonds that they have to each other are going to start not being strong enough to contain the vibrations. And once that happens, the molecules-- let me draw a couple more. Once that happens, the molecules are going to start moving past each other. So now all of a sudden, the molecule will start shifting. But they're still attracted.
Maybe this side is moving here, that's moving there. You have other molecules moving around that way. But they're still attracted to each other. Even though we've gotten the kinetic energy to the point that the vibrations can kind of break the bonds between the polar sides of the molecules.
Our vibration, or our kinetic energy for each molecule, still isn't strong enough to completely separate them.
They're starting to slide past each other. And this is essentially what happens when you're in a liquid state. You have a lot of atoms that want be touching each other but they're sliding.
They have enough kinetic energy to slide past each other and break that solid lattice structure here. And then if you add even more kinetic energy, even more heat, at this point it's a solution now. They're not even going to be able to stay together.
They're not going to be able to stay near each other. If you add enough kinetic energy they're going to start looking like this. They're going to completely separate and then kind of bounce around independently.
Especially independently if they're an ideal gas. But in general, in gases, they're no longer touching each other. They might bump into each other. But they have so much kinetic energy on their own that they're all doing their own thing and they're not touching. I think that makes intuitive sense if you just think about what a gas is. For example, it's hard to see a gas. Why is it hard to see a gas? Because the molecules are much further apart.
So they're not acting on the light in the way that a liquid or a solid would. And if we keep making that extended further, a solid-- well, I probably shouldn't use the example with ice. Because ice or water is one of the few situations where the solid is less dense than the liquid. That's why ice floats. And that's why icebergs don't just all fall to the bottom of the ocean. And ponds don't completely freeze solid. But you can imagine that, because a liquid is in most cases other than water, less dense.
That's another reason why you can see through it a little bit better.
Or it's not diffracting-- well I won't go into that too much, than maybe even a solid. But the gas is the most obvious. And it is true with water. The liquid form is definitely more dense than the gas form. In the gas form, the molecules are going to jump around, not touch each other.
And because of that, more light can get through the substance. Now the question is, how do we measure the amount of heat that it takes to do this to water? And to explain that, I'll actually draw a phase change diagram. Which is a fancy way of describing something fairly straightforward.
Let me say that this is the amount of heat I'm adding. And this is the temperature. We'll talk about the states of matter in a second. So heat is often denoted by q. Sometimes people will talk about change in heat. They'll use H, lowercase and uppercase H. They'll put a delta in front of the H.
Delta just means change in. And sometimes you'll hear the word enthalpy. Let me write that. Because I used to say what is enthalpy? It sounds like empathy, but it's quite a different concept. At least, as far as my neural connections could make it. But enthalpy is closely related to heat. It's heat content. For our purposes, when you hear someone say change in enthalpy, you should really just be thinking of change in heat.
I think this word was really just introduced to confuse chemistry students and introduce a non-intuitive word into their vocabulary.
The best way to think about it is heat content. Change in enthalpy is really just change in heat. And just remember, all of these things, whether we're talking about heat, kinetic energy, potential energy, enthalpy.
You'll hear them in different contexts, and you're like, I thought I should be using heat and they're talking about enthalpy. These are all forms of energy.
And these are all measured in joules. And they might be measured in other ways, but the traditional way is in joules.
And energy is the ability to do work. And what's the unit for work? Well, it's joules. Force times distance. But anyway, that's a side-note. But it's good to know this word enthalpy. Especially in a chemistry context, because it's used all the time and it can be very confusing and non-intuitive. Because you're like, I don't know what enthalpy is in my everyday life. It's easier to figure out tough problems faster using Chegg Study. Unlike static PDF Chemistry In Context 7th Edition solution manuals or printed answer keys, our experts show you how to solve each problem step-by-step.
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