- States of matter
- States of matter follow-up
- Specific heat and latent heat of fusion and vaporization
- Specific heat, heat of fusion and vaporization example
- Chilling water problem
- Change of state example
- Vapor pressure
- Phase diagrams
- Representing solids, liquids, and gases using particulate models
- Crystalline and amorphous polymers
- Representing alloys using particulate models
- Structure of metals and alloys
- Solids, liquids, and gases
Introduction to the states or phases of matter. Created by Sal Khan.
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Why doesn't it change temperature? I mean where/what does the energy go/do?(57 votes)
- think of it like this........the energy is being used to break the bonds...since it is all being used to break the bonds their is No more extra energy to RAISE the TEMPERATURE. Remember raising the temperature takes energy. The temperature will only start to rise when the state of matter has changed completely and no more energy has to be diverted to breaking bonds.(34 votes)
- Where can you find the fifth form of matter which is Bose-Einstein Condensate?(23 votes)
- The first "pure" Bose–Einstein condensate was created by Eric Cornell, Carl Wieman, and co-workers at JILA on 5 June 1995. They cooled a dilute vapor of approximately two thousand rubidium-87 atoms to below 170 nK using a combination of laser cooling (a technique that won its inventors Steven Chu, Claude Cohen-Tannoudji, and William D. Phillips the 1997 Nobel Prize in Physics) and magnetic evaporative cooling. About four months later, an independent effort led by Wolfgang Ketterle at MIT condensed sodium-23. Ketterle's condensate had a hundred times more atoms, allowing important results such as the observation of quantum mechanical interference between two different condensates. Cornell, Wieman and Ketterle won the 2001 Nobel Prize in Physics for their achievements.
A group led by Randall Hulet at Rice University announced a condensate of lithium atoms only one month following the JILA work. Lithium has attractive interactions, causing the condensate to be unstable and collapse for all but a few atoms. Hulet's team subsequently showed the condensate could be stabilized by confinement quantum pressure for up to about 1000 atoms. Various isotopes have since been condensed.(8 votes)
- Could you explain me why the oxygen atoms in the molecular formula of water have 4 extra electrons on their outermost shell? I thought that oxygen had 6 electrons on its outermost shell, so bonding with 2 hydrogen atoms it becomes "happy" because it has an electronic configuration like neon with 8 electrons. Why it has 4 more atoms that can be used for other bonds??(13 votes)
- The oxygen does have 8 valence electrons in the water molecule. Let us break down where they come from and what they are doing:
Oxygen started out with 6 valence electrons. By combining with two atoms of hydrogen it shares with each hydrogen one electron of its own and one electron from the hydrogen, so it shares a total of two of its electron with a total of two electrons from the hydrogen. This is a total of 4 electrons being shared.
But, it still has the other 4 valence electrons that it kept for itself which did not react with anything. Instead, they paired up within the oxygen atom into what are called "lone pairs". It has two lone pairs, for a total of 4 valence electron in lone pairs.
So, the extra 4 valence electrons are in lone pairs. But the total of all valence electrons is 8. There are 4 electrons involved in bonds and 4 valence electron in two lone pairs.(24 votes)
- Why are there two hydrogen atoms, but only one oxygen atom? Don't you have to have the same amount of different atoms?(8 votes)
- A noble gas (the most stable state of an atom/compound) has an electron configuration ending with a p orbital completely filled, p^6.
Neutral Oxygen has an electron configuration ending with 2p^4
Neutral Hydrogen has an electron configuration of 1s^1; it has one valence electron.
It wouldn't make sense to have Oxygen only take one Hydrogen, as that would only fill its valence orbital to 2p^5, and its most stable state is at 2p^6.
An easier way to think of it would be: Oxygen wants two electrons; Hydrogen has only one electron to give, ergo Oxygen takes two Hydrogens.
Compounds are *not* limited to have the same amount of each element.(20 votes)
- what makes liquid water have more density than ice?(13 votes)
- The way the ice crystals are connected to each other packs the molecules a little less densely than they are when they are not connected in a crystal structure(6 votes)
- Fire is a chemical reaction produced by rapid oxidation of some fuel in gaseous or plasma form.(11 votes)
- When at the beginning of the video he states the three states of matter. is there any other types of states?(5 votes)
- Most definitely, yes. The three that most people know about are solid, liquid, and gaseous states. We probably interact with these every single day. If you don't, there's something wrong with you. There is another state of matter that most people probably know, and that is plasma. Plasma is present in things such as neon lighting and stars, such as the one we call the Sun. Plasma can be created by exposing a gas to an electromagnetic field and creating ions. Physical properties of plasma include the fact that plasma has no shape unless enclosed in a container, similar to a gas. However, in the presence of an electromagnetic field, plasma can form structures. That's how I remember plasma, but I'd look it up to be sure. Those are the four fundamental states of matter, but there is a fifth state called the Bose-Einstein Condensate. This occurs when separate atoms are cooled to absolute zero, or zero degrees in Kelvin. I'd explain further, but I had to look this up, since I'd only known the name of the fifth state of matter, not what it actually is. Again, you'd probably be better off looking this up, I'm not an expert at this. I only just finished my Honors Chemistry class...anyways, good luck. For science, comrade!(11 votes)
- How come oxygen is a gas and hydrogen is a gas but water is a liquid? Shouldn't it also be a gas?(7 votes)
- this is not a question,, but i just wanted to say something - i loved the way you said that a bunch of falling sals can move a turbine(7 votes)
- At0:23, Sal shows 3 states of matter, solid,liquid,and gas. But if you search it up at science websites, and many other places such as google and bing, they say there is a 4th state of matter (PLASMA).So is plasma really a state of matter?(3 votes)
- How many states of matter there are depends on whom you ask and how they distinguish phases. This count could range anywhere from 5 or 6, to hundreds.
But for a beginning chemistry student, there are only four that are important. Plasma is mainly important in understanding lightning and certain modern technologies.(5 votes)
I think we're all reasonably familiar with the three states of matter in our everyday world. At very high temperatures you get a fourth. But the three ones that we normally deal with are, things could be a solid, a liquid, or it could be a gas. 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. Just think of it as heat contact, because that's really what it is. But anyway, on this axis, I have heat. So this is when I have very little heat and I'm increasing my heat. And this is temperature. Now let's say at low temperatures I'm here and as I add heat my temperature will go up. Temperature is average kinetic energy. Let's say I'm in the solid state here. And I'll do the solid state in purple. No I already was using purple. I'll use magenta. So as I add heat, my temperature will go up. Heat is a form of energy. And when I add it to these molecules, as I did in this example, what did it do? It made them vibrate more. Or it made them have higher kinetic energy, or higher average kinetic engery, and that's what temperature is a measure of; average kinetic energy. So as I add heat in the solid phase, my average kinetic energy will go up. And let me write this down. This is in the solid phase, or the solid state of matter. Now something very interesting happens. Let's say this is water. So what happens at zero degrees? Which is also 273.15 Kelvin. Let's say that's that line. What happens to a solid? Well, it turns into a liquid. Ice melts. Not all solids, we're talking in particular about water, about H2O. So this is ice in our example. All solids aren't ice. Although, you could think of a rock as solid magma. Because that's what it is. I could take that analogy a bunch of different ways. But the interesting thing that happens at zero degrees. Depending on what direction you're going, either the freezing point of water or the melting point of ice, something interesting happens. As I add more heat, the temperature does not to go up. As I add more heat, the temperature does not go up for a little period. Let me draw that. For a little period, the temperature stays constant. And then while the temperature is constant, it stays a solid. We're still a solid. And then, we finally turn into a liquid. Let's say right there. So we added a certain amount of heat and it just stayed a solid. But it got us to the point that the ice turned into a liquid. It was kind of melting the entire time. That's the best way to think about it. And then, once we keep adding more and more heat, then the liquid warms up too. Now, we get to, what temperature becomes interesting again for water? Well, obviously 100 degrees Celsius or 373 degrees Kelvin. I'll do it in Celsius because that's what we're familiar with. What happens? That's the temperature at which water will vaporize or which water will boil. But something happens. And they're really getting kinetically active. But just like when you went from solid to liquid, there's a certain amount of energy that you have to contribute to the system. And actually, it's a good amount at this point. Where the water is turning into vapor, but it's not getting any hotter. So we have to keep adding heat, but notice that the temperature didn't go up. We'll talk about it in a second what was happening then. And then finally, after that point, we're completely vaporized, or we're completely steam. Then we can start getting hot, the steam can then get hotter as we add more and more heat to the system. So the interesting question, I think it's intuitive, that as you add heat here, our temperature is going to go up. But the interesting thing is, what was going on here? We were adding heat. So over here we were turning our heat into kinetic energy. Temperature is average kinetic energy. But over here, what was our heat doing? Well, our heat was was not adding kinetic energy to the system. The temperature was not increasing. But the ice was going from ice to water. So what was happening at that state, is that the kinetic energy, the heat, was being used to essentially break these bonds. And essentially bring the molecules into a higher energy state. So you're saying, Sal, what does that mean, higher energy state? Well, if there wasn't all of this heat and all this kinetic energy, these molecules want to be very close to each other. For example, I want to be close to the surface of the earth. When you put me in a plane you have put me in a higher energy state. I have a lot more potential energy. I have the potential to fall towards the earth. Likewise, when you move these molecules apart, and you go from a solid to a liquid, they want to fall towards each other. But because they have so much kinetic energy, they never quite are able to do it. But their energy goes up. Their potential energy is higher because they want to fall towards each other. By falling towards each other, in theory, they could do some work. So what's happening here is, when we're contributing heat-- and this amount of heat we're contributing, it's called the heat of fusion. Because it's the same amount of heat regardless how much direction we go in. When we go from solid to liquid, you view it as the heat of melting. It's the head that you need to put in to melt the ice into liquid. When you're going in this direction, it's the heat you have to take out of the zero degree water to turn it into ice. So you're taking that potential energy and you're bringing the molecules closer and closer to each other. So the way to think about it is, right here this heat is being converted to kinetic energy. Then, when we're at this phase change from solid to liquid, that heat is being used to add potential energy into the system. To pull the molecules apart, to give them more potential energy. If you pull me apart from the earth, you're giving me potential energy. Because gravity wants to pull me back to the earth. And I could do work when I'm falling back to the earth. A waterfall does work. It can move a turbine. You could have a bunch of falling Sals move a turbine as well. And then, once you are fully a liquid, then you just become a warmer and warmer liquid. Now the heat is, once again, being used for kinetic energy. You're making the water molecules move past each other faster, and faster, and faster. To some point where they want to completely disassociate from each other. They want to not even slide past each other, just completely jump away from each other. And that's right here. This is the heat of vaporization. And the same idea is happening. Before we were sliding next to each other, now we're pulling apart altogether. So they could definitely fall closer together. And then once we've added this much heat, now we're just heating up the steam. We're just heating up the gaseous water. And it's just getting hotter and hotter and hotter. But the interesting thing there, and I mean at least the interesting thing to me when I first learned this, whenever I think of zero degrees water I'll say, oh it must be ice. But that's not necessarily the case. If you start with water and you make it colder and colder and colder to zero degrees, you're essentially taking heat out of the water. You can have zero degree water and it hasn't turned into ice yet. And likewise, you could have 100 degree water that hasn't turned into steam yeat. You have to add more energy. You can also have 100 degree steam. You can also have zero degree water. Anyway, hopefully that gives you a little bit of intuition of what the different states of matter are. And in the next problem, we'll talk about how much heat exactly it does take to move along this line. And maybe we can solve some problems on how much ice we might need to make our drink cool.