- Hydrogen bonding in water
- Hydrogen bonds in water
- Capillary action and why we see a meniscus
- Surface tension
- Cohesion and adhesion of water
- Water as a solvent
- Specific heat, heat of vaporization, and density of water
- Importance of water for life
- Lesson summary: Water and life
- Structure of water and hydrogen bonding
Discussion of the properties of water that make it essential to life as we know it: polarity, "universal" solvent, high heat capacity, high heat of vaporization, cohesion, adhesion and lower density when frozen.
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- Why is it only a partial charge instead of a full charge?(7 votes)
- It's a partial charge because half of the molecule is positive and the other half is negative. It's not a full charge because the full molecule is not ionized.
Since Oxygen likes to hog electrons (as he mentions in the video) most of the electrons will be staying around oxygen. Since electrons have a negative charge, that creates a negative charge around the side of the molecule that has the oxygen atom. Since there is a lack of electrons around the hydrogen side of the molecule, that makes that half positive. But since it's only HALF of the molecule, it's going to be a PARTIAL charge. Hope that helps.(20 votes)
- from7:45to7:56, you are assuming a world where water is less dense than ice. However, as you go to explain how a lake would freeze over if that was the case, you say, "And then over time, the entire lake or the entire pond would freeze over, and life would not be able to live in that pond. Because when water freezes, it breaks membrane-bound structures as we know it. And so that would not be suitable for life". But here you are considering a world where ice is denser than water, so this explanation is not valid. This is a bit technical, but I just wanted to point it out. Life would not be able to live because there would be no space left in the pond; animals and plants would not be able to move.(4 votes)
- Your opinions don't seem contradictory. In fact both seem correct. A world where ice is denser than water would not be able to support life at all.(16 votes)
- But what if there is life that does not need water, say on another planet..? we really don't know, but all life on earth needs water but it could be way different on a different planet.(6 votes)
- You may be right! We believe that a moon called Titan with(theory next) methane seas and
oceans(theory 2 starts) could support life!(ends)(5 votes)
- Why are the partial charges of water strong enough to separate Sodium and Chloride which both have a full charge. If it is simply a matter of tug of war between partial charges and full charges, shouldn't the full charges win?(5 votes)
- It is not just a single molecule of water vs the chloride ion. Each of the sodium and chloride ion is surrounded by more than one molecules of water. Sometimes, these water-solvation-attraction is enough to overcome the ion-ion attraction, and the crystal dissolves in water. Sometimes, for some other compounds, it is not, and the crystal remains insoluble(4 votes)
- At 2.00 why is it called a hydrogen bond and not a oxygen bond?(3 votes)
- Hydrogen bonding is a type of bonding between hydrogen and an electronegative atom such as oxygen, fluorine, and nitrogen.(4 votes)
- When water dissolves,do the little partials that make up water disappear?(3 votes)
- No. Say if water dissolves because of the sun, the particles will be in the air. Energy can't be created either destroyed.(2 votes)
- Does this mean water is a zwitterion?(1 vote)
- It is not, as its negatives are not in a single 'group', and are rather scattered in a tetrahedral shape around the oxygen.(4 votes)
- 3:30- it is mentioned that a sodium ion will get attracted to the O molecule. But isn't Na bonded to Cl chemically?
How can the Na be separated from Cl?(2 votes)
- how can sodium be hydrophilic when in its pure form it is extremely reactive when it comes in contact with water(2 votes)
- [Instructor] When we look out into the cosmos for alien life, many folks look for signs of water on moons or planets. And that's because life as we know it is dependent on water. And to understand that, we just have to take a closer look at some of the properties of water. So what you see here are some molecules of water. This might be a review for you. Every water molecule has one oxygen atom. And it is bonded to two hydrogens. So that is a hydrogen, and that is a hydrogen as well. And the nature of that bond, it is a covalent bond, which means that the oxygen shares electrons with each of the hydrogen atoms. But oxygen is more electronegative, and that's just a fancy way of saying that even though those electrons are shared, they're going to be spending more time around the oxygen than around the hydrogens. One way to think about it is oxygen likes to hog electrons more than hydrogen does. And since the electrons will spend more time around the oxygen than around the hydrogen, and because it's a bent molecule with the hydrogens on one side of the molecule, what happens is the side where the oxygen is, where the electrons spend more time, that gets a partially negative charge. So this is the lowercase Greek letter delta. That just means partially negative charge. And then the sides where the hydrogens are, those acquire a partial positive charge. And so what you see here is that a water molecule is not charged in aggregate. But either side has a partial charge, so it is a polar molecule. And so you can imagine when you put a bunch of water molecules together what might happen? Well, the partially positive side of one water molecule where the hydrogens are would be attracted to the partially negative side of another water molecule. And so they would be attracted, and this is known as a hydrogen, hydrogen, hydrogen bond. And I could keep drawing that. This is going to be partially positive here. This is going to be partially negative. They will attract. This oxygen end is going to be attracted to that hydrogen end. This oxygen end is going to be attracted to the that hydrogen end as well. And so it's this hydrogen bonding that gives water a lot of the properties that make it special that, as far as we know, for harboring life or for even allowing life to be possible. Life as we understand it needs a fluid environment. Things move around and bump into each other. And it's these hydrogen bonds, when the temperature and conditions are appropriate, that allow water to be in that liquid form where they're strong enough so that the water stays together, but they're weak enough so that they allow the water molecules to flow past each other. And not only does it provide a good fluid environment, it's a very good solvent. Water is often known as the universal, universal solvent, but it's worth putting a disclaimer here. Even though people say it is a universal solvent, that does not mean that it dissolves everything. Water does dissolve more things in its liquid state than anything else we know about. But there are many molecules that it cannot dissolve well. The things that it does dissolve well are polar molecules or things that have a charge. For example, when sodium chloride dissolves in water, a sodium ion is positive, so that is positively charged. And so you can imagine it might be attracted to the side of the water molecules where the oxygen is. But it dissolves well. But things that don't have charge don't tend to dissolve well in water. But even the property that there's certain things that it does not dissolve is also good for life. Later on in biology we're going to study phospholipid bilayers where you have these molecules where one end is hydrophilic, which means it's attracted to water molecules. And then the other ends are hydrophobic, which means they're not attracted to water molecules. And many evolutionary biologists believe that this property of having one side that's hydrophilic and one side that's hydrophobic would have allowed these molecules to start collecting into membranes, eventually forming these spherical membranes which could be the containers for early cellular life. Now, another property of water which makes it very suitable for life is it's high heat capacity. Sometimes you'll hear people say it has a high specific heat. The specific heat is the amount of energy needed to raise one gram of water by one degree Celsius. And you might say why does that matter for life? Well, many life forms can only operate within a certain range of temperatures. And so if it was really easy to raise the temperature of water really high or very low temperatures very fast, well, that would make it much harder for life to operate within water, or even life to be made up of water. A related idea to this is that water also has a high heat of vaporization. We talk more about this in detail in other videos, but this is talking about how much energy does it take for water to go from its liquid form to its gas form. And this has proven valuable in many life forms for a form of cooling where the vaporization of water, evaporative cooling, can take heat away from an organism so that it doesn't overheat. Other properties that are important about water include cohesion and adhesion. Cohesion is the property of water molecules that is attracted to other water molecules. And you saw it here with the hydrogen bonds. But then when you look at a macroscale, you'll see things like water droplets form. You've all seen water droplets, or dew droplets. These droplets couldn't form if not for the cohesion of water. And even one drop can be an environment in which thousands of microorganisms can live. Adhesion is the property of water where it can adhere to other things. You might have seen this in a glass test tube where it looks like the water is kind of crawling up the top of the sides. And that's because some of the polarity of the glass molecules of the test tube. But this property, along with the cohesion, is what allows water to transport nutrients, say, from the roots of a tree all the way to the top of a tree. These properties are also an action in our own blood vessels, when you get to the really small blood vessels, the capillaries. And that is called capillaries 'cause you have capillary action of water, which is due to its cohesion and its adhesion. A last property of water, and this is not an exhaustive list, is that it is less dense as a solid. So another way to think about it is ice, which is solid water, is less, less dense than liquid water. Now, you might be thinking why does that matter for life? Well, imagine the environments where we think life first arose. If you imagine some type of a pond, and this is the cross-section of it, if ice was more dense than liquid water, and for many substances that is the case, a solid form tends to be more dense, then what would happen? If it's cold up here in the air, say, in the winter, then this part would freeze. But then as it got more dense it would sink to the bottom right over there. Then the next surface water would freeze and sink to the bottom. And then over time, the entire lake or the entire pond would freeze over, and life would not be able to live in that pond. Because when water freezes, it breaks membrane-bound structures as we know it. And so that would not be suitable for life. But because ice is less dense than water, what typically happens is just that top layer freezes. And then it'll freeze down as things get colder and colder. But you have an entire environment where life can continue to thrive even when the air is much colder than what is suitable for life. And because of water's high specific heat, that temperature variation in that water is going to be much less than the temperature variation outside of the water, either in the air or on the land. So this is just an introduction, but hopefully it makes you appreciate water a little more. And remember, and I've said this in other videos, we are mostly water. One way to think about it is that each of us is made up of trillions of cells which are primarily made up of water and exist in a water-based environment. They coordinate with each other and eventually have emergent complexity that thinks that it is a sentient being like each of us.