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AP.Chem:
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Video transcript

in a previous video we introduced ourselves to the idea of bonds and the idea of ionic bonds where one atom essentially is able to take electrons from another atom but then because one becomes positively charged and the other becomes negatively charged they get attracted to each other now we're going to go to the other end of the bonding spectrum where instead of stealing electrons from each other we're going to share them let's say we're dealing with two oxygen atoms so let me draw one oxygen here a neutral oxygen has eight electrons total but six of them are in its outer shell so it has one two three four five six valence electrons and the way that I arrange them is I paired them up last so you have these two valence electrons that are not paired with another electron and now let me draw another oxygen and I'm going to do it with a different color so we can keep track of the electrons so another oxygen right over there also has six valence electrons one two three four five six valence electrons now this oxygen on the left in order to become more stable it would love to somehow gain or maybe share two more electrons and of course this oxygen on the right it's still oxygen it also would love to gain or share two more valence electrons so how could it do it well what if the oxygen on the Left shared this electron and this electron with the oxygen on the right and the oxygen on the right shared this electron and this electron with the oxygen on the left well if they did that you would have something that looks like this you have your oxygen on the left you have the oxygen on the right and the way we show two electrons that are being shared let's say these two electrons are being shared is just a line like this this shows that there are two electrons that are being shared by these two oxygens and let's say that these two electrons are also being shared you would do that with a line like this and then we could draw the remainder of the valence Tron's this oxygen on the left head outside of the electrons that are being shared it had four more valence electrons and then the oxygen on the right had four more valence electrons one two three four now what's interesting here is the shared electrons these are going to cause these oxygens to stick together if they don't stick together these electrons aren't going to be shared so what we have formed here is known as a covalent bond covalent bond and what's interesting is it allows both of these oxygens in some ways to be more stable from the left oxygens point of view it had six valence electrons but now it's able to share two more remember each of these bonds each of these lines represent two electrons so this oxygen could say hey I get to have 1 2 3 4 6 8 electrons that I'm dealing with and the same thing is going to be true of this oxygen on the right now there are some covalent bonds that are between not so equals so for example if we're talking about water and if we're talking about how oxygen bonds with hydrogen so if we have oxygen right over here once again I can draw it six valence electrons 1 2 3 4 5 and let me just draw the sixth one right over there and if I have hydrogen hydrogen has one valence electron so let's say that's a hydrogen right over there with one valence electron maybe another hydrogen right over there with one valence electron oxygen and hydrogen form covalent bonds in fact that is how water is formed and so what would that look like well it would look like this you have oxygen right over here you have these two pairs of electrons that I keep drawing and then this electron right over here could be shared with the hydrogen and that hydrogen is electron could be shared with the oxygen so that forms a covalent bond with this hydrogen and then this electron from the oxygen can be shared with the hydrogen and that electron from the hydrogen can be shared with the oxygen and so that would form a covalent bond with that other hydrogen and now here once again oxygen can kind of pretend like it has eight valence electrons two four six eight and the hydrogen's can kind of pretend that it has two valence electrons but the one difference here is that oxygen is a lot more electronegative than hydrogen is to the right of hydrogen it's in this top right corner outside of other than the noble gases that really like to hog electrons so what do you think is going to happen here well the electrons in each of these covalent bonds are going to hang out around the oxygen more often than around the hydrogen so the electrons spend more time around the oxygen you're going to have in general more negative charge around the oxygen and so you're going to have a partial negative charge on the oxygen end of the water molecule and then you're going to have partial positive charges on the hydrogen ends of the molecules and in case you're curious that little symbol I'm using for partial that's the lowercase Greek letter Delta which is just the convention in chemistry and so this type of covalent bond because there is some polarity one side has more charge than the other this is known as a polar covalent bond polar covalent bond
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