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So, now with this framework, I said that talking about these valence electrons might give us some insight into chemical reactivity.
所以，现在对于这个结构，我认为讨论价电子能,会让我们对化学反应有更深的领悟。
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So, what we do as our seventh step is then figure out if we have any extra valence electrons left at all.
那么，第七步要做的是看看,我们还有没有剩下的价电子。
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And, at the other extreme, we have elements with very high value, elements with high average valence electron energy.
另外，在另一端，我们有原子序数较大的元素，这些元素有着较高的平均化合价和电子能。
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So we started with 10 valence electrons, we used up 8 of those electrons in terms of making bonds.
我们一开始有十个价电子，然后用掉了八个电子来成键。
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CO Right, so you take the co here, and we take the valence here, and out of that comes covalent.
好了，然后我们看到，我们可以看到他的化合价，他们成共价键。
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OK, then it says draw a single bond from each surrounding atom to the central atom, and subtract two valence electrons.
后将中心原子与其相邻原子之间,连上单键，然后减掉2个价电子。
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if we're actually thinking about electron configuration and we look at lithium, sodium and potassium, these all have one valence electron.
让我们来想一想,锂，钠，钾的电子排布，它们都只有一个价电子。
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OK, elements with low average valence electron energy, and here I'm saying below 11 electron volts, these are good electron donors.
平均价电子能都较低的元素，我是指那些低于11电子伏的，这些是很好的电子给体。
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Its average valence electron energy is 5.2 electron volts, which is a heck of a lot less than 11.
它的平均价电子能是,5。2电子伏，那比11电子伏要少得多。
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Over here in the lower left corner, we have elements that as a group have very low values of average valence electron energy.
在底层的左侧角落，我们看到以组为单位的,价电子能较低的元素。
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So, seven asks us if we have any valence electrons left, and how many valence electrons do we have left?
那么，第七步问我们是否还有价电子剩下，我们剩下了几个价电子？
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So in terms of total numbers that we would need to complete our octets and fill our valence shells, we would need 18 electrons.
因此要填满我们的“八隅体“,排满所有的价壳层，我们总共需要十八个电子。
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In this case, 6 valence electrons for each oxygen, so we have 18 total valence electrons.
在这种情况下，每个氧原子都有六个价电子，因此我们总共有十八个价电子。
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So, in this case, we're just drawing the molecular orbital diagram for the valence electrons, so we have three for each.
所以在这个例子里面，我们只需要画出,价电子的分子轨道图，所以每个有3个电子。
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The reason is because we already have a full valence shell for our hydrogen, it doesn't want any more electrons.
原因是因为我们的氢,已经有一个排满的价壳层了，它不再需要多余的电子了。
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And we do so by a quantity called the average valence electron energy.
我们可以通过,一个叫做平均价电子能的量来解决这一问题。
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For the carbon, we start with 4 valence electrons, we have 0 lone pair electrons minus 4, and we end up with a formal charge of 0.
对于碳，我们从四个价电子开始，我们有零个孤对电子，再减去四，最终我们有零个形式电荷。
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We have to account for that in some way because we know that they don't have identical average valence electron energies.
我们需要从一些方面来解释一下,因为我们都知道,他们没有相同的,平均价电子能。
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So we have a total of 2, 4, 6, 8, 10 valence electrons, so I'll make sure I count to 10 as we fill up our molecular orbitals here.
我们一共有2，4，6，8，10个价电子，所以我一边填一边要确认,我数到10。
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Yeah, so also 4. We started with 10 valence electrons, we used up 6 of those as bonding electrons, so we have 4 left, which will be lone pair electrons.
对，也是四个，我们从十个价电子开始，只用了六个来成键，因此我们还剩下四个，它们将成为孤对电子。
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So in terms of remaining valence electrons we have 12, so we can finish off each of our Lewis structures, so that's our first structure there, and our second structure there.
那么关于剩下的价电子，我们有十二个，因此我们可以完成这两个路易斯结构了，那么这是我们的第一个结构，而那是我们的第二个结构。
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Step three in our Lewis structure rules is to figure out how many electrons we would need in order for every single atom in our molecule to have a full valence shell.
路易斯结构规则的第三步是,找出让分子中每个原子的价壳层,都排满应该需要多少个价电子。
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OK PROFESSOR: Valence electrons. OK, sometimes you're going to be asked to draw a molecular orbital diagram where you're asked to include all electrons, and sometimes it will specifically say only include valence electrons.
教授：价电子，有时候你画一幅分子轨道图,有时候要求你画出所有的电子，有时候特别要求,只包括价电子。
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So the 3 s 1, or any of the other electrons that are in the outer-most shell, those are what we call our valence electrons, and those are where all the excitement happens.
它们是经常发生激发情况的,那也是我们所看到，我们称之为价电子，它们是经常发生激发情况的。
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And the idea is that when you do these Lewis dot structures, we're representing electrons with dots, which we'll see in a minute, and each dot is going to represent a valence electron.
而当你遇到这些路易斯点结构时，我们会将电子用点来表示，我们马上就会看到，每个点都代表了一个价电子。
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So in terms of nitrogen that starts off with a valence number of 5, again we have 2 lone pair electrons in the nitrogen, and again, we have 6 electrons that are shared.
对于氮来说,我们应该从五个价电子开始，同样，氮也有两个孤对电子，共用电子的个数也一样，是六个。
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So then, I could say that the average valence electron energy for oxygen would then be, I've got two s electrons.
所以，我可以说,氧的平均价电子能,就是，以我得到的两个s轨道的电子来算。
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It's got an average valence electron energy of about 16 eV, 16.5 eV, which is a lot greater than 11.
它的平均价电子能,大约是16eV，16。5eV，那比11要多很多。
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All right, so that's really all there is to thinking about valence bond theory in terms of the most simple explanation here.
好了，这就是,价电子轨道理论的,最简单的解释。
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So in oxygen again, this is just showing the valence electrons, so we end up having six valence electrons from each oxygen atom.
所以在氧里面，这里只展示价电子，我们最后每个氧得到6个价电子。
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