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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 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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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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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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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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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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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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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 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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Now here is fluorine, same skeleton, only fluorine has seven valence electrons.
这是氟，同样的结构，只有氟有七个价电子。
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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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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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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 if we look at sulfur, what we need to do is take the valence electrons in sulfur, and there are 6.
因此如果我们来看硫原子的话，我们需要做的是,将硫的价电子，有六个。
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We told you that phosphorous has 5 valence electrons plus 3 from each of the hydrogens, so we have a total of 8 valence electrons.
我告诉过你们磷有5个价电子,另外氢有3个，所以我们一共有8个价电子。
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And to do this we're going to introduce valence bond theory, and the idea of hybridization of orbitals.
在这之前我们要引入价电子成键理论，和杂化轨道的概念。
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In valence bond theory, the focus is on discussing the bonds, but it should look very familiar to you, because there's two types of bonds that we want to discuss here.
在价电子成键理论中，所关注的是讨论成键，但这对于你们来说应该很熟悉，因为这是我们要讨论的两种键。
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I'm averaging it over the entire set of valence electrons which gives me 1.91 MJ per mole.
我是在整个价电子的集合上作平均,最后得到1。91兆焦每摩尔。
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But, we know for example that magnesium, when it reacts, it reacts with both of its electrons, not just one of its electrons.
但是我们知道，拿镁来说，当它发生反应的时候，并不只是，某一个电子反应，而是两个价电子都发生反应。
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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 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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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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And if we go on to step three where we figure out how many we would need for full octets, it's just going to be 2 times 8, so we have 16.
而如果我们继续到第三步,判断一下填满所有“八隅体“需要多少个价电子，结果应该就是二乘以八，也就是十六个。
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So then in order to figure out the complete number of valence electrons in our molecule, we just add 5 plus 4 plus 1.
那么接下来为了得到,这个分子中价电子的总个数，我们只需要将五加上四，再加上一。
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So we need to add those 2 valence electrons left as lone pair electrons in our structure.
因此我们需要将这两个剩下的价电子,作为孤对电子加到我们的结构中。
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