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We don't have to just stick with carbon, we can think about describing other types of atoms as well using this hybridization.
我们不用局限于碳，我们可以考虑利用杂化轨道,描述其它类型的原子。
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So you see in the hybrid orbital we actually have a larger lobe on top where they constructively interfered.
所以你们可以看到在杂化轨道里,我们上面,由很大的一叶相长干涉。
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If I now hybridize these, if I take these and I make four symmetric, now, these are just the sp3 orbitals.
如果我将他们杂化，然后形成4个对称的轨道，这就是sp3轨道。
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So why don't you have a seat on the chair on the right-hand side there. All right.
你坐在杂这个椅子上,在这里的右手边，好的。
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And if I'm running an exponential algorithm, any guesses?
杂度是指数级的呢？,有人猜猜么？
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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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PROFESSOR: All right, start again, what's the hybridization of the carbon atom?
好了，再说一遍，碳原子的杂化轨道是什么？
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All right, so let's consider our methane situation now that we have our hybrid orbitals.
好，让我们考虑甲烷的情形,既然我们有了杂化轨道。
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So it's going to be carbon, and then what's the hybridization here?
这是碳，杂化的什么样的？
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He did some hybridization of methane.
就是甲烷的杂化。
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If we think about bringing in those last two carbons, what you can see is that for every carbon, two of its hybrid orbitals are being used to bond to other carbons.
如果我们考虑引入最后两个碳原子，你会看到的是对于每个碳原子，其中的两个杂化轨道,和另外的碳原子成键。
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And an important thing to remember when we talk about resonance hybrids is that the structure it's not 1/2 the time this structure, and 1/2 of the time this structure, it's actually some combination or some average between the two structures.
而当我们讨论共振杂化的时候,有一件重要的事情需要牢记,那就是这种结构并不是,一半时间处于这种结构的状态，而另外一半时间又变成了这种结构的状态，它实际上是两种结构在,一定程度上的组合或者平均。
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So if we go ahead and hybridize our p orbitals and our s orbitals, we'll switch from having these original orbitals to having something called hybrid orbitals.
如果我们,杂化p轨道和s轨道，我们会从原来的轨道,变成一个叫杂化轨道的东西。
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So it's along the bond axis and it's between a carbon s p 2 hybrid, and then the hydrogen is just a 1 s orbital that we're combining here.
所以它是沿着键轴方向的,而且这里是一个碳sp2杂化轨道，和一个氢的1s轨道的结合,在这里我们可以合并他们。
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And if we think about the six hydrogens, now each of those are going to bind by combining one of the carbon hybrid orbitals to a 1 s orbital of hydrogen.
如果我们考虑有六个氢原子，每个都会合起来,碳杂化轨道成键,每个氢的1s轨道。
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This bond is polar, but again, as I alluded to earlier, because the carbon is centered in the tetrahedron, because of the sp3 hybridization, the molecule itself is symmetric and nonpolar.
这个键是非极性的，但是，我们断言过早，因为C是中心原子，由于sp3杂化，这个分子本身是非极性的且对称的。
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So let's switch to thinking about oxygen hybridization here.
让我们考虑一下氧的杂化。
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Remember, we didn't hybridize the 2 p y orbital, so that's what we have left over to form these pi bonds.
记住，我们并没有杂化2py轨道，这是我们剩下的那个行成了π键。
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So let's quickly talk about our last type of hybridization that we're going to discuss today, which is s p hybridization.
我们今天要讨论的最后一个类型的杂化,也就是sp杂化。
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And hybrid orbitals are all going to be completely equal, and lower in energy than the p orbital.
杂化轨道是完全相等的，你会注意到它们的能量比s轨道高，比p轨道低。
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Again, the name is very straightforward, it comes from 1 s and 2 p orbital, so it will be s p 2.
所以，如果我们杂化这三个轨道，我们最后会得到的是sp2杂化轨道，同样，这个名字是很直接的。
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We can still hybridize all these orbitals, however, so we can still form four hybrid orbitals, which are again, 2 s p 3 hybrid orbitals.
但我们仍然可以杂化这些轨道，所以我们还是可以形成4个杂化轨道，同样的，是2sp3杂化轨道。
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So let's take a look at another case where we have s p 2 hybridization, we can actually also have it happen in carbon.
它是B2sp2杂化轨道,和H1s轨道的相互作用，让我们看看另外一个。
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I have four bonds that are of equal energy, and he called this an sp3 hybrid.
我已经将4个能量相等的键画好了，他把这称为sp3杂化。
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So, if we think about this z bonding axis between the two carbon atoms, we can picture overlap of those s p hybrid orbitals, and then we can also picture bonding to hydrogen.
如果我们考虑,两个碳原子之间的z成键轴，我们可以画出sp杂化轨道的交叠，我们也可以画出和氢原子的成键。
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The reason that it's a sigma bond is sp3 because the s p 3 hybrid orbital is directly interacting with the 1 s orbital of the hydrogen atom, and that's going to happen on the internuclear axis, they're just coming together.
它是sigma键的原因,是因为,杂化轨道直接和氢原子1s轨道相互作用，它们作用发生在核间轴上，它们会到一起。
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So, this forms a tetrahedron, which forms the sp3 hybrid orbitals.
这就形成了一个四面体，它是由sp3杂化轨道形成的。
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So again, we can think of an example here.
和三个杂化的sp2轨道。
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So if we don't have to hybridize one of the p orbitals, we can actually end up with a lower energy situation, because now these s p 2 orbitals are 1/3 s character, and only 2/3 p character, instead of 3/4.
我们的杂化轨道就有更多的p轨道成分，所以它们的能量更高，如果我们不杂化这个p轨道，我们可以得到一个能量更低的情况。
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So essentially, we have two ethene or ethylene molecules here to start with where these blue are our 2 s p 2 hybrid orbitals, so you can see that for each carbon atom, one is already used up binding to another carbon atom.
本质上，我们从两个乙烯分子开始,蓝色的是2sp2杂化轨道，你可以看到，对于每一个碳原子，其中一个已经用来和另外一个碳原子成键。
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