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So when we talk about orbitals in multi-electron atoms, they're actually lower in energy than the corresponding h atom orbitals.
它们的能量实际上,比对应的氢,原子轨道要低。
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So, why don't you go ahead and tell me, keeping that in mind, which atom in terms of h c or n would you expect to be in the center of hydrogen cyanide?
那么，请大家来告诉我，并且记住它，你认为氢，碳和氮中哪个原子,应该在氰化氢的中间呢？
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All right, so the type of bond energies that we can go and look up in tables are individual atom bonds, H-H, F-F, and the like.
好的，键能的类型,我们能够在表中查到,都是独立的原子键，H-H，F-F以及类似的。
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So, we see that the two h atoms separate have a certain energy that's lower than when the electron's not with the atom.
那么，我们看到两个分开的氢原子所具有的能量,比原子中没有电子时更低。
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H2 So the simplest case we can think of is with h 2 where we have two unpaired electrons, each in a 1 s orbital of a separate h atom.
最容易想到的例子是2,我们有两个未配对电子，每个都在一个分开的1s轨道上。
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The more important thing that I want you to notice when you're looking at this wave equation for a 1 s h atom, is the fact that if you look at the angular component of the wave function, you'll notice that it's a constant.
我要你们注意的,更重要的一点是,当你们看到,这个氢原子1s轨道方程的时候，如果你们看,波函数，的角向部分，你们会发现它是一个常数。
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What I want to point out also is that this h hat, the Hamiltonian operator written out for the simplest case we can even imagine, which is a hydrogen atom where we only have one electron that we're dealing with, and of course, one nucleus.
我也想指出的是，我们能想到的最简单情况,的哈密顿算符，是一个只有一个电子,也只有一个原子核的氢原子。
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And in doing that, we'll also talk about the shapes of h atom wave functions, specifically the shapes of orbitals, and then radial probability distribution, which will make sense when we get to it.
为了这样做，我们要讲一讲，氢原子，波函数的形状，特别是轨道的形状，然后要讲到径向概率分布，当我们讲到它时，你们更能理解。
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So, in talking about covalent bonds, we should be able to still apply a more general definition of a chemical bond, which should tell us that the h 2 molecule is going to be lower in energy than if we looked at 2 separate hydrogen atom molecules.
那么，既然提到了共价键，我们应该还可以,给化学键下一个更普遍的定义,那就是告诉我们氢分子能量应该更低,与两个分开的氢的单原子分子相比。
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