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So in addition to having these two carbon bonds, we actually also have four carbon hydrogen bonds in addition to our carbon-carbon bonds.
在这碳碳之间的键以外，我们还有四个碳氢键,除了我们的碳碳键外。
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One of the main difference is is that when you're talking about multi-electron orbitals, they're actually smaller than the corresponding orbital for the hydrogen atom.
其中最主要的区别之一,是当你讨论多电子轨道时,它们实际上，要比对应的氢原子轨道,要小一些。
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There's not actually chemical covalent bonds that are formed but it's a non-covalent interaction, usually dominated by hydrogen bonding.
所以配体和受体之间不生成共价键,这是一种非共价化合反应,它们通常以氢键相联
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Well, we would have to H+ have one of these hydrogen atoms go to an H plus, * plus an electron, right? **H --> H+ + e-** So, now we have a hydrogen ion here.
我们先要让,一个氢原子变成氢离子，加上一个电子，对么*,我们现在有一个氢离子了。
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When we increase the potential between the 2 electrodes that we have in the tube -- we actually split the h 2 into the individual hydrogen atoms, and not only do that, but also excite the atoms.
当我们增大两个电极之间电压,我们有-我们可以把氢气2,分解成单个的氢原子，不仅这样，还能激发原子。
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The electrons are not equally shared and the carbon hogs the electrons a little bit more than the hydrogen, so the carbon is electron-rich and the hydrogen is just a little bit electron-deficient.
电子不是平均共享的,碳原子比氢原子吸引电子,更强烈一点点，所以碳原子是富电子,而氢原子是缺电子。
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And there again is another difference between multi-electron atom and the hydrogen atoms.
在多电子原子和氢原子,之间还有一个区别,当我们谈论多电子原子轨道时。
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As we see a little bit later, I could talk about the carbon-hydrogen bond in methane where there is a plurality of bonds. In this case, there is only the one bond but I just want to get the formulas.
因为我们后来看到一点点，我能讨论甲烷中的碳氢共价键,那有许多共价键，这种情况下，这只有一条共价键,但我想得到氟。
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So when we talk about the size of multi-electron orbitals, they're actually going to be smaller because they're being pulled in closer to the nucleus because of that stronger attraction because of the higher charge of the nucleus in a multi-electron atom compared to a hydrogen atom.
所以当我们讨论,多电子轨道的尺寸，它们实际上会变得更小,因为多电子原子的原子核,相比于氢原子,有更高的电荷量所以,有更强的吸引力,所以可以拉的更近。
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So, what we say here is we need to take a step back here and come up with an approximation that's going to allow us to think about using the Schrodinger equation when we're not just talking about hydrogen or one electron, but when we have these multi-electron atoms.
所有我们这里要说的是,我们需要退回一步,做一个近似,那样可以使我们用,薛定谔方程来考虑,让我们不是仅仅在讨论氢原子或者,一个电子的时候，而是多个电子的原子。
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Now I want to ask, what's the nature of the carbon-hydrogen bond?
现在我想问问，碳氢键的本质是什么？
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Is a hydrogen bond shorter, or is a nitrogen-nitrogen triple bond going to be shorter?
是氢的键更短，还是氮与氮的三键更短？
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Let's show that carbon-hydrogen is polar.
我们把他们的极性表示出来。
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And we can look at precisely why that is by looking at the equations for the energy levels for a hydrogen atom versus the multi-electron atom. So, for a hydrogen atom, and actually for any one electron atom at all, this is our energy or our binding energy.
而且我们可以精确地看看,为什么是这样的,通过看对于氢原子和,多电子原子能级的方程所以对于氢原子，事实上对于任何一个电子，这是我们的能量或者我们的结合能。
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Let's look at this carbon-hydrogen bond.
我们来看看这跟碳氢键。
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So, let's take a look here at an example of an energy diagram for the hydrogen atom, and we can also look at a energy diagram for a multi-electron atom, and this is just a generic one here, so I haven't actually listed energy numbers, but I want you to see the trend.
所以让我们来看看,一个例子氢原子的能量图，我们也可看看一个,多电子原子的能量图，这是一个普通的图谱，我没有列出能量的数字，但是我想让你们看这个趋势。
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So we can have our two hydrogen atoms come in here, and what we will find is - now that we have all of our orbitals filled up -- so thinking about what this angle is here, would you expect it to be less than or greater than what we saw for ammonia before?
我们在这里有两个氢原子，我们会发现,现在我们所有的轨道都填满了-,考虑一下这里的角度，你们觉得它比在氨中看到的,要大还是要小？
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So, if we look at this graph where what we're charting is the internuclear distance, so the distance between these two hydrogen atoms, as a function of energy, -- what we are going to see is a curve that looks like this -- this is the general curve that you'll see for any covalent bond, and we'll explain where that comes from in a minute.
因此，如果我们来看一看这幅曲线图,这里我们画的横坐标是核间距，也就是这两个氢原子之间的距离，纵坐标是能量，我们看到的这是能量关于核间距的曲线-,这是一条普遍的曲线，在研究任何共价键时你都会遇到，我们马上就会解释一下它是怎么来的。
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So for example, if you look at the 1 s orbital here, you can see that actually it is lower in the case of the multi-electron atom than it is for the hydrogen atom.
所以举例来说，如果你看到这里的1s轨道,你可以看到实际上,多电子原子情况的。
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And I want to really highlight here we're talking about for a hydrogen atom orbitals - with the same n value have the same energy.
我想强调的是,我们所说的,都是对单个的氢原子,和言的,对于同样的n值能量相同。
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For example, for the 2 s, again what you see is that the multi-electron atom, its 2 s orbital is lower in energy than it is for the hydrogen.
举例来说对于2s轨道，在多电子原子，中可以看到,它的2s轨道的能量低于氢原子的。
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Again the 2 p orbitals for the multi-electron atom, lower in energy than for the hydrogen atom.
p轨道能量,多电子原子的，低于氢原子的。
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This should make a lot of sense, because we know that a hydrogen has 1 s as it's outer-most or valence orbital, so it can be filled up just with two 1 s electrons.
这也是很合理的，因为我们,知道氢只有，1，s，轨道,这就是它最外层的轨道或者说价轨道，因此只要两个，1，s，电子就可以将它填满。
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It's a sigma bond, - and it's going to be -- N2sp3 no. OK, it's going to be nitrogen 2 s p 3, because it's a nitrogen atom, 1s and then hydrogen 1 s.
它是sigma键，它是-,不，OK，它是，因为这是个氮原子，然后是氢。
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So in terms of the carbon hydrogen bond, it's a sigma bond, - because we define it -- any time we are bonding to an atom, we have to keep redefining our bond axis to whatever two atoms we're talking about.
对于碳氢键，它是sigma键，因为我们定义它-,任何时候我们有原子成键，我们要重新定义键轴方向,为我们所讨论的两个原子方向。
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So what we end up with is one radial node for the 2 s orbital of hydrogen, and we can apply that for argon or any other multi-electron atom here, we also have one radial node for the 2 s orbital of argon.
那意味着它们都是径向节点,所以我们得出的结论是，氢的2s轨道是1个径向节点,我们可以将它应用，到氩或者任意一个多电子原子,对于氩的2s轨道。
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You don't need to know those, but just because it's a special case with the hydrogen atom, they do tend to be named -- the most important, of course, tends to be the Balmer series because that's what we can actually see being emitted from the hydrogen atom.
你们不需要记住,但因为这是氢原子的特例,人们想要命名它，最重要的是当然是Balmer系,因为它是我们可以看到的,从氢原子放出来的光谱。
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