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。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

This should make sense, because if an atom has a very high electron affinity, that means it's really happy taking an electron from another atom, or taking a free electron -- that that's very favorable.

这应该是合理的，因为如果一个原子有很高的电子亲和能，这意味着,它非常乐意从另外一个原子那里夺取一个电子，或者得到一个自由电子--这是非常利于发生的。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

We can also look at the energy equation now for a multi-electron atom.

我们也可以看到现在对于,一个多电子原子的能量方程。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

A kind of consequence of this is if we're thinking about a multi-electron atom, which we'll get to in a minute where electrons can shield each other from the pull of the nucleus, we're going to say that the electrons in the s orbitals are actually the least shielded.

这样的一个后果就是,如果我们考虑一个多电子原子，我们等会就会讨论到它,电子会互相,屏蔽原子核的吸引，我们说ｓ轨道电子,更不容易被屏蔽。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

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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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。

麻省理工公开课 - 化学原理课程节选

So, essentially when we're talking about these equations up here, all we're doing is talking about the regular Rydberg formulas, but instead we could go back and re-derive the equation for any one electron atom, which would just mean that we put that z squared term in the front.

所以本质上,当我们讨论，这些问题时，我们说的是常规的，Rydberg公式，但对任何其他单电子原子，我们不用,从头再推到，而是仅仅把，z平方项放在前面。

麻省理工公开课 - 化学原理课程节选