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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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We started talking about these on Wednesday, and what we're going to start with is considering specifically the wave functions for multi-electron atoms.
我们从周三开始讨论这些，而且我们将要以特别地考虑,多电子原子的波函数,为开始。
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And this is the energy level diagram for multi-electron atoms.
看一下能量级图表中,多电子原子的部分。
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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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So, the wave functions for multi-electron atoms.
所以，对于多电子原子的波函数。
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So let's compare what some of the similarities and differences are between hydrogen atom orbitals, which we spent a lot of time studying, and now these one electron orbital approximations for these multi-electron atoms.
很长时间的氢原子轨道和,现在多电子原子中,的单个电子轨道近似，我们可以对比，它们之间,的相似性和不同。
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All right, so today we're going to fully have our discussion focused on multi-electron atoms.
好了，今天我们将要完整的讨论,关于多电子原子的问题。
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So on Friday, we'll start with talking about the wave functions for the multi-electron atoms.
在周五，我们要开始讨论,多电子原子的波函数。
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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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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。
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So now that we can do this, we can compare and think about, we know how to consider wave functions for individual electrons in multi-electron atoms using those Hartree orbitals or the one electron wave approximations.
现在我们可以做这些了，我们可以对比和考虑，我们知道如何用哈特里轨道,或者单电子波近似去考虑,多电子原子中的单个电子波函数,所以对于我们研究了。
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So, one we finish our discussion of how we think about multi-electron atoms, we can go right on and start talking about these other things.
一旦我们结束了,多电子原子的讨论,我们马上就可以,开始讨论这些问题。
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And once we do that, we're actually going to move on to multi-electron atoms.
在这之后，我们就可以继续多电子原子的内容。
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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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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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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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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。
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Soon when we're talking about multi-electron atoms, and I just want to introduce it here, that it is sort of opposing ideas that even though the s is the biggest and it's most likely that the electron's going to be furthest away from the nucleus, that's also the orbital in which the electron can, in fact, penetrate closest.
当我们说多电子原子时，我这里要先介绍一下，这些概念有些相反,虽然ｓ轨道最大,所以电子最可能远离原子核，但它上面的最容易，穿透到离原子核最近。
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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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But when we get to the multi-electron atoms, we see that actually the p orbitals are higher in energy than the s orbitals.
但是当我们来看多电子原子时，可以看到实际上p轨道的能量,要高于s轨道。
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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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We know that the orbitals for multi-electron atoms depend both on n and on l.
我们知道对于多电子原子轨道,是依赖于n和l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。
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The other main difference that we're really going to get to today is that in multi-electron atoms, orbital energies depend not just on the shell, which is what we saw before, not just on the value of n, but also on the angular momentum quantum l number. So they also depend on the sub-shell or l.
我们今天要讨论的,另一个很重要的区别就是,在多电子原子中，轨道能力不仅仅依赖于，我们以前看到的外层，不仅仅依赖于n的值，而是与角动量量子数也有关系,所以它们也依赖于亚外层或者。
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