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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 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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This is the clouds or the orbitals, electron cloud interactions.
这就是电子云或轨道电子云相互影响。
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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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The reason that there is increased electron density here is you can see that these two orbitals come together and constructively interfere.
你们可以看到两个轨道,靠在一起相长叠加,这就是为什么中间的电子态密度增加了。
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So what we're doing is filling in those eight electrons following the Aufbau principle, so our first electron is 1s going to go in the 1 s, and then we have no other options for other orbitals that are at that same energy, 1s so we put the second electron in the 1 s as well.
它会是什么样子呢,我们正在做的是将这8个电子按照奥弗,堡原理进行填充,所以我们第一个电子将会进入，然后我们没有其他的,轨道的选择在同一个能级，所以我们把第二个电子也放入。
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When you are done you have three electron pairs in bonding orbitals.
当你完成的时候,成键轨道上共有三对电子。
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And the third fact that we need to keep in mind is that spins remain parallel prior to adding a second electron in any of the orbitals.
第三个事实是我们需要记住在,每个轨道加入第二个电子之前,自旋保持平行。
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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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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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It makes sense, right, because they're the furthest away from the nucleus, they're the ones that are most willing to be involved in some chemistry or in some bonding, or those are the orbitals that are most likely to accept an electron from another atom, for example. So the valence electrons, those are the exciting ones.
它讲得通，对，因为它们距离,原子核最远，它们是最容易发生,化学反应和结合的地方，另一个原子的电子的轨道或者它们是,最容易接受，举个例子所以价电子，他们是活跃的电子。
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So you can see here in this slide we have the atomic orbitals for the two hydrogen atoms, each of them have one electron in them, hydrogen has one electron in a 1 s orbital.
从这个幻灯片你们可以看到我们,有这两个氢原子的原子轨道，每个上面有个电子，氢原子上面有一个电子在1s轨道上。
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Would you expect to see electron promotion in nitrogen where we pull one of these 2 s electrons into one of the 2 p orbitals?
你们觉得会看到电子激发吗？,1个2s电子,跑到2p轨道里？
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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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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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And by state we just mean orbital, so if we're looking at the p orbitals here, x that means that a single electron goes in x, and then it will go in the z orbital before a second one goes in the x orbital.
我们说的态仅仅意味着轨道，所以如果我们观察这里的p轨道，那意味着单个电子进入，然后它会进入z轨道,在它第二个进入x之前。
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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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And if we hybridize these orbitals in carbon, what we end up with is having two hybrid orbitals, and then we're going to be left with two of our p orbitals that are each going to have an electron associated in them.
如果我们杂化碳原子里这些轨道，我们能得到两个杂化轨道，另外剩下两个p轨道,每个里面有一个电子。
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So if we're comparing the difference between these 2 now, what you'll notice is that in nitrogen we have all half-filled 2 p orbitals, and now, once we move into oxygen, we actually have to add 1 more electron into 1 of the 2 p orbitals.
那么如果我们来比较下它们两个有什么不同，你会发现氮的，2，p，轨道,都是半满的，现在，我们继续看一下氧，我们不得不在其中一个，2，p，轨道上,再放上一个电子。
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There's not two bonds, that's one pi bond, and the reason is because it's 2 p orbitals coming together, and remember p orbitals have electron density above and below the axis, so when they come together, it kind of looks like one bonds, but essentially what we have here is one pi bond.
这不是两个键，这是一个π键，因为这是两个2p轨道组合而成的，记住p轨道在键轴之上,和键轴之下都有电子密度，当它们靠近时，这看着很像两个键，但本质上它是一个π键。
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I think most and you are familiar with the Aufbau or the building up principle, you probably have seen it quite a bit in high school, and this is the idea that we're filling up our energy states, again, which depend on both n and l, one electron at a time starting with that lowest energy and then working our way up into higher and higher orbitals.
我认为你们大多数熟悉奥弗堡,或者构建原理，你们可能,在高中见过它，又一次,这是我们填充能级的观点，与n和l有关，一个电子每次从,最低的能级开始,然后以我们的方式上升到,更高更高的轨道。
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