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So for example, if we think about fluorine, 1 s 2 2 s 2 2 p 5 that has an electron configuration of 1 s 2, 2 s 2, 2 p 5, so all we would need to do is add one more electron to get the same configuration as for neon.
比如，如果我们考虑氟原子的话，它的电子排布是，因此我们所需要做的就是给它加上一个电子,使得它与氖原子的电子排布相同。
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s 2 2 s 2 2 p 6 This has the electron configuration of 1 s 2, 2 s 2, and 2 p 6.
它的电子排布是。
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The same thing when you're going from filling in the 2 s to putting that first electron into the 2 p.
当你填满，2，s，后再往，2，p，中,放第一个电子的时候就会发生这种问题。
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So, if we say that in this entire plane we have zero probability of finding a p electron anywhere in the plane, the plane goes directly through the nucleus in every case but a p orbital, so what we can also say is that there is zero probability of finding a p electron at the nucleus.
而只要是ｐ轨道,这个平面都直接，穿过原子核，那么我们,可以说在原子核上,找到一个ｐ电子的概率为零。
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But unlike the case with boron where we had an empty p orbital, we're actually going to have an electron in the p orbital of carbon as well.
但和硼里面有个空的p轨道不同，我们实际上有一个电子,在碳里p轨道里也有电子。
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And we can think about here we did get that energy for electron promotion that I mentioned before 2p where we moved the electron from the 2 s to the 2 p.
我们可以考虑,我们从哪里,获得了能量使电子,从2s激发到。
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Will it be if you take a 3 s electron from neutral silicone, if you take a 3 p electron from the neutral atom, or if you take a 3 p from the ion?
是从中性硅原子中拿走一个，3，s，电子呢，还是从中性硅原子中拿走一个，3，p，电子呢，又或者是从硅离子中拿走一个，3，p，电子呢？
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So we can think about what is our most loosely-bound electron, what's that highest energy orbital, and it's going to be the 2 p orbital, that's going to be what's highest in energy.
我们来想一想,它“束缚得最松“的电子是哪一个，能量最高的轨道是哪一个？,它就是，2，p，轨道，是能量最高的轨道。
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What we're proposing here is that you take a nice low energy s electron and move it into a higher energy p orbital.
我们这里说的是,你把一个低能s电子,移到高能p轨道里去。
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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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So if that's the case doing a quick little calculation, what would the ionization energy be for a 2 p electron in neon?
么请稍微计算一下，氖原子的，2，p，电子的,电离能是多大？
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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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So, for example, it's not just the 2 p that we could actually take an electron from, we could also think about ejecting an electron from the 2 s orbital.
比如，我们不只可以从，2，p，轨道上,打出一个电子，还能考虑从，2，s，轨道上,发射出一个电子。
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So what we can say is look at each of these separately, so if we start with looking at the 2 p z orbital, the highest probability of finding an electron in the 2 p z orbital, is going to be along this z-axis.
我们可以来分别看看这些图，首先来看看2pz轨道，在2pz轨道里,找到电子的最大概率，是沿着ｚ轴。
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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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So think about what that means, we're, of course, not talking about this in classical terms, so what it means if we have an electron in the 2 p orbital, it's more likely, the probability is that will be closer to the nucleus than it would be if it were in the 2 s orbital.
想想这意味着什么，我们不是从经典的角度考虑，这意味着如果我们有个电子在2p轨道上，它更有可能比在2s轨道上,更加靠近原子核。
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But it doesn't actually cost as much energy as you might think, because in this s orbital here we have a paired electron situation where we're moving up to a p orbital where the electron is no longer paired, so it won't feel quite as much electron repulsion, but nonetheless, this is going to cost us energy.
但它消耗的并没有,你们想象的那么多,因为s轨道里我们电子是配对的,当我们把，电子移到p轨道,电子不再配对，所以它不会感受到那么多的电子排斥，但尽管如此，这个过程还是要消耗能量的。
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So if we write the electron configuration you see that this is the electron configuration here, 1s22s22p 1 s 2, 2 s 2, 2 p 6, 3s1 and now we're going into that third shell 3 s 1.
现在我们来到第三层,你们会看到3s1价电子之间的区别，电子构型是，现在我们来到第三层。
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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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All right, so what we see here is we have our sigma bond that's along the internuclear axis here, but we also have a pi bond, because each of these atoms now has electrons in it's in a p orbital, so we're going to overlap of electron density above and below the bond.
这里我们看到sigma键,是沿着核间轴的，但我们还有一个π键，因为每个原子的p轨道上,都有电子，所以电子密度在键的上面,和下面都有电子密度交叠。
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