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What is this orbital? Yup. And there's only 2pz one correct answer here, which is to 2 p z.
它的轨道是什么？，嗯，这里,只有一个答案，那就是。
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And if we talk about m equals 0, we're looking at the p z orbital.
如果ｍ等于０，那我们讨论的就是ｐｚ轨道。
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All right. So let's look now at the case where we do have 2 p z orbitals that we're talking about.
好的，让我们现在看一个,需要2pz轨道的例子。
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You might be asking where the 2 p z orbital is and we'll get to that soon once we need it.
你可能会问2pz轨道在哪里,我们等会就会讲到这个问题。
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px And I arbitrarily chose to put it in the 2 p x, 2pz we also could have put it in the 2 p y or the 2 p z, it doesn't matter where you double up, they're all the same energy.
我任意地选择放入至，我们也可以把它放入2py或，它与你在哪双倍填充没有关系，它们都在相同的能级。
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So now let's look at an example where we talk about using these 2 p z orbitals, so let's look at oxygen.
现在让我们来看一个要,用到2pz轨道的例子，让我们来看一下氧。
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So again, what we're talking about is the linear combination of atomic 2 p orbitals, and now we're talking about 2 p z.
同样，我们说的是,原子2p轨道的线性组合，现在我们我们说的是2pz。
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So you should know that 0 any time m is equal to zero that it's the p z.
所以当我们讨论p轨道时,只要m等于,它就是pz轨道。
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We can fill right up our table just like we did before, but now we have included our 2 p z orbital here.
我们可以像以前一样填充表格，但现在我们包括了2pz轨道。
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Now we're going to start in with that pi 2 p orbitals, which gives us 1 each, and then two each in those, we'll go up to our sigma 2 p z orbital.
现在我们要填π2p轨道，每个1个，然后每个2个，我们我们填sigma2pz轨道。
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And now we get the p orbitals, remember we want to fill up 1 orbital at a time before we double up, so we'll put one in the 2 p x, then one in the 2 p z, and then one in the 2 p y.
我们到了p轨道，记住在双倍填充之前,我们想要每次填充至一个轨道，所以我们在2px填充一个然后2pz填充一个，然后2py填充一个。
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So, we can have the 2 p x, 2 p y, and 2 p z orbitals.
所以我们有2个px2个py2个pz轨道。
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If m is equal to 0, in this case we would call it the p z orbital, z so we would have the subscript z here.
如果m等于0，这种情况下,我们叫它pz轨道，我们在这里有下标。
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This is, in fact, a sigma 2 p z orbital is what this orbital is called.
这是这个轨道是因为,一个sigma2pz轨道。
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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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So this is still a sigma it's a sigma 2 p z star orbital.
这还是一个sigma轨道,它是sigma2pz星轨道。
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So it's OK to not specify. I want to point out, pz whether you're in the p x, the p y, or the p z, unless a question specifically m asks you to specify the m sub l, which occasionally will happen, but if it doesn't happen you just write it like this.
我想指出的是，无论你在px，py或，除非一个问题特别地,让你指出l下面的，这种情况有时会发生，这样就可以了,但是如果它不做要求你们写成。
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All right, so one thing that I want to point out, which I said many, many times on Friday, and this is perhaps the last time I'll say it, but one last time is we can think about why we only see a line for the 2 p orbital, versus we don't see separate lines for a 2 p x, a 2 p y, and a 2 p z.
好的，我还要指出一个问题，这个问题我在上周五已经说了很多很多次了，这可能是我最后一次提到它，但是这最后一次让我们来考虑一下,为什么我们只看到了一条，对应于，2，p，轨道的线,而不是分别对应于，2，p，x，2，p，y，2，p，z，的线？
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So essentially, each of these orbitals come from linear combinations of all of the original orbitals, and it's hard to picture exactly how that happens, but one that you can at least start to get an idea is if you think about combining the 2 s and the 2 p z here, which is not quite accurate because of course, we're combining all of them.
本质上，这些轨道每个都来,自原来所有轨道的线性组合，我们很难想象这是怎么发生的，但你们可以至少有个概念,如果你们考虑2s和2pz轨道的结合，这当然是不太准确的，因为我们要把所有的都组合起来。
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Specifically, it's always the z that forms the sigma orbital, and the reason is at least at a minimum for this class we always define the internuclear axis as the z axis, so this is always the z axis, so it's always going to be the 2 p z's that are coming together head-on.
特别的，z总是形成sigma轨道，这是因为至少在这个课里面,我们总是定义核间轴为z轴，所以这总是z轴，所以2pz轨道总是,朝一个方向出现。
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And in terms of thinking about the phase of this p orbital, the phase is going to be positive anywhere where z is positive.
对于ｐ轨道的相位，在ｚ大于零的地方都是正的。
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So z equals 7 -- this is the cut-off where, in fact, the sigma orbital is going to be higher in energy than the pi 2 p orbitals.
所以z等于7-这是分界点，实际上，sigma轨道能量,要比π2p轨道高。
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That's it. Again, these other p dxy dyz - or the d x y, d y z, those are going to be those more complicated linear combinations, you don't need to worry about them.
同样，这些p轨道,或者，它们是一些,很复杂的线性组合，你们，不用管它。
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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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And what we're actually talking about again is the zeffective. So that z effective felt by the 2 p is going to be less than the z effective felt by the 2 s.
我们实际上所谈论的,所以被2p感觉到的,的有效电荷量,有效电荷量小于2s感觉到。
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So, if we think about this z bonding axis between the two carbon atoms, we can picture overlap of those s p hybrid orbitals, and then we can also picture bonding to hydrogen.
如果我们考虑,两个碳原子之间的z成键轴，我们可以画出sp杂化轨道的交叠，我们也可以画出和氢原子的成键。
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And it turns out that if we have a, for example, for s, a very large z effective or larger z effective than for 2 p, and we plug in a large value here in the numerator, that means we're going to end up with a very large negative number.
结果是如果我们有一个，举例来说对于s一个很大的有效电荷量或者,比2p大的有效电荷量，并且我们将一个较大的值代入计算器，那意味着我们最后会得到,一个非常大的负数。
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