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So here's the pneumonic I mentioned for writing the electron configuration and getting those orbital energies in the right order.
这里是我提到的,对于写电子构型,和以正确的顺序得到轨道能量。
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And what you find is when you have a bonding orbital, the energy decreases compared to the atomic orbitals.
你们发现当你有个成键轨道的时候，相比原子轨道能量要降低。
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The radius of the orbit, the energy of the system and the velocity of the electron, I am just going to present you the solutions.
是轨道的半径，系统的能量,以及电子的速度，我接下来会给你们讲解其方程的解法。
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So, I think we have these molecular orbital energies down, so let's move on to talking about more complex molecules.
分子轨道能量就说到这里，让我们继续来讨论一下更复杂的分子。
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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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For example, with neon we can think about all of the different orbital energies we could be looking at.
比如氖，我们可以想象一下,它的所有不同轨道的能量。
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And the other thing to point out is that the energy that an anti-bonding orbital is raised by, is the same amount as a bonding orbital is lowered by.
另外一个要指出的事情是,反键轨道引起的能量升高，和成键轨道引起的能量降低是相同的。
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You can see that as you fill up your periodic table, it's very clear. But also we'll tell you a pneumonic device to keep that in mind, so you always remember and get the orbital energy straight.
在你们填周期表的时候，非常清楚但是我们也要告诉你们,一个策略去记住它，所以你们总是记得,并得到连续的轨道能量。
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And again, you'll notice that our energy is absolutely the same for an electron in that 2px and 2s orbital.
同样，你们会发现2px轨道的能量,和2s轨道是一样的。
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So it's going to be favorable for the electrons instead to go to that lower energy state and be within the molecular orbital.
所以对于电子来说,更倾向于能量更低的轨道,呆在分子轨道里。
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What we've seen is we have a net lowering of energy of the molecule versus the individual atoms.
分子轨道对于单个原子轨道来说,我们可以看到的是一个净的能量降低。
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So in the case of 12 32, that is our highest kinetic energy, it's the smallest amount of energy it takes to pop an electron out of that orbital.
因此，1232是我们能够得到的,最高的动能，它是从这个轨道中,打出一个电子需要消耗的最低能量。
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Orbitals of equivalent energy, we strive for unpaired electrons.
相同能量轨道，我们找到不成对电子。
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Electrons will occupy orbitals in order of ascending energy, occupying the lowest energy first and up.
电子是按其能量递增顺序,排布在轨道上的，首先占满第一级，即最低能级。
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So any time I draw these molecular orbitals, I do my best, and I'm not always perfect, yet trying to make this energy different exactly the same for the anti-bonding orbital being raised, versus the bonding orbital being lowered.
所以我在画这些分子轨道的时候，虽然不是很完美，但我总是尽量,让反键轨道引起的，能量升高和成键轨道。
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The best suggestion is just to write it out completely for the neutral atom, and then you want to take an electron out of the highest orbital.
最好的办法是先写出它所对应,中性原子，然后再从,能量最高的轨道上拿走一个电子。
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But when we think about where anti-bonding orbitals should be, it should be higher in energy.
但当我们讨论反键轨道的时候，它的能量应该更高。
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What we do care about is the energy of our orbitals that have electrons in them, and if we combined all four of the orbitals, then our hybrid orbitals would have more p character to them, so they'd actually be higher in energy.
是不是很高,我们不关心它的能量很高，我们关心的是，有电子的轨道的能量，如果我们把四个轨道结合。
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And that's going to be lower in energy than the two individual atomic orbitals.
它的能量要比,两个独立的原子轨道能量要低。
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All four of these orbitals have the same energy, t hey're degenerate.
这四个轨道,能量相同,是简并的。
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You see the same thing regardless of which orbital you're looking at.
能量是低于氢原子的,无论你观察哪个轨道都可以看到相同的事情。
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That's what we call degenerate orbitals, they're the same energy.
我们称之为简并轨道，它们具有相同的能量。
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Degeneracy is where you have orbitals of equivalent energy.
简并发生在轨道能量相同的地方。
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So that lowered the energy of the molecular orbital.
所以降低了分子轨道的能量。
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We can also figure out the energy of this orbital here, and the energy is equal to the Rydberg constant.
我们同样可以知道,这个轨道的能量，它等于，Rydberg常数。
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When we talk about the n equals 2 state, we now have 2 squared or 4 degenerate same energy orbitals, and those are the 2 s orbital.
当考虑n等于2的态时，我们有2的平方,或者4个简并能量的轨道，它们是2s轨道。
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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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But actually there is a little bit of an energy cost into doubling up into a single orbital, because, of course, it takes energy when you create more electron repulsion, that's not something we want to do, but we have to do it here, and it turns out that that effect predominates over, again, the energy that we gain by increasing the atomic number by one.
但实际上，在一个轨道上放两个电子,确实会亏损一点能量，因为，当你加入更多电子，引起更大的排斥能,这显然会消耗能量，这不是我们想要做的，但是在这种情况下我们不得不做，结果这一影响，超过了增加一个,原子序数所得到的能量。
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So what we know is that these 3 d orbitals are higher in energy than 4 s orbitals, so I've written the energy of the orbital here for potassium and for calcium.
我们所知道的是,3d轨道能量,比4s轨道能量高，所以我写出了,钾和钙的轨道能量。
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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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