sigma2sp It's going to be a sigma bond. So, we have sigma 2 s p, carbon 2 s p. So they're two s p bonds combining.

是sigma键，我们有，碳2sp。，所以它们是两个sp键结合。

麻省理工公开课 - 化学原理课程节选

So it's along the bond axis and it's between a carbon s p 2 hybrid, and then the hydrogen is just a 1 s orbital that we're combining here.

所以它是沿着键轴方向的,而且这里是一个碳sp2杂化轨道，和一个氢的1s轨道的结合,在这里我们可以合并他们。

麻省理工公开课 - 化学原理课程节选

We're going to change the pressure above, Pext right now there's a p external, which is equal to p on the inside.

来改变外界条件，可以改变外界的压强，它将与气体压强p相等。

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So, it turns out that in this case, 2 p and any time that we see we're going from a 2 s to 2 p, filling in of electrons, we actually see that little bit of glitch in ionization energy.

在这种情形下的结果就是，任何时候我们从，2，s，到，填充进电子，我们都会看到电离能会稍稍偏离我们的规律。

麻省理工公开课 - 化学原理课程节选

So now we're putting 2 electrons into the same p orbital, that's not a problem, we can do it, it's not a huge energy cost to do that.

现在我们在同一个，p，轨道上放了两个电子，这没问题，我们可以这样做，这样不会亏损太多能量。

麻省理工公开课 - 化学原理课程节选

So that's true for a hydrogen atom, it doesn't matter if you're in a p or an s orbital, their energies are the same.

这对于氢原子来说是这样的，不论是p或，者s轨道，能量是一样的。

麻省理工公开课 - 化学原理课程节选

All right, so if we think about b h bond here, again, it's the sigma bond, and we're going to say it's a boron 2 s p 2 hybrid orbital interacting with a hydrogen 1 s orbital.

这可以告诉我们，为什么它倾向于周围只有6个电子，好了，考虑一下这里的BH键,同样的，它是sigma键,我们说。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选

And again, this is between the p orbitals, these are not hybrid orbitals, so when we name this bond we're going to name it as a pi bond here, because it's between two p orbitals, and it's going to be between the carbon 2 p y orbital, and the other carbon 2 p y orbital.

同样，这是在p轨道之间的，它们不是杂化轨道，所以当我们命名这个键时,我们要命名它为π键，因为它在两个p轨道之间，而且是在碳2py轨道，和另一个碳2py轨道之间。

麻省理工公开课 - 化学原理课程节选

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。

麻省理工公开课 - 化学原理课程节选