So you see in the hybrid orbital we actually have a larger lobe on top where they constructively interfered.

所以你们可以看到在杂化轨道里,我们上面,由很大的一叶相长干涉。

麻省理工公开课 - 化学原理课程节选

So that leaves each carbon with only one hybrid orbital left.

这样每个碳原子只剩下一个杂化轨道。

麻省理工公开课 - 化学原理课程节选

So if you picture this as our s p 2 carbon atom where we have three hybrid orbitals, and then one p y orbital coming right out at us.

如果你把这想象成sp2碳原子,这里有3个杂化轨道，然后一个py轨道朝向我们。

麻省理工公开课 - 化学原理课程节选

And if we think about the six hydrogens, now each of those are going to bind by combining one of the carbon hybrid orbitals to a 1 s orbital of hydrogen.

如果我们考虑有六个氢原子，每个都会合起来,碳杂化轨道成键,每个氢的1s轨道。

麻省理工公开课 - 化学原理课程节选

So this is a little bit trickier to look at and see what it means, but essentially we have two hybrid orbitals, which are shown in blue here, and then we have one p orbital that's left alone that's going up and down on the page.

看这个图肯能会觉得比较诡异，但本质上，骂我们有两个杂化轨道，这里用蓝色表示，还有剩下一个p轨道,在图中上下方向上。

麻省理工公开课 - 化学原理课程节选

And hybrid orbitals are all going to be completely equal, and lower in energy than the p orbital.

杂化轨道是完全相等的，你会注意到它们的能量比s轨道高，比p轨道低。

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

The reason that it's a sigma bond is sp3 because the s p 3 hybrid orbital is directly interacting with the 1 s orbital of the hydrogen atom, and that's going to happen on the internuclear axis, they're just coming together.

它是sigma键的原因,是因为,杂化轨道直接和氢原子1s轨道相互作用，它们作用发生在核间轴上，它们会到一起。

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

So we end up with 1 p orbital completely untouched, and three hybrid s p 2 orbitals.

没有变化，所以我们得到的是1个完全没有变化p轨道。

麻省理工公开课 - 化学原理课程节选