It turns out that the antibonding orbital is a little bit higher from the atomic orbital level than the bonding orbital is lower.

这证明了,反键轨道,比原子轨道高,成键轨道比原子轨道第。

麻省理工公开课 - 固态化学导论课程节选

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。

麻省理工公开课 - 化学原理课程节选

Now, from your book as well, this is the pz's of the two atomic orbitals forming the bonding orbital.

现在，也是你们书上，这是两个pz轨道,组成的成键轨道。

麻省理工公开课 - 固态化学导论课程节选

So, let's think of the energy of interaction when we're comparing atomic orbitals to molecular bonding orbitals.

当我们比较原子轨道和分子轨道的时候,我们来考虑一下相互作用能。

麻省理工公开课 - 化学原理课程节选

The thesis of 3.091, and this is where the chemistry comes in, is that electronic structure of the elements holds the key to the understanding, not just the chemical bonding, but the long range atomic order.

这是这门课的论点，这是化学的研究点，也就是元素的电子结构,那即是理解的关键，不只是化学键，还有长程的原子排序。

麻省理工公开课 - 固态化学导论课程节选

So, up here, atomic theory, periodic table, bonding, structures and molecules.

原子理论，元素周期表，价键，分子结构。

麻省理工公开课 - 化学原理课程节选

So we would label our anti-bonding orbital higher in energy than our 1 s atomic orbitals.

我们应该把反键轨道标在,高于1s原子轨道能量的地方。

麻省理工公开课 - 化学原理课程节选

So we have two electrons in our bonding orbital, but because we use the same rules to fill up molecular orbitals as we do atomic orbitals, so the Pauli exclusion principle tells us we can't have more than two electrons per orbital, so we have to go up to our anti-bonding orbital here.

所以在成键轨道上有两个电子，但因为我们用了和原子轨道时,用的相同的规则，所以Pauli不相容原理告诉我们,一个轨道上不能有两个以上的电子，所以我们需要填充到反键轨道上去。

麻省理工公开课 - 化学原理课程节选