So, if we think of just an example, 2 we could say that 4 l equals 2, what would be our lowest value of m sub l?

举个例子，如果我们说l等于，那m小标l，最小值是多少？

麻省理工公开课 - 化学原理课程节选

So, our next level up that we can go is going to be the n equals 2 energy level, but we also have an l and an m value, 0 so our lowest l is going to be a there.

所以下一个能量,是n等于2的能级，但我们还有l和m的值，所以我们最低的l等于。

麻省理工公开课 - 化学原理课程节选

So finally, if we talk about our last example of when n is going to be equal 2, l -1 and then minus 1 for m.

最后我们要讲的,这个例子，是n等于2时，等于1，we，can，have，2，，1，for，l,而m等于。

麻省理工公开课 - 化学原理课程节选

So, we can put our sulfur in the middle, and then it doesn't really matter how we draw the rest of it, where we put our c l's versus where we put our oxygen.

那么，我们可以把硫放在中间，然后把其它的原子画在哪里就不重要了，把两个氯原子与一个氧原子放在哪里都行。

麻省理工公开课 - 化学原理课程节选

We didn't just need that n, not just the principle quantum number that we needed to discuss the energy, but we also need to talk about l and m, as we did in our clicker question up here.

我们不仅需要ｎ,不仅要这个可以,决定能量的主量子数，还需要ｍ和ｌ,就像我们做这道题这样。

麻省理工公开课 - 化学原理课程节选

And the last example that we're going to talk about is thionyl chloride, so it's s o c l 2. This is another good step forward, because now we actually have four different atoms in our molecule.

我们要讨论的最后一个例子,是氯化亚砜，就是硫，氧，氯，二，这又是一个进步，因为我们的分子中现在有四个不同的原子了。

麻省理工公开课 - 化学原理课程节选

And the first is l, and l is angular momentum quantum number, and it's called that because it dictates the angular momentum that our electron has in our atom.

第一个就是l，l是,角动量量子数，叫它这个名字,是因为它表明，原子中,电子的角动量是多少。

麻省理工公开课 - 化学原理课程节选

So if we say that l is just talking about our kinetic energy part, our rotational kinetic energy, and we know that electrons have potential energy, then it makes sense that l, in fact, can never go higher than n.

如果我们说，l仅仅是,描述动能项，我们的旋转动能，我们知道，电子有势能，所以可以理解，l不能比n高。

麻省理工公开课 - 化学原理课程节选

l So, if we're talking about a 4 p orbital, and our equation is n minus 1 minus l, the principle quantum number is 1 4, 1 is 1 -- what is l for a p orbital?

我们方程是n减去1减去，主量子数是，4，1是1，--p轨道的l是多少？,学生：

麻省理工公开课 - 化学原理课程节选

I think most and you are familiar with the Aufbau or the building up principle, you probably have seen it quite a bit in high school, and this is the idea that we're filling up our energy states, again, which depend on both n and l, one electron at a time starting with that lowest energy and then working our way up into higher and higher orbitals.

我认为你们大多数熟悉奥弗堡,或者构建原理，你们可能,在高中见过它，又一次,这是我们填充能级的观点，与n和l有关，一个电子每次从,最低的能级开始,然后以我们的方式上升到,更高更高的轨道。

麻省理工公开课 - 化学原理课程节选