And we can look at precisely why that is by looking at the equations for the energy levels for a hydrogen atom versus the multi-electron atom. So, for a hydrogen atom, and actually for any one electron atom at all, this is our energy or our binding energy.

而且我们可以精确地看看,为什么是这样的,通过看对于氢原子和,多电子原子能级的方程所以对于氢原子，事实上对于任何一个电子，这是我们的能量或者我们的结合能。

麻省理工公开课 - 化学原理课程节选

So, let's take a look here at an example of an energy diagram for the hydrogen atom, and we can also look at a energy diagram for a multi-electron atom, and this is just a generic one here, so I haven't actually listed energy numbers, but I want you to see the trend.

所以让我们来看看,一个例子氢原子的能量图，我们也可看看一个,多电子原子的能量图，这是一个普通的图谱，我没有列出能量的数字，但是我想让你们看这个趋势。

麻省理工公开课 - 化学原理课程节选

So what we end up with is one radial node for the 2 s orbital of hydrogen, and we can apply that for argon or any other multi-electron atom here, we also have one radial node for the 2 s orbital of argon.

那意味着它们都是径向节点,所以我们得出的结论是，氢的2s轨道是1个径向节点,我们可以将它应用，到氩或者任意一个多电子原子,对于氩的2s轨道。

麻省理工公开课 - 化学原理课程节选

So, essentially when we're talking about these equations up here, all we're doing is talking about the regular Rydberg formulas, but instead we could go back and re-derive the equation for any one electron atom, which would just mean that we put that z squared term in the front.

所以本质上,当我们讨论，这些问题时，我们说的是常规的，Rydberg公式，但对任何其他单电子原子，我们不用,从头再推到，而是仅仅把，z平方项放在前面。

麻省理工公开课 - 化学原理课程节选