When we talk about orbitals in multi-electron atoms, they're actually lower in energy than the corresponding H atom orbitals.
当我们讨论多电子原子的轨道时，它们的能量实际上比对应的氢原子轨道要低。
Doing those probability density dot graphs, we can get an idea of the shape of those orbitals, and we know that they're spherically symmetrical.
通过那些概率密度图，我们可以知道轨道的形状，我们知道它们是球形对称的。
这是原子轨道。
让我们占据这些轨道。
What will we call that in terms of orbitals?
我们从轨道的角度，怎么命名它？
What is the filling sequence of electrons in orbitals?
什么是电子在轨道上的排布顺序呢？
And then we are going to construct molecular orbitals.
接着我们就建立分子轨道。
Electrons fill orbitals from lowest energy to highest energy.
电子从最低能级到最高能级，填满轨道。
Linear combination of atomic orbitals into molecular orbitals.
原子轨道的线性叠加，成分子轨道。
When we're talking about orbitals, we're talking about wave functions.
当我们说轨道的时候，我们说的是波函数。
So we'll see specifically why it is that the s orbitals are lower in energy.
所以我们会特别地看到，为什么s轨道的能量是较低的。
We did it for the s orbitals, we can also do it for the p, we can do it for the d.
我们对s轨道这样做了，我们也可以对p轨道这样做，对d轨道这样做。
So we can add three hydrogen atoms here, and fill in our other orbitals right here.
我们可以加三个氢原子到这里，填满其它的轨道。
Well, essentially what that tells is that these s orbitals are spherically symmetrical.
实际上它告诉我们，这些s轨道，是球对称的。
We'd started on Monday talking about radial probability distributions for the s orbitals.
我们从星期一开始讨论了，s轨道的径向概率分布。
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。
So in molecular orbital theory, what we did was we named orbitals based on their symmetry.
在分子轨道理论中，我们基于轨道的对称性给它们命名。
All right, so let's consider our methane situation now that we have our hybrid orbitals.
好，让我们考虑甲烷的情形，既然我们有了杂化轨道。
So, this means we have a total of six electrons that we need to put into molecular orbitals.
这意味着我们一共有，6个电子要放进分子轨道。
But when we think about where anti-bonding orbitals should be, it should be higher in energy.
但当我们讨论反键轨道的时候，它的能量应该更高。
And again, we have the pairing of the unpaired electrons, and we have two orbitals coming together.
同样，我们有未配对电子的配对，我们有两个轨道结合。
So we can think about now doing bonding, and now we have four equal orbitals with one electronic each.
我们现在可以考虑成键了，现在我们有4个等价的轨道，每个上面有1个电子。
And to do this we're going to introduce valence bond theory, and the idea of hybridization of orbitals.
在这之前我们要引入价电子成键理论，和杂化轨道的概念。
So now we're just counting up our orbitals, an orbital is completely described by the 3 quantum Numbers.
所以现在我们只要把这些轨道加起来，一个轨道是由3个量子数完全确定的。
If I now hybridize these, if I take these and I make four symmetric, now, these are just the sp3 orbitals.
如果我将他们杂化，然后形成4个对称的轨道，这就是sp3轨道。
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。
Any time two orbitals come straight on together in that internuclear axis, you're going to have a sigma bond.
任何时候两个轨道，在核间轴上直接到一起，你就能得到sigma键。
And a sigma bond forms any time you have two orbitals coming together and interacting on that internuclear axis.
当你把两个轨道合在一起，并在核间轴上有相互作用时，就形成了sigma键。
First of all, this is the two s orbitals in hydrogen, 1s plus 1s smearing to give us this sigma molecular orbital.
首先，这是氢气中的两个s轨道，1s与1s轨道重叠，产生sigma分子轨道。
So again, we can fill in our atomic orbitals here, there's going to be two electrons in each of our atomic orbitals.
同样的，我们可以填充原子轨道，每个原子轨道上有两个电子。
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