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a0 This is equal to a sub nought for a hydrogen atom, and we remember that that's just our Bohr radius, which is . 5 2 9 angstroms.
它等于,我们记得，这就是波尔半径,也就是0，529埃，实际上。
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When we increase the potential between the 2 electrodes that we have in the tube -- we actually split the h 2 into the individual hydrogen atoms, and not only do that, but also excite the atoms.
当我们增大两个电极之间电压,我们有-我们可以把氢气2,分解成单个的氢原子，不仅这样，还能激发原子。
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That energy will be absorbed by the hydrogen atom, n=1 the electron will rise from n equals one n=2 to n equals two.
这能量将会被氢原子吸收，这个电子会从,上升到。
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If we want to talk about two hydrogen atoms, then we just need to double that, so that's going to be negative 2 6 2 4 kilojoules per mole that we're talking about in terms of a single hydrogen atom.
而要讨论两个氢原子，我们只需要把它乘以二，因此应该是负的，2624，千焦每摩尔,这就是单个的氢原子的情况。
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Well, oxygen, we'll put a hydrogen here, 1 2 3 4 hydrogen here, and one, two, three, four.
如果把一个氢放在这边，另一个氢这边，然后。
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For hydrogen our bond order is going to equal 1/2, 2 minus 0.
对于氢原子键序等于1/2，2减去。
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So it's going to be a sigma bond, 1s and we have oxygen 2 s p 3 and hydrogen 1 s.
它是sigma键，我们有氧2sp3和氢。
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So again, what we're saying here is that it is most likely in the 3 s orbital that we would find the electron 11 and 1/2 times further away from the nucleus than we would in a around state hydrogen atom.
同样我们,这里说的是,氢原子３ｓ轨道中,最可能找到电子的地方,是基态的１１．５倍。
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So, in talking about covalent bonds, we should be able to still apply a more general definition of a chemical bond, which should tell us that the h 2 molecule is going to be lower in energy than if we looked at 2 separate hydrogen atom molecules.
那么，既然提到了共价键，我们应该还可以,给化学键下一个更普遍的定义,那就是告诉我们氢分子能量应该更低,与两个分开的氢的单原子分子相比。
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So, if we talk about dissociating h 2, we're going from the h 2 molecule, and breaking this bond right in half, so we now have two individual hydrogen atoms here.
那么，如果我们讨论的是离解氢分子，我们将从氢分子开始，使这个键断裂，一分为二，那么就得到了两个分开的氢原子。
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So, let's change our graph where we now have this zero point set as the two individuals hydrogen atoms, and then we see that our h 2 molecule is at the negative of the dissociation energy, or the negative what that bond strength is.
那么让我们把曲线图中的零点能改到,两个分离的氢原子处，那我们就会看到,氢分子就是负的离解能，或者负的键的强度。
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So another way to say that is, in a sense, if we're thinking about the excited state of a hydrogen atom, the first excited state, or the n equals 2 state, what we're saying is that it's actually bigger than the ground state, or the 1 s state of a hydrogen atom.
换句话说，如果我们激发一个氢原子，第一激发态或者说ｎ等于２的态，我们说它比氢原子基态,或者说１ｓ态要大。
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so when we think about what it is that this radial probability distribution is telling us, it's telling us that it is most likely that an electron in a 2 s orbital of hydrogen is six times further away from the nucleus than it is in a 1 s orbital.
我们来讨论一下这个径向概率分布,告诉了我们什么，它告诉我们,对于氢原子２ｓ轨道的电子,最可能位置是１ｓ轨道的６倍。
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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。
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And then we're going to name the atomic orbitals that make it up, and it's being made up of a carbon 2 s p 3 orbital, and a hydrogen 1 s orbital.
然后我们要命名,组成它的原子轨道，它是由碳2sp3轨道，和氢原子1s轨道组成。
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And then this second term, if we go to the Periodic Table, 2 we will find that the value here for hydrogen is 2.2 98 and the value for fluorine is 3.98.
再算上第二个条件，翻看元素周期表，我们查处H，F电负性分别为2,2。2，3。
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For example, for the 2 s, again what you see is that the multi-electron atom, its 2 s orbital is lower in energy than it is for the hydrogen.
举例来说对于2s轨道，在多电子原子，中可以看到,它的2s轨道的能量低于氢原子的。
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Again the 2 p orbitals for the multi-electron atom, lower in energy than for the hydrogen atom.
p轨道能量,多电子原子的，低于氢原子的。
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It's a sigma bond, - and it's going to be -- N2sp3 no. OK, it's going to be nitrogen 2 s p 3, because it's a nitrogen atom, 1s and then hydrogen 1 s.
它是sigma键，它是-,不，OK，它是，因为这是个氮原子，然后是氢。
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So, for example, if we look at the 2 s orbital of argon, it's going to have the same amount of nodes and the same type of nodes that the 2 s orbital for hydrogen has.
所以举例来说，如果我们看氩的2s轨道，它有相同数量的节数,和相同类型的节点,对于氢的2s轨道。
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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。
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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。
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So what we'll do is this problem here, which is let's calculate out what the wavelength of radiation n would be emitted from a hydrogen atom if we start at the n equals 3 level and we go down to the n equals 2 level.
我们来做这个问题,让我们来计算一下,从n等于3到,等于2能级氢原子辐射的波长是多少。
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We also have carbon s p 2 hydrogen 1 s bonds.
我们还有碳sp2氢1s键。
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So, for example, 1s1 again we see hydrogen is 1 s 1, helium we say is 1 s 2, or 1 s squared, 1s2 so instead of writing out the 1 s 1 and the 1 s 2, we just combine it 1s22s1 as 1 s squared, lithium is 1 s 2, 2 s 1.
简化符号所以举例来说，我们又看到氢是，氦是1s2或者1s的平方，所以不是将它写为1s1和1,而是我们将它合并为1s的平方,锂是。
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But there's something you'll note here also when I point out the case of the 2 s versus the 2 p, which is what I mentioned that I would be saying again and again, which is when we look at the hydrogen atom, the energy of all of the n equals 2 orbitals are exactly the same.
但是这里有一些事情你们也会注意到,当我指出2s和2p的情况，我之前提过,我会一次又一次的说，我们在观察氢原子的时候，2层轨道的所有n的能量,是完全相同的。
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