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And an electron is something where, i n fact, we might be able to, if we calculate it and see how that works out, actually observe some of its wave-like properties.
如果我们对电子做计算,并且知道如何算出来的,那么我们是可以观测到,电子的一些波动性质的。
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So, if we took the case of nitrogen, if we add an electron to nitrogen and go to n minus, we find that the change in energy is 7 kilojoules per mole.
如果我们以氮为例，如果我们给氮增加个电子令它变成-1价的氮，我们会发现能量的变化是，7，千焦每摩尔。
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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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So this is our final equation, and this is actually called the Balmer series, which was named after Balmer, and this tells us the frequency of any of the lights where we start with an electron in some higher energy level and we drop down to an n final that's equal to 2.
把2代入到这里，所以得到1除以,这就是我们最终的方程，这叫做Balmer系，以Balmer名字命名的,它告诉我们从高能级掉到n等于2的,最终能级所发出光的频率。
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So, for example, we could talk about the n equals 2 state, so that's this state here, and it's also what we could call the first excited state. So we have the ground state, and if we excite an electron into the next closest state, we're at the first excited state, or the n equals 2 state.
例如，我们可以考虑n等于2的状态，它在这里，它也被称作是第一激发态,我们有基态，如果我们把一个电子,激发到它最近邻的态,那就是第一激发态，或者n等于2的态。
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So we have 4 plus 5, but we're actually not done yet, because it's c n minus, so if we have minus, we actually have an extra electron in our molecule.
我们有四个加上五个，但是我们实际上还没做完，因为这是个负离子，所以如果我们有这个负号，那么我们的分子实际上还有一个额外的电子。
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And we know that n describes the total energy, that total binding energy of the electron, so the total energy is going to be equal to potential energy plus kinetic energy.
我们知道，n是描述总能量的，电子总的结合能，所以总能量，等于,势能加动能。
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We knew from Friday, when we talked about energy, that ground state was that n equals 1 value, that was the lowest energy, that was the most stable place for the electron.
我们上周五知道了，在讨论能量的时候，基态指，n等于1的态，它能量最低，是，最稳定的态。
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They're not going to want to add on another electron, because then it'll have to jump a very large energy level go from n equals 2, to n equals 3, and n equals 4, and so on.
它们不愿意增加另外一个电子，因为这会让它们跳到一个非常高的能级上去,依次是，n，等于，2，3，4，等等。
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And if that is the energy to go from n equals one n=2 this is the amount of energy that has to be left as kinetic energy of the electron.
如果这个能量是从n=1到,然后，to，n，equals，two，then,这些能量,会作为电子的动能,被消耗掉。
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And, in fact, it can't even reach n, because then we would have no potential energy at all in our electron, which is not correct.
事实上，它连n都达不到，因为如果那样的话,电子就没有势能了，这是不可能的。
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So there are two electron configurations in the n equals one shell, if we follow according to the selection rules that we spelled out last day.
如果根据上次课,我们阐明的原子光谱选择定则，我们就会知道在n等于1的那一层,有两种电子图像构型。
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This should make sense to you, because they don't, in fact, want to gain another electron, because that would mean that electron would have to go into a new value of n, a new shell, and that's really going to increase the energy of the system.
这对大家来说应该容易理解，因为它们实际上不想得到另一个电子，因为这意味着这个电子不得不,到一个新的，n，值更大的壳层上去，这将会增加系统的能量。
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We know that the orbitals for multi-electron atoms depend both on n and on l.
我们知道对于多电子原子轨道,是依赖于n和l的。
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n So the velocity is given by this product of the quantum number n Planck constant 2 pi mass of the electron time the radius of the orbit, which itself is a function of n.
速度是量子数,普朗克常数2π乘以轨道半径的值,它自身也是n的函数。
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We're going to get to more complicated atoms eventually where we're going to have more than one electron in it, but when we're talking about a single electron atom, we know that the binding energy is equal to the negative of the Rydberg constant over n squared, so it's only depends on n.
我们以后会讲到，更加复杂的情况,那时候,不只有一个原子，但当我们讲，单个原子的时候，我们知道结合能，等于,负的Rydberg常数,除以n平方，所以它仅仅由n决定的。
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So, if, for example, we were looking at a hydrogen atom in the case where we have the n equals 1 state, so the electron is in that ground state, the ionization energy, it makes sense, is going to be the difference between the ground state and the energy it takes to be a free electron.
电离氢原子所需要的能量,如果我们看n等于1的情况,电子在基态，那电离能，很合理的就是基态,和自由电子态的能量差。
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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。
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