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And specifically, when we talk about ionization energy, it's assumed that what we mean is actually the first ionization energy.
特别地，当我们讨论电离能的时候，我们默认,这指的是第一电离能。
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Well, if we look on the chart, the first ionization energy is what is reported in your Periodic Table.
如果我们查阅图表，一级电离能,已经在元素周期表上标示了。
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So I've sort of just spread out what we have as the second row here, graphed against the ionization energy.
所以我将第二行的情况,在这里展了，纵坐标是电离能。
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Yup. So it's just that ionization energy 94×10-18J that we have experimentally measured, 3 . 9 4 times 10 to the negative 18 joules.
它就是我们通过实验测得的,电离能3。,我们用所有的这些。
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Our ionization energy is going to be equal to the incident energy coming in, minus the kinetic energy of the electron.
我们的电离能将等于,入射能量，减去电子的动能。
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In this case, it's called the ionization energy, plus whatever kinetic energy we have left over in the electron.
在这种情况下，它就是电离能，剩余部分将转化为,出射电子的动能。
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One major difference between electron affinity and ionization energy is that when we talked about ionization energy, remember ionization energy always has to be positive.
电子亲和能,与电离能之间最大的不同就在于,当我们提到电离能的时候，记得电离能总是正的。
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As we go across the row what happens is that the ionization energy actually increases, and we can think about logically why it is that that's happening.
当我们沿着行,向右走的时候，可以发现电离能是逐渐升高的,我们可以从逻辑上思考一下为什么会这样。
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This is the second ionization energy. That is to say the ionization energy of the second most electron.
这是二级电离能，这就是说,电子数第二多的电离能。
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We call these first, second, third ionization energies in sequence. This is the first ionization energy.
我们按照顺序把这些叫做一级，二级,三级电离能，这是初级电离能。
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If something has a high ionization energy, it means that it really, really, really does not want to give up an electron.
如果某个东西有很高的电离能，这意味着它非常非常，非常不愿意失去一个电子。
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So, in a first blush, you might say, well, why don't we just take the first ionization energy?
当你在这个问题上第一次陷入尴尬境地的时候，你可能会说，我们为什么不取第一个电离能呢？
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And let's look at the final kinetic energy that we'd observe in this spectrum, which is 384 electron volts, so what is that third corresponding ionization energy?
然后让我们来看一下,在光谱中观测到的，最后一种动能，它大小是，384，电子伏，那么这相应的第三种电离能是多大？
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And if we experimentally know z what the ionization energy is, we actually have a way to find out what the z effective will be equal to.
我们实际上就有了一个办法,去找出有效的，等于多少,我们可以使用这里的方程。
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We'll then take a turn to talking about the periodic table, we'll look at a bunch of periodic trends, including ionization energy, electron affinity, electronegativity and atomic radius.
然后我们再开始讲元素周期表，我们会看到很多周期性规律，比如电离能，电子亲和能，电负性以及原子半径。
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We talked about ionization energy, electron affinity, we talked about electronegativity, which is just kind of a combination of the first two, and then ended with atomic radius here.
我们讲了电离能的，电子亲和能的，还讲了电负性的，也就是前两个的组合，最后讲了原子半径的。
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And remember again, the binding energy physically is the negative of the ionization energy, and that's actually how you can experimentally check to see if this is actually correct.
电离能的负值，那个事实上是可以,通过实验来验证，它是否是对的,并且它等于负的。
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We know that ionization energy is going to increase as we go across the periodic table, so that means carbon has a lower ionization energy than nitrogen which is right next to us.
我们知道电离能会随着周期表,向右而逐渐变大，因此碳的电离能比旁边的氮要低一些,那么就像我说的。
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But, in fact, we can also talk about the ionization energy of different states of the hydrogen atom or of any atom.
但实际上我们也可以讨论氢原子,或者其它任何原子的其它能级的电离能。
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So it's going to keep in mind the limitations, so let's start off with talking about ionization energy.
那么让我们将这些局限性记在心里，继续来讨论一下电离能。
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So, second ionization energy simply means you've already taken one electron out, now how much energy does it take for you to take a second electron out.
第二电离能简单地说就是,在你已经拿走一个电子以后，再拿走第二个电子,所需要消耗的能量。
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And we know what that's equal to, this is something we've been over and over, ionization energy is simply equal to the negative of the binding energy.
而且你知道它等于什么，这是我们说过一遍又一遍的，电离能就等于,负的束缚能。
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So we can use an equation to relate the incident energy and the kinetic energy to the ionization energy, or the energy that's required to eject an electron.
因此我们可以用一个公式将入射能量,与动能和电离能，就是发射出一个电子所需要的能量关联起来。
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What we've learned so far is as a first approximation, what we want to do is put the atom with the lowest ionization energy in the middle here.
我们之前所学的可以作为第一近似，我们要做的是把电离能,最低的原子放在中间。
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So, this one can be tricky because oxygen looks like it's in the middle because of the way it's written, but we need to start by looking at the lowest ionization energy.
这个例子可能有些狡猾,因为氧看起来是在中间的,因为它是这样写的，但是我们需要从寻找最低的电离能开始。
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So here we have that graphed here, Z we have atomic number z graphed against ionization energy, so, let's fill in what the actual atoms are here, and we can see in general, yes, we're following the trend.
这就是我们要画的，横坐标是原子序数，纵坐标是电离能，让我们把真正的原子填上去，我们可以看出，总体来说，没错，满足规律。
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If you flip the Periodic Table over you will have the ionization energy of sodium, first ionization energy, 5eV and it is about 5 eV which, when you convert, 496kJ/mol is a whopping 496 kilojoules per mole.
如果浏览周期表,你可以得到钠的离子化能，第一电离能，大约，当你转换的时候，是巨大的。
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We would expect the ionization energy to decrease, that means that sulfur has our lowest ionization energy.
我们预期电离能会降低，这就意味着硫的电离能最低。
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The first ionization energy of lithium is about 5.4 electron volts per atom.
锂的一级电离能,大约是每原子5。4电子伏。
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So, what we can do instead of talking about the ionization energy, z because that's one of our known quantities, so that we can find z effective.
我们做的事可以代替讨论电离能,因为那是我们知道的量子数之一，那是我们可以解出有效的，如果我们重新排列这个方程。
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