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So, in order to fill our octet, what we do is put two on the nitrogen and two on the carbon.
因此，为了填满我们的“八隅体“,我们需要将两个放到氮上，将另外两个放到碳上。
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So, electron promotion does not happen in terms of nitrogen, because it would not increased our number of unpaired electrons.
这里对于氮原子不会有电子激发，因为这不会增加,未配对电子的数目。
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We know nitrogen bonds multiple bonds, so let's look at nitrogen.
我们了解氮气中有多重键，我们看看氮气。
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So what we can actually directly compare is the dissociation energy or the bond strength of nitrogen versus hydrogen.
因此实际上我们可以直接进行比较,对氮分子与氢分子的离解能,或键的强度。
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So in terms of nitrogen that starts off with a valence number of 5, again we have 2 lone pair electrons in the nitrogen, and again, we have 6 electrons that are shared.
对于氮来说,我们应该从五个价电子开始，同样，氮也有两个孤对电子，共用电子的个数也一样，是六个。
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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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So if we take a look at nitrogen here, what you'll notice is we have thre available for bonding, - and we already have our lone pair -- one of our orbitals is already filled up.
如果我们看一下氮原子，我们注意到我们可以成3个键，我们已经有一个孤对-,其中的一个轨道已经被填满了。
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So, in this case, we see that our formal charge is negative on the nitrogen, in this case it's negative on oxygen.
那么，在这种情况下，我们看到氮的形式电荷是负的，而在这种情况下，氧的是负的。
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So that explains one of our glitches here, but we have another glitch, and that second glitch comes between nitrogen and oxygen.
那么我们的第一种小偏差已经解释清楚了，但是我们还有另外一种，它在氮和氧之间发生。
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So this means nitrogen has low electron affinity, it doesn't actually want to gain an electron.
这意味着氮的电子亲和能很低，它实际上并不愿意得到一个电子。
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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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So, if we talked about a nitrogen-nitrogen single versus double versus triple bond, the triple bond will be the shortest and it will be the strongest.
因此，如果我们讨论的是氮与氮之间的单键,双键与三键，那么三键应该是其中最短的一个，同时也是最强的一个。
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We see that the radius is shorter, so that means that the nitrogen-nitrogen bond is going to be shorter.
我们看到这个距离更短，这就意味着,氮与氮之间的键应该更短。
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So, shared electrons are the ones that are shared between the carbon and the nitrogen, so we have 6 shared electrons, and we want to take 1/2 of that.
共用电子是那些在碳和氮之间,被它们共用的电子，那么我们有六个共用电子，然后我们要给它乘上二分之一。
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So we can put actually all 4 of our extra electrons in between the carbon and the nitrogen.
因此我们可以把这剩下的,四个电子都放在碳和氮之间。
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So in our first structure, we would find for the nitrogen we have a formal charge 5 minus 4 minus 2, because we're starting with 5 valence electrons, so that is a formal charge of minus 1.
那么在我们的第一个结构中，我们发现氮的形式电荷量是五减去四4,再减去二，因为我们开始有五个价电子，因此它的形式电荷量是负一。
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So that takes care of the hydrogen, what about between the carbon and the nitrogen?
因此氢就被排除了，那么碳和氮呢？
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So, nitrogen is shown here, we know that because it has 7 electrons.
那么这里显示的是氮，我们能看出来是因为它有七个电子。
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So what we see is that the formal charge on the nitrogen is 0.
因此我们看到氮的形式电荷是零。
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So, let's, for example, look at nitrogen. So n 2, we can do the chart here in green, so it's the green dotted line, and what we see is that we have now defined this energy as where the 2 nitrogen atoms are separated.
那么，让我们举个例子，看一下氮，那么氮分子，我们可以把它用绿色曲线画在这，这是绿色的虚线，可以看到,我们已经定义为零点能，当两个氮原子分离时。
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But for anything 7 or less, so what is the atomic number for nitrogen?
但对于7或者更少，对于N原子序数是多少？
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So if we're comparing the difference between these 2 now, what you'll notice is that in nitrogen we have all half-filled 2 p orbitals, and now, once we move into oxygen, we actually have to add 1 more electron into 1 of the 2 p orbitals.
那么如果我们来比较下它们两个有什么不同，你会发现氮的，2，p，轨道,都是半满的，现在，我们继续看一下氧，我们不得不在其中一个，2，p，轨道上,再放上一个电子。
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