If these bonds were all completely of equal distance apart, whether is was a lone pair or bonding electrons, 5° the angles would be 109 . 5 degrees.
如果不管它是孤对,还是成键,它们等距分开的话,键角是109。
Yeah, so also 4. We started with 10 valence electrons, we used up 6 of those as bonding electrons, so we have 4 left, which will be lone pair electrons.
对,也是四个,我们从十个价电子开始,只用了六个来成键,因此我们还剩下四个,它们将成为孤对电子。
That's because you have to satisfy this base pair matching in order to have hydrogen bonding in each of the struts of the ladder in order to form a stable structure.
NA双链要满足互补配对原则,以使碱基对之间,形成氢键,从而形成稳定的双链结构
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。
For the sulfur, we start off with 6 valence electrons, minus 4 lone pair electrons, minus 2, taking in account our bonding electrons, so we end up with a formal charge of 0.
对于硫,我们从六个价电子开始,减去四个孤对电子,再减去二,算上我们的成键电子,因此最终我们有零个形式电荷。
That's what we call when we have three bonding atoms and one lone pair.
这是当我们有3个成键电子,和一个孤对时这样称它。
So what we see is on ammonia here, 107 we know that it's less than a 109 . 5, it's actually 107, so it's less than a 109 . 5, because of that lone pair pushing down in the bonding electrons.
我们看到在氨分子里,我们知道它比109.5要小,它是,所以比109。5要小,因为孤对会把成键电子向下推。
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