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OK, a couple of good questions
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Posted by Erik919kt (more from Erik919kt) on Fri, 18 Jul 2008 20:07:18 Share Post by Email
In Reply to: Did not try myself, but have read plenty on it., dim33, Thu, 17 Jul 2008 05:52:59
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Why is an oxygen atom smaller than a nitrogen atom? If you google "atomic radius", you will find tables that demonstrate that, as you move across the first row from carbon to nitrogen to oxygen to fluorine, the atomic radius, in Angstroms, decreases. The atomic radius consists entirely of the electron cloud around the nucleus, and as the nuclear charge increases with increasing atomic number (atomic number equals the number of protons in the nucleus), the electron cloud becomes held in more tightly.

So is the molecule O2 smaller than N2? Here you need to take into account the bond length for these diatomic species. O2 has a bond length of 121 pm (picometers), and nitrogen is 110 pm. The reason for this is that the bond order for N2 is 3, whereas the bond order for oxygen is 2. How much difference does this make in the diffusing capacity of the two gases? I don't know, but room air is like 79% nitrogen, anyway, so it seems silly to worry about it.

The one error in your presentation is the statement that N2 is not inert because there are many reactive nitrogen species that are not N2. N2 is somewhat reactive at high temperatures - that's where we get our oxides of nitrogen in our exhaust. However, equating N2 with NH3 or any other molecule containing nitrogen is just as silly as equating benzene with diamonds or glucose. Or saying that diamonds should be flammable because benzene is. All these molecules contain carbon but... Reactivity, physical properties - all have to do with molecular structure, oxidation state, physical shape of molecules, and so on.

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