Chemical insanity!

Pre-College Issues High School Life
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<p>Actually, it's not insane at all. Here is my question:</p>

<p>For the Resonance structures of NO2F, I know there are no unshared electron pairs and there is always only one single bond with the F. For the O, I know we use one single and one double bond. Would you put 3 pairs of electrons on the o with the single bond and 2 on the o with the double bond or would both Os have only 2 electron pairs? Any help would be great.</p>

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<p>Also I hate to be a bother, but does the lewis structure for h2o2 have any unshared electron pairs? Do we use double or triple bonds or is it just a single bond with unpaired electrons?</p>

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<p>please help me!</p>

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<p>I have no idea about the answer to your question but just wanted to tell you I like your screenname. I have no idea why I find it funny but I just do.</p>

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<p>
[quote]
Also I hate to be a bother, but does the lewis structure for h2o2 have any unshared electron pairs? Do we use double or triple bonds or is it just a single bond with unpaired electrons?

[/quote]
</p>

<p>I'm not good at chem either but i'll try;</p>

<p>h202 has 4 unshared electron pairs i belive. 2 pairs on O, each.
so, it will be : H - O - O - H
with 2 lone pairs on the O's (each)</p>

<p>And i dont really get what you mean by 'showing them with single/double/triple lines'. Don't you just represent them with dots..? Sorry i'd try draw it for you but i cant really.</p>

<p>Sorry if the info's wrong.. acutally i dont really know the answer- it's just my theory lol</p>

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<p>oh and i like ur sn also</p>

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<p>First, for NO2F (and for any resonance structures), you must draw all possibilities. So you draw a structureconnecting one of the oxygen with a double bonds, giving it two lone pairs, and the other oxygen with a single bond, this one having three lone pairs. Then switch, and have the first oxygen with a single bond and the second with a double, also switching the number of lone pairs on each (here is an example with Benzene - <a href="http://www.chem.wisc.edu/%7Enewtrad/CurrRef/BDGTopic/BDGFigs/2_6benz.gif%5B/url%5D"&gt;http://www.chem.wisc.edu/~newtrad/CurrRef/BDGTopic/BDGFigs/2_6benz.gif&lt;/a&gt;)&lt;/p>

<p>For H2O2, you will have one oxygen in the middle with one free/lone pair of electrons, connected to both the Hs and another oxygen,which will have 3 lone pairs.</p>

<p>For lone electrons, just draw them as dots (no bonds) (here is water as an example <a href="http://members.aol.com/rottenrat/chem9/h2o2.gif%5B/url%5D"&gt;http://members.aol.com/rottenrat/chem9/h2o2.gif&lt;/a&gt;)&lt;/p>

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<p>hahaha ok yeah i was wrong then ignore my post!</p>

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<p>thanks but it was already collected and discussed. nofx you actually were correct about the nofx, but bcc is correct about no2f. i ended up figuring it out myself but thanks.</p>

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<p>Ooops, nofx was right about the structure for the hydrogen peroxide... god i hate molecular orbital theory :(</p>