Hello everybody. I have some questions I will post without further ado.
1. Au has 1 valence electron, and the same goes for Na. Can Au and Na be considered radicals (in the form which they appear in the periodic table)?
2. Radicals are highly reactive; but this doesn't seem to be the case for Au, as you can find big lumps of gold naturally, and practically every text book states that gold is not very reactive at all. I am assuming that this is because an Au-atom shares its valence electron with all the other Au-atoms in the compound. Is my assumption correct? If no, please elaborate.
3. If the answer to question 2 is yes, why is it that you cannot find pure Na in nature? I went ahead and assumed this after googling it.
4. This question is easier to ask if you follow the following steps:
- Go to
http://www.colby.edu/chemistry/OChem/DEMOS/MassSpec.html- Click on the animation window to start the animation
- Click on the ionization chamber (where it says 50-70 eV)
- Click on continue 3 times
If a molecule loses two electrons, how is it that it is still a
radical cation, and not just a cation? I can imagine that the two electrons might be picked off from different locations in the electron cloud, but wouldn't the two remaining lone electrons in the ion pair together?
5. I am supposed to predict the ratio between the relative areas under the chemical shifts using
1H-NMR spectroscopy on CH
3-CH
2Cl, which I found to be 2:1 (From CH
3:From CH
2). The answer is supposed to be 3:2, which, after an hour of work, still doesn't make sense to me.
All constructive replies will be highly appreciated.