Question is above. Thank you in advance
Hi, can anyone help me set up the redox equation for the following reaction in acidic aqueous solution? Reaction: COOH, MNO4^- + CO2, MN^2+ I've already listed the oxidation numbers, but I'm stuck. I've already listed the reduction number, but what about the oxidation number? I don't understand how to handle this with the hydrogen…
Oil floats on water. But if you put a cell phone in oil, will it also float on water?
Could someone sketch this for me
Hello, I have several questions about this program. I have been given spectra to evaluate, which I am supposed to analyze using Mmass. Unfortunately, the program crashes frequently, which is a clear indication that the adduct is incorrect. But in the spectra it is usually the case that only H+ peaks are visible next to…
I have a chemistry question. If I have a redox reaction and I want to set up the partial equation, I have to do the reduction and oxidation equations separately. But what do I do if I have two substances that are being oxidized/reduced? Do I have to set up the oxidation equation twice? Or…
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Moin,
You must be aware that a molecule with at least one atomic bond is produced according to a rule of thumb between at least two nonmetal atoms.
Then you can see which elements are suitable for this on the basis of a (good) PSE.
On the PSE, you can also see how many external electrons (valence electrons) have the atoms of the affected elements. Here the following applies: main group number = number of valence electrons.
At the period you realize how many shells have to be occupied with electrons at all. Depending on the position of the element, this results for the elements…
Depending on the position of the respective element, you have to paint various electrons into the third shell:
Then, with the help of the octet rule, you can come up with how many atomic bonds have to be formed so that all involved binding partners get their outer shell full of electrons (hydrogen needs 2 electrons, the other 8 electrons).
And then you just have to paint it up.
For the oxygen minimolecules, for example:
The four electrons in the overlap region belong simultaneously to the left AND to the right oxygen atom. As a result, both in their 2nd shell come to a total of 8 external electrons (Oktett rule). And in total, each O atom has 10 electrons (like the atom of the noble gas neon; noble gas rule).
For (essentially) larger molecules or those with many bonds, however, this is quickly confusing…
LG from the Waterkant
A very detailed and really helpful answer, thank you!!
You’re welcome.
For a molecule, a shell model does not really make sense. In simple cases, Lewis formulas are drawn into which only the valence electrons enter, i.e. the outer shell. The molecular orbital model provides a much better description, but this is also much more complicated. Beyond the PSE, you should be clear.
“For a molecule, a shell model doesn’t really make sense.” that’s true, but much in school doesn’t make sense 😀
Unfortunately, we must be able to do it in the exam as a shell model, I didn’t think it out.
Thanks for the answer!🙌🏼
From the PSE you can directly read the number of “shells” and the number of valence electrons for main group elements (period; No. 1-8)