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Suppose I know that Selenium has electron configuration $[Ar] 4s^2 3d^{10} 4p^4$.

How can I use this information to then come to the conclusion that its possible oxidation states are 6, 4, 2, 1 and -2?

I understand the 6: Give up all s electrons to reach $Ar$ configuration I also understand the -2: Obtian two electrons to complete the 4th shell. I can guess why 4 is plausible: Give up all your 4p electrons

But 2 and 1? A guess for 2 would be to give up the 4s electrons, but why should it? And for the 1 I have no idea. Maybe give up one electron in the 4th shell and have it replaced by one of the 3d electrons?

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Oxidation number is an abstraction that is only useful to a certain extent: try to calculate it for $Fe$ in $Fe_3O_4$ and then relate it to its electron configuration. – gigacyan Jan 31 '11 at 8:07
up vote 1 down vote accepted

Dear Lagerbaer, first, this is an inorganic chemistry question. Chemistry is a subset of physics but it probably has special servers with questions and answers.

Second, one may get a rough idea about the oxidation numbers by your method but it's not universally valid. The oxidation number of an atom depends on the molecule in which the atom is incorporated. The "shape" of the atom (and its electron shells) in a molecule depends on and is also influenced by the other atoms.

By the way, I think that both parts of this sentence

I understand the 6: Give up all s electrons to reach Ar configuration I also understand the -2: Obtian two electrons to complete the 4th shell.

had bugs. I guess you meant that the oxidation number 6 is achieved by giving up all 4s and 4p electrons (rather than "all s electrons": 4p is not s) while -2 is obtained by getting two electrons to complete the 4p6 shell - which will not yet complete 4d and other 4th shells.

At any rate, in principle, you may get any oxidation number between the minimum and the maximum value. And the minimum and maximum values usually have an explanation of the kind you offered for +6 and -2.

The more electronegative the partner atoms will be, the higher (or more positive or less negative) the oxidation number of an atom will be. So there's no reason why it shouldn't happen that the partner atoms in the molecule will only remove or add a subset (a priori, any subset) of the removed or added electrons that you discussed in the case of +6 and -2. One has to check individual molecules to figure out whether a particular oxidation number is realized somewhere.

Selenium's oxidation numbers

In particular, selenium belongs to Group 16 - Oxygen, Sulphur, Selenium, etc. Their oxidation number is -2 unless they're combined with more electronegative elements - namely Oxygen or halogens. If they are, they may possess some positive oxidation numbers. To see that your list is the right one, one would have to go through all possible compounds - or at least all possible "neighborhoods of a Selenium atom" - and list all possibilities.

In principle, such things may be calculated from many-body quantum mechanics (assuming that we have a good enough definition of the oxidation state - it depends on some conventions). However, chemists don't do such things - instead, they learn many cases and acquire some experience.

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About this issue you can not finally conclude that its oxidation stage is 6,2 ,1 and -2 because the rules governing it has not been found. Rather you are to say the oxidation number of any element in a periodic table is found based on the column of the group it falls in to.

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Please adhere to standard orthography and typographic rules. – Sebastian Riese May 15 '15 at 11:17

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