Can a S+ cation be formed with the electronic configuration 1s2,2s2,2p6,3s2,3p4?

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The discussion centers on the feasibility of forming a S+ cation from the electronic configuration 1s2, 2s2, 2p6, 3s2, 3p4. It is established that the valence electrons consist of 3s2 and 3p4, indicating that removing one electron from the p subshell to create a +1 cation is theoretically possible. However, the stability of the resulting cation in contact with other elements or molecules is questioned, emphasizing the importance of ionization energy and electron affinity in this context.

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Is it feasible to form a S+ cation?

Goin on the basis that the electronic configuration is 1s2,2s2,2p6,3s2,3p4

the valence electrons would be 3s2 and 3p4. So I'm thinking that it would be relatively easy to remove the 4th electron in the p subshell

BUT looking at the 6 valence electrons on the whole, with the sole purpose of any atom being to form a stable octet then would it lose an electron as opposed to gaining 2 in order to form the octet?

Please help me out...
 
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Try to analyze ionization energy and electron affinity.

Generally speaking it is always possible to ionize an atom and produce +1 cation in vacuum, question is, will it survive contact with other elements/ions/molecules?
 

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