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 an S+ cation from an atom with the electronic configuration of 1s2, 2s2, 2p6, 3s2, 3p4. The focus is on the valence electrons, specifically the 3s2 and 3p4 electrons, and the implications of removing an electron to achieve a stable octet. It is noted that while it is generally possible to ionize an atom to create a +1 cation in a vacuum, the real challenge lies in the stability of this cation when interacting with other elements, ions, or molecules. The discussion emphasizes the need to consider ionization energy and electron affinity in determining whether the atom would lose an electron or gain two to reach a stable state.
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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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