In the compound (WX) formed by the interaction of elements W and X, if element W possesses a single valence electron, it suggests that W is likely a metal, possibly from Group 1 of the periodic table (like sodium or potassium).
For W to form a stable compound with X, it typically loses that single valence electron to achieve a noble gas electron configuration, which means it will have a positive charge (W^+).
To maintain electrical neutrality in the compound WX, element X must be able to accept that electron. This implies that X must have a higher electronegativity and be capable of gaining an electron to reach a stable electron configuration.
Element X could likely be a nonmetal. Nonmetals that readily gain electrons to achieve a stable electron configuration often have six or seven valence electrons. For instance:
- If X has 7 valence electrons (like halogens), it can gain one electron to achieve a stable octet configuration.
- If X has 6 valence electrons (like oxygen), it can gain two electrons but would usually form a compound with two W atoms (W2X).
Therefore, the most probable count of valence electrons for element X in the compound WX, with W having one valence electron, is likely to be 7, making X similar to halogens that typically form -1 anions (like Cl^- in NaCl).
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