The electron configuration of an element,X,is [Ne]3s¹^. The formula of the most probable ionic compound that this element will form with O is A)XO B)X₂O₃ C)X₂O D)X₃O₂

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The electron configuration of O is 1s2 2s2 2p4, so it has 6 valence electrons. X has 4 valence electrons in its 3s and 3p subshells. X will lose its 4 valence electrons to form X4+ ion and O will gain 2 electrons to form O2- ion. The resulting compound will have the formula XO2. However, since X can form multiple oxidation states (+1, +2, +3), there may be other possible compounds. Among the given choices, only option C has the correct ratio of ions (1:1) and the correct charges (+2 for X and -2 for O) to form a stable ionic compound.

The Electron Configuration of an Element,X,is [Ne]3s1

The Electron Configuration of an Element,X,is [Ne]3s¹