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Expert Solution

When deciding which of these Lewis structures is most reasonable, you must assign formal charges to each atom. The best Lewis structure has:

(A) The smallest and fewest formal charges (which still add up to the charge of the ion; in this case 2-)
(B) The negative formal charges on the most electronegative atoms (O or F)
(C) Any positive formal charges on the most electropositive atoms (P)
(D) "Like" formal charges (- and -, or + and +) on non-adjacent atoms, and
(E) "Opposite" formal charge (- and +) on adjacent atoms.

Formal charge: (Group number)-[(n of bonds)+ (n of electrons in lonely pairs)]

If you see C E and F are the same structure, in fact the double bond is placed in another oxigen. They are reasonable.

A and D have a positive formal charge en Fluor that is the most electronegative atom so are not reasonable.

B is reasonable because P is the most electropositive atom.

So B, C, E and F are the most reasonable structures.

queen_honey_blossom answered 1 hour ago

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