Which of the following statement are true for the above Lewis structures ?

Question

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Which of the following statement are true for the above Lewis structures ?

a) There are atoms in both of these structures with non-zero formal charges

b) The structures represent different compounds

c) The number of atoms S is bonded to is 4 in each structure

d) The number of atoms S is bonded to plus the number of lone pair electrons it has is equal to 4 in each structure


enter all tru statments

Answer 1

You should realize that both of these structures are essentially the same. They each show the central Sulfur with three bonds and one lone pair of electrons. This atom would have a formal +1 charge (one electron per bond plus the lone pair, 6 - 5 = +1).

The Oxygen atom without an attached Hydrogen is shown with 3 lone pairs. This would have a formal charge of -1 (6 -7 = -1).

a) is true.

b) and c) are false.

d) is also true (3 + 1 = 4).

Answer 2

Only d) is true. a) is false, because the S-O, where the O has three more lone-pair electrons around it, is a coordinate covalent bond, which is usually drawn S->O. That means that both electrons to be shared between the S and that O are donated by the S.

Answer 3

Lewis structures will not keep you warm on a cold night. All the others are true.

Answer 4

Just d