Question

Determine the oxidation state of sulfur in SF₆, SO₂F₂, and KHS.

a. SF₆: +6, SO₂F₂: +4, KHS: -1
b. SF₆: -6, SO₂F₂: +4, KHS: +1
c. SF₆: +6, SO₂F₂: +2, KHS: +1
d. SF₆: +6, SO₂F₂: +4, KHS: -1

Answer 1

The oxidation states of sulfur in SF₆, SO₂F₂, and KHS are +6, +4, and -1 respectively, by applying standard rules for determining oxidation numbers.

The correct answqer is A.

Step-by-step explanation:

To determine the oxidation state of sulfur in SF₆, SO₂F₂, and KHS, we apply the following rules of oxidation states. For SF₆, rule 3 indicates that fluorine has an oxidation state of -1. Since there are six fluorine atoms, the sum of their oxidation states is -6. Sulfur must therefore have an oxidation state of +6 to balance out the fluorine and make the molecule neutral.

In SO₂F₂, oxygen has an oxidation state of -2 according to rule 5. With two oxygen atoms, this contributes a -4 charge. Since there are also two fluorine atoms, each with a -1 oxidation state, sulfur's oxidation state in SO₂F₂ must be +4 to balance the molecule.

For KHS, hydrogen has an oxidation state of +1, and since the molecule is neutral, sulfur must balance out the charges from potassium (K, which typically has an oxidation state of +1) and hydrogen. This means sulfur has an oxidation state of -1 in KHS.

Therefore, the correct answer is a. SF₆: +6, SO₂F₂: +4, KHS: -1.