Question

Choose the oxidation state for each reactant and product below.

Mg+S⟶Mg²⁺+S²⁻
A. Mg:0
B. S:0
C. Mg²⁺:+2
D. S²⁻:−2

Answer 1

The oxidation states for the reaction Mg + S → Mg²⁺ + S²⁻ are Mg: 0, S: 0, Mg²⁺: +2, and S²⁻: -2, indicating that Mg is oxidized and S is reduced.

Step-by-step explanation:

To determine the oxidation states for each reactant and product in the reaction Mg + S → Mg²⁺ + S²⁻, we must consider the rules for assigning oxidation numbers. For the elements in their elemental form, such as magnesium (Mg) and sulfur (S), the oxidation state is zero.

When these elements are transformed into ions, Mg becomes Mg²⁺ and S becomes S²⁻, reflecting their charges as ions. Therefore, the oxidation states for the given reaction are:

• Mg: 0
• S: 0
• Mg²⁺: +2
• S²⁻: −2

In the process, Mg is oxidized as it loses electrons and its oxidation state increases from 0 to +2. S is reduced as it gains electrons, with its oxidation state going from 0 to -2.

This type of reaction, where there is a transfer of electrons between reactants, is a redox reaction.