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when zinc metal reacts with oxygen gas, 2zn(s) + o2(g) → 2zno(g), large amounts of light and heat are released. a student states that this reaction is a combustion reaction but not a redox reaction. do you agree? defend your answer by explaining whether or not it meets the requirements of each type of reaction.

Explanation:

1. Combustion?

It is difficult to get zinc to burn but, when you heat it in pure oxygen, it burns rapidly with a blue flame and the production of a large amount of heat.

Combustion is the rapid chemical combination of a substance with oxygen, involving the production of heat and light.

Thus, the reaction meets the requirements for being a combustion.

2. Redox reaction?

Zn is a metal and O₂ is a nonmetal, so ZnO is an ionic compound.

It consists of Zn²⁺ ions and O²⁻ ions.

Zn ⟶ Zn²⁺ + 2e⁻

When Zn becomes Zn²⁺, it loses electrons, and loss of electrons is oxidation.

O₂ + 4e⁻ ⟶ 2O²⁻  

When O becomes O²⁻, it gains electrons, and gain of electrons is reduction.

Thus, the reaction meets the requirements for a redox reaction.