Zn + 2HCL → ZnCl$_2$ + H$_2$  What happens to zinc in the above reaction?

Analyze the question: The question asks what happens to zinc in the reaction. This is about the change in zinc's oxidation state, which is a redox concept.

Concept:

• Oxidation = loss of electrons (oxidation number increases)
• Reduction = gain of electrons (oxidation number decreases)
• Memory aid: OIL RIG (Oxidation Is Loss, Reduction Is Gain)

Solution:

Zn + 2HCl → ZnCl₂ + H₂

1. Oxidation number of Zn on the left: 0 (free element)
2. Oxidation number of Zn on the right, in ZnCl₂: +2
3. Zn goes from 0 to +2, so it loses 2 electrons:

Zn → Zn²⁺ + 2e⁻ (oxidation)

4. Meanwhile, hydrogen goes from +1 in HCl to 0 in H₂, so H⁺ is reduced:

2H⁺ + 2e⁻ → H₂ (reduction)

So zinc is oxidized (it is also the reducing agent).

Checking the other options:

• B. "A reactant": true as a statement, since zinc is on the left side, but it does not describe what happens to it in the reaction. The question is asking about the chemical change.
• C. "Reduced": wrong, because zinc's oxidation number increases.
• D. "A metal": true, but it is a description of what zinc is, not what happens to it.

Answer: A. oxidized

Exam tip: For any redox question, write the oxidation numbers of each element before and after. If the number goes up, it is oxidized; if it goes down, it is reduced. Also, a free element (like Zn or H₂) always has an oxidation number of 0.