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[tex]\[
\text{Mg}_{(s)} + \text{H}^{+} \text{Cl}^{-} \rightarrow \text{Mg}^{2+} \text{Cl}^{-} + \text{H}_2
\][/tex]

What most likely happens during this reaction?

A. Magnesium gains two electrons.
B. Magnesium loses two electrons.
C. Chlorine gains one electron.
D. Chlorine loses one electron.


Sagot :

To determine what most likely happens during the given chemical reaction:

[tex]\[ Mg_{(s)} + H^+ Cl^- \rightarrow Mg^{2+} Cl^- + H_2 \][/tex]

We need to analyze the changes in the oxidation states of the elements involved.

1. Magnesium (Mg):
- In its elemental form, magnesium (Mg) is in the zero oxidation state ([tex]\(Mg_{(s)}\)[/tex]).
- After the reaction, magnesium is present as [tex]\(Mg^{2+}\)[/tex], indicating it is in the +2 oxidation state.

Since magnesium goes from 0 to +2, it means that it has lost two electrons. The change can be written as:

[tex]\[ Mg \rightarrow Mg^{2+} + 2e^- \][/tex]

This illustrates that magnesium loses two electrons during the reaction.

2. Hydrogen (H):
- The hydrogen ion ([tex]\(H^+\)[/tex]) starts in the +1 oxidation state.
- In the product, hydrogen is present as [tex]\(H_2\)[/tex] gas, which is in the 0 oxidation state because [tex]\(H_2\)[/tex] is a diatomic molecule with no charge.

The reduction of hydrogen can be described as:

[tex]\[ 2H^+ + 2e^- \rightarrow H_2 \][/tex]

Hydrogen gains two electrons in this case, but the problem specifically concerns what happens to magnesium and chlorine.

3. Chlorine (Cl):
- Throughout the reaction, chlorine starts and remains as [tex]\(Cl^-\)[/tex] with a -1 oxidation state.

There is no change in the oxidation state of chlorine, so it neither gains nor loses electrons.

Summarizing from the steps:

- Magnesium loses two electrons.
- Hydrogen gains electrons.
- Chlorine’s oxidation state does not change.

Hence, based on the reaction, the correct and most likely event is:

[tex]\[ \text{Magnesium loses two electrons.} \][/tex]
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