To solve this problem, let's carefully analyze the given chemical equation:
[tex]\[
Mg _{( s )}+ H ^{+} Cl ^{-} \rightarrow Mg ^{2+} Cl ^{-}+ H _2
\][/tex]
We need to determine what happens to the magnesium in this reaction. Here are the steps to guide us through the analysis:
1. Identify the initial state of Magnesium (Mg):
- Magnesium in its solid state is represented as [tex]\( Mg \)[/tex] (s). In this form, magnesium is in a neutral state, meaning it has no charge.
2. Identify the final state of Magnesium (Mg):
- On the product side of the equation, magnesium appears as [tex]\( Mg^{2+} \)[/tex]. This notation indicates that magnesium now has a charge of [tex]\( +2 \)[/tex].
3. Analyze the change in charge for Magnesium (Mg):
- Magnesium changes from a neutral state [tex]\( Mg \)[/tex] (s) to [tex]\( Mg^{2+} \)[/tex].
- This change implies that magnesium has lost electrons. Electrons carry a negative charge, so losing electrons results in a more positive charge.
4. Determine the number of electrons lost:
- Magnesium shifts from a neutral state [tex]\( Mg \)[/tex] with an oxidation state of 0 to an ion with a charge of [tex]\( +2 \)[/tex] ([tex]\( Mg^{2+} \)[/tex]).
- To move from 0 to [tex]\( +2 \)[/tex], magnesium must lose 2 electrons (each electron has a charge of [tex]\(-1\)[/tex]).
Based on the analysis, the most likely change for magnesium in this reaction is the loss of two electrons.
Thus, the correct answer to the question is:
Magnesium loses two electrons.
