When `Sn^(2+)` changes to `Sn^(4+)` in a reaction

Options

A. It loses two protons
B. It gains two electrons
C. It loses two electrons
D. It gains two protons

Explanation

To solve the question of how `Sn^(2+)` changes to `Sn^(4+)`, we can follow these steps:

### Step 1: Write the reaction
We start with the initial and final states of the tin ion:
\[ \text{Sn}^{2+} \rightarrow \text{Sn}^{4+} \]

### Step 2: Analyze the charges
Next, we need to analyze the charges on both sides of the equation:
- On the left side, we have `Sn^(2+)`, which has a charge of +2.
- On the right side, we have `Sn^(4+)`, which has a charge of +4.

### Step 3: Determine the change in charge
To balance the charges, we note that:
- The change in charge from +2 to +4 is an increase of 2 units of positive charge.

### Step 4: Identify electron loss
Since the charge is increasing, this indicates that the tin ion is losing electrons. Each electron carries a charge of -1. Therefore, to increase the positive charge by 2, `Sn^(2+)` must lose 2 electrons.

### Step 5: Write the balanced half-reaction
We can now write the balanced half-reaction to show the loss of electrons:
\[ \text{Sn}^{2+} \rightarrow \text{Sn}^{4+} + 2e^- \]

### Final Conclusion
Thus, when `Sn^(2+)` changes to `Sn^(4+)`, it loses 2 electrons.

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