Identify the `Mg^(2+)` ion from the figure where, n and p represent the number of neutrons and protons respectively.

Options

A.
B.
C.
D.

Explanation

To identify the `Mg^(2+)` ion from the given figures, we can follow these steps:

### Step 1: Understand the Atomic Structure of Magnesium
- The atomic number of magnesium (Mg) is 12. This means it has 12 protons (p = 12).

### Step 2: Determine the Number of Neutrons
- The mass number of magnesium is given as 24. The mass number is the sum of protons and neutrons.
- Therefore, the number of neutrons (n) can be calculated using the formula:
\[ \text{Mass Number} = \text{Number of Protons} + \text{Number of Neutrons} \]
\[ 24 = 12 + n \implies n = 24 - 12 = 12 \]
- Thus, magnesium has 12 neutrons.

### Step 3: Analyze the `Mg^(2+)` Ion
- The `Mg^(2+)` ion indicates that magnesium has lost 2 electrons.
- The electronic configuration of neutral magnesium is `K^2 L^8 M^2`, which means it has 12 electrons.
- After losing 2 electrons, the electronic configuration of `Mg^(2+)` becomes `K^2 L^8`, which means it now has 10 electrons.

### Step 4: Confirm the Number of Protons and Neutrons in `Mg^(2+)`
- The number of protons remains the same (12) because the atomic number does not change.
- The number of neutrons also remains the same (12) since losing electrons does not affect the number of neutrons.

### Step 5: Identify the Correct Option
- Now, we need to find the figure that represents `Mg^(2+)` with 12 protons and 12 neutrons.
- Look for an option where the number of protons (p) is 12 and the number of neutrons (n) is also 12.

### Conclusion
- The correct option that corresponds to the `Mg^(2+)` ion is the one where both the number of protons and neutrons are equal to 12. This is represented by option D.

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