Which of the following require maximum amount of energy ?

Options

A. `NerarrNe^(+)+e^(ө)`
B. `Be^(+2)rarrBe^(+3)+e^(ө)`
C. `LirarrLi^(+)+e^(ө)`
D. `MgrarrMg^(+)+e^(ө)`

Explanation

To determine which of the given options requires the maximum amount of energy to remove an electron, we need to analyze the electronic configurations of the elements in question. Here’s a step-by-step solution:

### Step 1: Identify the Electronic Configurations
- **Option A:** Lithium (Li) - 1s² 2s¹
- **Option B:** Beryllium (Be) - 1s² 2s²
- **Option C:** Neon (Ne) - 1s² 2s² 2p⁶
- **Option D:** Magnesium (Mg) - 1s² 2s² 2p⁶ 3s²

### Step 2: Determine the Stability of Each Configuration
- **Lithium (Li):** Has one electron in the outermost shell (2s¹). Removing this electron will require less energy because it is relatively far from the nucleus and experiences less effective nuclear charge.
- **Beryllium (Be):** Has two electrons in the outermost shell (2s²). Removing one of these electrons requires more energy than lithium because it has a higher effective nuclear charge.
- **Neon (Ne):** Has a complete outer shell (2s² 2p⁶). Removing an electron from a noble gas configuration requires a significant amount of energy due to its stability.
- **Magnesium (Mg):** Has two electrons in the outermost shell (3s²). Although it has a higher principal quantum number, the outermost electrons are still relatively shielded, requiring less energy than removing an electron from a noble gas.

### Step 3: Compare Ionization Energies
- Ionization energy generally increases across a period and decreases down a group. Since Neon is a noble gas with a full outer shell, it will have the highest ionization energy among the options provided.

### Conclusion
The element that requires the maximum amount of energy to remove an electron is **Neon (Ne)**.

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