Amongst the following elements (whose electronic configuration an given below) the one having bighest ionization energy is

Options

A. `[Ne]3s^(2)3p^(1)`
B. `[Ne]3s^(2)3p^(3)`
C. `[Ne]3s^(2)3p^(2)`
D. `[Ar]3d^(10)4s^(2)4p^(3)`

Answer

To determine which element has the highest ionization energy among the given options based on their electronic configurations, we can follow these steps:

### Step 1: Understand Ionization Energy
Ionization energy is defined as the minimum energy required to remove an electron from an atom in its gaseous state. Generally, the higher the ionization energy, the more difficult it is to remove an electron.

### Step 2: Analyze the Electronic Configurations
We need to analyze the electronic configurations provided for the elements. The configurations will help us understand the arrangement of electrons and their stability.

### Step 3: Consider the Factors Affecting Ionization Energy
1. **Atomic Size**: As the atomic size increases, the ionization energy generally decreases because the outermost electrons are farther from the nucleus and experience less nuclear attraction.
2. **Nuclear Charge**: A higher nuclear charge (more protons in the nucleus) increases the attraction on the electrons, leading to higher ionization energy.
3. **Shielding Effect**: Inner electrons can shield outer electrons from the full effect of the nuclear charge, reducing the ionization energy.
4. **Electron Configuration Stability**: Atoms with filled or half-filled subshells are more stable and have higher ionization energies.

### Step 4: Compare the Given Configurations
Let’s denote the configurations as follows:
- A: 3P1
- B: 3P3
- C: 3P6
- D: 3P2

Now, we can analyze each configuration:
- **3P1**: This configuration has one electron in the p subshell, which is relatively less stable.
- **3P2**: This configuration has two electrons in the p subshell, which is slightly more stable than 3P1.
- **3P3**: This configuration has three electrons in the p subshell, which is more stable and has a half-filled subshell, providing additional stability.
- **3P6**: This configuration has a full p subshell, which is the most stable configuration.

### Step 5: Determine the Highest Ionization Energy
Based on the stability of the configurations:
- The 3P3 configuration (B) is more stable than 3P1 and 3P2.
- The 3P6 configuration (C) is the most stable due to being fully filled.

Thus, the element with the configuration **3P6** will have the highest ionization energy due to its full p subshell, which provides maximum stability and requires more energy to remove an electron.

### Conclusion
The element with the highest ionization energy among the given options is the one with the electronic configuration **3P6**.

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