The energy required to remove an electron from the outermost shell of an isolate gaseous atom is known as `IE_(1)` of that atom. Similarly, the energy required for the removal of the electron from the unipositive ion, diapositive ion and tripositive ion are known as `IE_(2),IE_(3)` and `IE_(4)` respectively, and are called successive ionisation energies. The magnitude of the charge depends on the size of the orbital of electron. Electrons in smaller orbitals are on average close with each other and have more repulsion. Thus for `Be(2s^(2))`, the `IE_(1)` and `IE_(2)` are `9.3` and `18.2 eV "atom"^(1)`, whereas for `Ca(4s^(2))`, the values are `6.1` and `11.9 eV`.
Consider the `IE_(1)` of the element whose electronic configurations correspond to the following

Options

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

Explanation

To solve the problem, we need to determine the first ionization energy (IE₁) of different elements based on their electronic configurations. We will analyze the provided configurations step by step.

### Step-by-Step Solution:

1. **Identify the Elements from Electronic Configurations:**
- **Configuration 1:** He 2s² 2p³
- This configuration corresponds to Nitrogen (N), which has an atomic number of 7.
- **Configuration 2:** He 2s² 2p⁴
- This configuration corresponds to Oxygen (O), which has an atomic number of 8.
- **Configuration 3:** Ne 3s² 3p¹
- This configuration corresponds to Aluminum (Al), which has an atomic number of 13.
- **Configuration 4:** Ar 3d¹⁰ 4s² 4p¹
- This configuration corresponds to Gallium (Ga), which has an atomic number of 31.

2. **Compare the Ionization Energies:**
- From the provided information, we know that:
- The first ionization energy of Nitrogen (IE₁ for N) is higher than that of Oxygen (IE₁ for O) due to the half-filled p subshell stability in Nitrogen.
- The first ionization energy of Aluminum (IE₁ for Al) is generally lower than that of Gallium (IE₁ for Ga) due to the increase in atomic size down the group. However, because of the poor shielding effect of the d-electrons in Gallium, the IE₁ of Ga can be comparable to that of Al.

3. **Conclusion:**
- The first ionization energies of Aluminum and Gallium are expected to be approximately the same due to the poor shielding effect of the d-electrons in Gallium. Thus, the answer to the question is that the first ionization energies of Aluminum and Gallium are comparable.

### Final Answer:
The first ionization energy (IE₁) of Aluminum (Al) and Gallium (Ga) are approximately the same due to the poor shielding effect of the d-electrons in Gallium.