Consider the first ionization energies of the elements whose electronic configurations correspond to the following.
I. `[He]2s^(2) 2p^3`
II. `[He]2s^(2) 2p^4`
III. `[Ne]3s^(2)3p^(1)`
`[Ar]3d^(10)4p^1`
Which of the above have almost the same first ionization energies?

Options

A. I and II
B. I and III
C. III and IV
D. II and IV

Explanation

To determine which of the given electronic configurations correspond to elements with almost the same first ionization energies, we will follow these steps:

### Step 1: Identify the Elements
We start by identifying the elements corresponding to the given electronic configurations.

1. **Configuration I: `[He] 2s^2 2p^3`**
- This configuration corresponds to Nitrogen (N), which has an atomic number of 7.

2. **Configuration II: `[He] 2s^2 2p^4`**
- This configuration corresponds to Oxygen (O), which has an atomic number of 8.

3. **Configuration III: `[Ne] 3s^2 3p^1`**
- This configuration corresponds to Aluminum (Al), which has an atomic number of 13.

4. **Configuration IV: `[Ar] 3d^{10} 4p^1`**
- This configuration corresponds to Gallium (Ga), which has an atomic number of 31.

### Step 2: Analyze the Position in the Periodic Table
Next, we will analyze the position of these elements in the periodic table to understand their ionization energies.

- **Nitrogen (N)** and **Oxygen (O)** are in the second period, with Oxygen having a higher ionization energy than Nitrogen due to its higher nuclear charge.
- **Aluminum (Al)** is in the third period, and **Gallium (Ga)** is in the fourth period. Both Aluminum and Gallium belong to Group 13 of the periodic table.

### Step 3: Compare Ionization Energies
Now we will compare the ionization energies of the identified elements:

- **Nitrogen (N)** has a relatively high ionization energy due to its small size and high effective nuclear charge.
- **Oxygen (O)** has a higher ionization energy than Nitrogen due to its increased nuclear charge but also experiences electron-electron repulsion in its p-orbitals.
- **Aluminum (Al)** has a lower ionization energy than Nitrogen and Oxygen because it is in a higher period and has a larger atomic radius.
- **Gallium (Ga)** has a similar ionization energy to Aluminum due to the poor shielding effect of the d-orbitals, which makes its effective nuclear charge comparable to Aluminum.

### Conclusion
From the analysis, we can conclude that:

- **Aluminum (Al)** and **Gallium (Ga)** have almost the same first ionization energies due to their similar atomic sizes and the effect of d-orbital shielding in Gallium.

Thus, the correct answer is that **III (Aluminum) and IV (Gallium)** have almost the same first ionization energies.

### Final Answer
**The elements with almost the same first ionization energies are Aluminum (III) and Gallium (IV).**

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