Which of the following orders of ionic radii is correctly represented?

Options

A. `H^(-) gt H^(+) gt H`
B. `Na^(+) gt F^(-) gt O^(2-)`
C. `F^(-) gt O^(2-) gt Na^(+)`
D. `Al^(3+) gt Mg^(2+) gt N^(3-)`

Explanation

To determine the correct order of ionic radii among the given options, we need to analyze the ionic forms of hydrogen, sodium, fluoride, oxide, aluminum, magnesium, and nitrogen. Here's a step-by-step solution:

### Step 1: Understand Ionic Forms
- **Hydrogen (H)** has one proton and one electron.
- **Hydride ion (H⁻)** is formed when hydrogen gains an electron, resulting in one proton and two electrons.
- **Hydrogen ion (H⁺)** is formed when hydrogen loses its electron, resulting in one proton and no electrons.

### Step 2: Compare Sizes of Hydrogen Ions
- **H⁻ (Hydride)**: Has two electrons, which means the effective nuclear charge (the ability of the nucleus to attract electrons) is weaker because one proton is binding two electrons. Hence, H⁻ is larger than H.
- **H (Neutral Hydrogen)**: Has one proton and one electron, so it has a normal size.
- **H⁺ (Hydrogen Ion)**: Has one proton and no electrons, making it the smallest since there are no electrons to repel each other.

### Step 3: Analyze Sodium, Fluoride, and Oxide Ions
- **Sodium ion (Na⁺)**: Atomic number 11, loses one electron, resulting in 10 electrons.
- **Fluoride ion (F⁻)**: Atomic number 9, gains one electron, resulting in 10 electrons.
- **Oxide ion (O²⁻)**: Atomic number 8, gains two electrons, resulting in 10 electrons.

### Step 4: Determine Ionic Sizes
- All three ions (Na⁺, F⁻, O²⁻) are isoelectronic (same number of electrons). The size of isoelectronic species depends on the number of protons:
- **Na⁺ (11 protons)**: Smallest size due to the highest positive charge attracting electrons.
- **F⁻ (9 protons)**: Larger than Na⁺.
- **O²⁻ (8 protons)**: Largest size because it has the least positive charge.

### Step 5: Analyze Aluminum, Magnesium, and Nitrogen Ions
- **Aluminum ion (Al³⁺)**: Atomic number 13, loses three electrons, resulting in 10 electrons.
- **Magnesium ion (Mg²⁺)**: Atomic number 12, loses two electrons, resulting in 10 electrons.
- **Nitride ion (N³⁻)**: Atomic number 7, gains three electrons, resulting in 10 electrons.

### Step 6: Determine Sizes of These Ions
- All three ions are also isoelectronic. The sizes will depend on the number of protons:
- **Al³⁺ (13 protons)**: Smallest size.
- **Mg²⁺ (12 protons)**: Larger than Al³⁺.
- **N³⁻ (7 protons)**: Largest size.

### Conclusion
Based on the analysis:
- The order of ionic radii from smallest to largest is:
- H⁺ < Na⁺ < F⁻ < O²⁻ < Al³⁺ < Mg²⁺ < N³⁻

Since the options provided in the question are incorrect, the final answer is **None of these**.