Which one of the following should be most stable

Options

A. `H_(2)^(+)`
B. `H^(+)`
C. H
D. `H^(-)`

Explanation

To determine which of the given options is the most stable, we need to analyze the electronic configuration of hydrogen and its ion forms.

### Step-by-Step Solution:

1. **Identify the Electronic Configuration of Hydrogen (H)**:
- Hydrogen has an atomic number of 1, which means it has one electron.
- The electronic configuration of hydrogen is 1s¹.

2. **Consider the Ionized Forms**:
- **Hydrogen Ion (H⁺)**: When hydrogen loses its electron, it becomes H⁺. The electronic configuration of H⁺ is empty (0 electrons).
- **Hydride Ion (H⁻)**: When hydrogen gains an electron, it becomes H⁻. The electronic configuration of H⁻ is 1s².

3. **Evaluate Stability**:
- Stability in atoms and ions is often associated with having a filled outer shell (or subshell).
- For hydrogen:
- H⁺ has no electrons, making it highly reactive and unstable.
- H⁻ has two electrons in the 1s orbital, which means it has a filled orbital (1s²). This configuration is stable because filled orbitals tend to lower the energy of the atom or ion.

4. **Conclusion**:
- Among H, H⁺, and H⁻, the H⁻ ion is the most stable due to its filled 1s orbital (1s²).
- Therefore, the answer is H⁻.

### Final Answer:
The most stable option is **H⁻**.

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