`H^(+)`is a

A

Lewis acid

B

Lewis base

C

Bronsted-Lowry base

D

None of the above

Text Solution

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The correct Answer is:
**Step-by-Step Solution:** 1. **Identify the Species**: The question asks about \( H^+ \), which is the hydrogen ion. 2. **Understand the Nature of \( H^+ \)**: The \( H^+ \) ion is essentially a proton. It is formed when a hydrogen atom loses its electron. 3. **Determine the Chemical Behavior**: \( H^+ \) has a strong tendency to accept electrons because it has a positive charge and is electron-deficient. 4. **Relate to Lewis Acid Definition**: According to the Lewis theory of acids and bases, a Lewis acid is defined as a species that can accept a pair of electrons. Since \( H^+ \) can accept a lone pair of electrons, it fits the definition of a Lewis acid. 5. **Conclusion**: Therefore, \( H^+ \) is classified as a Lewis acid. **Final Answer**: \( H^+ \) is a Lewis acid. ---
**Step-by-Step Solution:** 1. **Identify the Species**: The question asks about \( H^+ \), which is the hydrogen ion. 2. **Understand the Nature of \( H^+ \)**: The \( H^+ \) ion is essentially a proton. It is formed when a hydrogen atom loses its electron. 3. **Determine the Chemical Behavior**: \( H^+ \) has a strong tendency to accept electrons because it has a positive charge and is electron-deficient. ...
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