The basic character of amines can be explained

Options

A. in terms of Lewis and Arrhenius
B. only in terms of Lowry Bronsted
C. in terms of Lewis and Lowry Bronsted
D. only Lewis concept

Explanation

To explain the basic character of amines, we will analyze it using three different theories: Lewis theory, Arrhenius theory, and Bronsted-Lowry theory.

### Step-by-Step Solution:

1. **Understanding Basicity**:
- Basicity refers to the ability of a substance to accept protons (H⁺ ions) or donate electron pairs. The basic character of amines can be explained through different acid-base theories.

2. **Lewis Theory**:
- According to Lewis theory, a base is defined as an electron pair donor. Amines contain a nitrogen atom with a lone pair of electrons. This lone pair can be donated to form a bond with a proton (H⁺), making amines Lewis bases.
- **Conclusion**: Amines are basic according to Lewis theory because they can donate their lone pair of electrons.

3. **Arrhenius Theory**:
- Arrhenius defined a base as a substance that increases the concentration of hydroxide ions (OH⁻) in solution. Amines do not directly produce OH⁻ ions when dissolved in water, so they do not fit this definition of a base.
- **Conclusion**: Amines do not qualify as bases under Arrhenius theory since they do not increase OH⁻ concentration.

4. **Bronsted-Lowry Theory**:
- Bronsted-Lowry theory defines a base as a substance that can accept protons (H⁺). Amines can accept protons due to the presence of the lone pair of electrons on the nitrogen atom. When an amine accepts a proton, it forms an ammonium ion (RNH₃⁺).
- **Conclusion**: Amines are basic according to Bronsted-Lowry theory because they can accept protons.

5. **Final Summary**:
- The basic character of amines can be explained through Lewis theory (as electron pair donors) and Bronsted-Lowry theory (as proton acceptors). However, they do not fit the Arrhenius definition of a base.