Assertion: Amines are basic in nature.
Reason: Presence of ione pair of electron on nitrogenatom.

Explanation

**Step-by-Step Solution:**

1. **Understanding the Assertion:**
The assertion states that "Amines are basic in nature." This means that amines can accept protons (H⁺ ions) and therefore act as bases according to the Brønsted-Lowry definition of acids and bases.

**Hint:** Recall the definition of a base in the context of the Brønsted-Lowry theory.

2. **Understanding the Reason:**
The reason provided is "Presence of lone pair of electrons on nitrogen atom." Nitrogen in amines has a lone pair of electrons which can be used to bond with protons. This property is what makes amines basic.

**Hint:** Consider how the lone pair on nitrogen can interact with protons.

3. **Types of Amines:**
Amines can be classified into primary (1°), secondary (2°), and tertiary (3°) amines based on the number of alkyl or aryl groups attached to the nitrogen atom. All types of amines exhibit basic properties due to the lone pair of electrons.

**Hint:** Remember the structural differences between primary, secondary, and tertiary amines.

4. **Basicity Comparison:**
While all amines are basic, there is a distinction between aliphatic (alkyl) amines and aromatic amines. Aliphatic amines are generally more basic than aromatic amines due to the delocalization of the lone pair in aromatic systems, which reduces its availability for bonding with protons.

**Hint:** Think about how the structure of aromatic compounds affects electron availability.

5. **Conclusion:**
Both the assertion and the reason are true. The presence of the lone pair of electrons on the nitrogen atom is indeed the reason why amines are basic. Therefore, the assertion and reason support each other.

**Final Answer:** Both the assertion and reason are correct, and the reason is a correct explanation of the assertion.