Describe the orbital with following quantum numbers:
(i) n=3, l=2
(ii) n=4, l=3

Options

A. (i) 3p, (ii) 4f
B. (i) 3d, (ii) 4d
C. (i) 3f, (ii) 4f
D. (i) 3d, (ii) 4f

Explanation

To describe the orbitals corresponding to the given quantum numbers, we need to understand the significance of the principal quantum number (n) and the azimuthal quantum number (l).

### Step-by-Step Solution:

1. **Understanding Quantum Numbers**:
- The principal quantum number (n) indicates the energy level or shell of the electron. It can take positive integer values (1, 2, 3, ...).
- The azimuthal quantum number (l) determines the shape of the orbital and can take integer values from 0 to (n-1). The values of l correspond to different types of orbitals:
- l = 0: s orbital
- l = 1: p orbital
- l = 2: d orbital
- l = 3: f orbital

2. **Analyzing the First Set of Quantum Numbers (n=3, l=2)**:
- Here, n = 3 and l = 2.
- Since l = 2, this corresponds to a d orbital.
- Therefore, the orbital is a **3d orbital**.

3. **Analyzing the Second Set of Quantum Numbers (n=4, l=3)**:
- Here, n = 4 and l = 3.
- Since l = 3, this corresponds to an f orbital.
- Therefore, the orbital is a **4f orbital**.

4. **Final Description**:
- The orbital with quantum numbers n = 3 and l = 2 is the **3d orbital**.
- The orbital with quantum numbers n = 4 and l = 3 is the **4f orbital**.

### Summary:
- (i) n=3, l=2 → **3d orbital**
- (ii) n=4, l=3 → **4f orbital**