The spectral line obtained when an electron jumps from `n = 6 `to `n = 2` level in hydrogen atom belongs to the

Options

A. Balmer series
B. Lyman series
C. Paschen series
D. Pfund series

Explanation

To determine the series to which the spectral line obtained when an electron jumps from the n = 6 to n = 2 level in a hydrogen atom belongs, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Energy Levels**: In a hydrogen atom, electrons occupy discrete energy levels denoted by principal quantum numbers (n = 1, 2, 3, ...). The energy levels are quantized.

2. **Identify the Transition**: The question specifies a transition from n = 6 to n = 2. This means the electron is moving from a higher energy level (n = 6) to a lower energy level (n = 2).

3. **Determine the Series**: The spectral lines emitted during electron transitions correspond to specific series based on the final energy level:
- **Lyman Series**: Transitions to n = 1 (ultraviolet region)
- **Balmer Series**: Transitions to n = 2 (visible region)
- **Paschen Series**: Transitions to n = 3 (infrared region)
- **Brackett Series**: Transitions to n = 4 (infrared region)

4. **Identify the Correct Series for n = 2**: Since the electron is transitioning to n = 2, it falls into the Balmer series, which is specifically for transitions that end at n = 2.

5. **Conclusion**: Therefore, the spectral line obtained from the transition of an electron from n = 6 to n = 2 belongs to the **Balmer series**.

### Final Answer:
The spectral line obtained when an electron jumps from n = 6 to n = 2 level in a hydrogen atom belongs to the **Balmer series**.