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

Options

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

Answer

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

### Step 1: Identify the Initial and Final Energy Levels
The electron is transitioning from the \( n = 6 \) level (initial state) to the \( n = 2 \) level (final state).

### Step 2: Determine the Series of the Transition
In hydrogen, spectral lines are categorized into different series based on the principal quantum numbers involved in the transitions:
- **Lyman series**: Transitions to \( n = 1 \) (from \( n = 2, 3, 4, \ldots \))
- **Balmer series**: Transitions to \( n = 2 \) (from \( n = 3, 4, 5, 6, \ldots \))
- **Paschen series**: Transitions to \( n = 3 \) (from \( n = 4, 5, 6, \ldots \))
- **Brackett series**: Transitions to \( n = 4 \) (from \( n = 5, 6, 7, \ldots \))

### Step 3: Classify the Transition
Since the electron is moving from \( n = 6 \) to \( n = 2 \), we can see that this transition falls under the Balmer series, which includes transitions to the \( n = 2 \) level from higher levels (3, 4, 5, 6, etc.).

### Conclusion
Thus, the spectral line obtained when an electron jumps from \( n = 6 \) to \( n = 2 \) in a hydrogen atom belongs to the **Balmer series**.

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