The transition of electron from n = 3 to n = 1 in H atom produces

Options

A. Emission spectrum
B. Absorption spectrum
C. Paschen line
D. Pfund line.

Explanation

To determine the outcome of the transition of an electron from n = 3 to n = 1 in a hydrogen atom, we can follow these steps:

### Step 1: Understand the Energy Levels
In a hydrogen atom, electrons occupy specific energy levels, denoted by the principal quantum number \( n \). The ground state of hydrogen corresponds to \( n = 1 \), while \( n = 3 \) is an excited state.

**Hint:** The principal quantum number \( n \) indicates the energy level of an electron in an atom.

### Step 2: Identify the Transition
The transition from \( n = 3 \) to \( n = 1 \) indicates that the electron is moving from a higher energy level to a lower energy level. This is a downward transition.

**Hint:** When an electron moves to a lower energy level, it releases energy.

### Step 3: Determine the Type of Spectrum
When an electron transitions from a higher energy level to a lower energy level, it emits energy in the form of electromagnetic radiation. This process produces an emission spectrum.

**Hint:** Emission spectra are produced when electrons fall to lower energy levels and release energy.

### Step 4: Identify the Wavelength of Emission
The specific transition from \( n = 3 \) to \( n = 1 \) corresponds to the emission of a photon with a specific wavelength. In the case of hydrogen, this transition falls within the ultraviolet region of the electromagnetic spectrum and is part of the Lyman series.

**Hint:** The Lyman series involves transitions to the ground state (n=1) and emits ultraviolet light.

### Conclusion
The transition of an electron from \( n = 3 \) to \( n = 1 \) in a hydrogen atom produces an **emission spectrum**.

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