Question

Which series of the Hydrogen spectrum lies in the visible region?

• A. Lyman Series
• B. Balmer Series
• C. Paschen Series
• D. Brackett Series

Hint:

Remember the order of hydrogen spectral series with increasing wavelength: Lyman (UV) → Balmer (Visible) → Paschen → Brackett → Pfund (Infrared).

Answer 1

The Correct Option is B

Concept:
The hydrogen atom emits spectral lines when an electron transitions between different energy levels. These spectral lines are grouped into series depending on the final energy level of the electron.
• Lyman Series: Ultraviolet region (\(n = 1\))
• Balmer Series: Visible region (\(n = 2\))
• Paschen Series: Infrared region (\(n = 3\))
• Brackett Series: Infrared region (\(n = 4\)) The wavelength of spectral lines in hydrogen is given by the Rydberg formula. \[ \frac{1}{\lambda} = R \left(\frac{1}{n_1^2} - \frac{1}{n_2^2}\right) \]

Step 1: Identify the series corresponding to the visible region.
In the hydrogen spectrum, transitions ending at the energy level \(n = 2\) produce visible spectral lines.

Step 2: Recognize the name of this series.
The spectral series corresponding to transitions terminating at \(n = 2\) is called the Balmer Series.

Step 3: State the conclusion.
Therefore, the hydrogen spectral series that lies in the visible region is the Balmer Series. \[ \boxed{\text{Balmer Series}} \]