Step 1: Understanding the Question:
The hydrogen emission spectrum consists of various sets of spectral lines grouped into series based on the electron's final energy level. We need to identify which one is visible to the human eye.
Step 2: Detailed Explanation:
The spectral series are defined by the principal quantum number of the lower energy state (\(n_1\)):
1. Lyman Series (\(n_1 = 1\)): Ultraviolet (UV) region.
2. Balmer Series (\(n_1 = 2\)): Visible region.
3. Paschen Series (\(n_1 = 3\)): Near-Infrared region.
4. Brackett Series (\(n_1 = 4\)): Infrared region.
5. Pfund Series (\(n_1 = 5\)): Far-Infrared region.
Since the Balmer series involves transitions from \(n_2>2\) to \(n_1 = 2\), the energy released corresponds to wavelengths between approximately \(400\,\text{nm}\) and \(700\,\text{nm}\), which is the visible spectrum.
Step 3: Final Answer:
The Balmer Series lies in the visible region.