The ground state energy of hydrogen atom is `-13.6eV`. If an electron makes a transition form an energy level `-0.85 eV` to `-3.4 eV`, calculate the wavelength of spectral line emitted. To which series of hydrogen spectrum does this wavelength belongs?

Explanation

To solve the problem, we need to calculate the wavelength of the spectral line emitted when an electron transitions from an energy level of -0.85 eV to -3.4 eV in a hydrogen atom. We will also determine which series of the hydrogen spectrum this wavelength belongs to.

### Step-by-Step Solution:

1. **Identify the Energy Levels**:
- The ground state energy of hydrogen is given as \( E_1 = -13.6 \, \text{eV} \).
- The energy levels can be calculated using the formula:
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