The ground state energy of hydrogen atom is -13.6eV. If an electron makes a transition from an energy level -0.85 eV to -1.51 eV, calculate the wavelength of spectral line emitted. To which series of hydrogen spectrum does this wavelength belongs?

Explanation

To solve the problem of calculating the wavelength of the spectral line emitted when an electron transitions from an energy level of -0.85 eV to -1.51 eV in a hydrogen atom, we can follow these steps:

### Step 1: Identify the energy levels
The energy levels of the hydrogen atom can be expressed using the formula:
\[ E_n = -\frac{13.6 \, \text{eV}}{n^2} \]
where \( n \) is the principal quantum number.
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