In a hydrogen atom , an electron makes a transition from energy level of -1.51 eV to ground level . Calculate the wavelength of the spectral line emitted and identify the series of hydrogen spectrum to which this wavelength belongs.

Explanation

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

### Step 1: Identify the energy levels
In a hydrogen atom, the ground state energy level (n=1) is given by:
\[ E_1 = -13.6 \, \text{eV} \]
The initial energy level (n=2, corresponding to -1.51 eV) is:
\[ E_2 = -1.51 \, \text{eV} \]

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