The energ of the electron in the second and third Bohr orbit of hydrogen atom is `-5.42 xx 10^(-12)` erg and `-2.41 xx 10^(-12)` erg respectively. Calculate the wavelength of the emitted radiation when the electron drops from the third to second orbit. `(h= 6.62 xx 10^(-27) " erg".s, c=3 xx 10^(10) cm//s))`

Explanation

To solve the problem, we need to calculate the wavelength of the emitted radiation when the electron transitions from the third orbit (n=3) to the second orbit (n=2) in a hydrogen atom. We can use the energy values provided for the orbits and the formula for the wavelength of emitted radiation.

### Step-by-Step Solution:

1. **Identify the Energy Levels**:
- Given:
- Energy of the electron in the second orbit (n=2), \( E_2 = -5.42 \times 10^{-12} \) erg
- Energy of the electron in the third orbit (n=3), \( E_3 = -2.41 \times 10^{-12} \) erg
...