What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit ? And what is the wavelength of the light emitted when the electron returns to the ground state ? The ground state electron energy is ` -2 18 xx 10 ^(-11)` erg.

Explanation

To solve the problem, we will follow a systematic approach to find the energy required to shift the electron from the first Bohr orbit to the fifth Bohr orbit and the wavelength of the light emitted when the electron returns to the ground state.

### Step 1: Calculate the energy of the electron in the first Bohr orbit (E1)
The formula for the energy of an electron in the nth Bohr orbit is given by:

\[ E_n = -\frac{2.18 \times 10^{-11}}{n^2} \text{ erg} \]
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