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 energy is `-2.18xx10^(-11)` ergs.

Explanation

To solve the problem of finding the energy required to shift the electron of the hydrogen atom 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, we can follow these steps:

### Step 1: Determine the Energy Levels
The energy of an electron in the nth Bohr orbit of a hydrogen atom is given by the formula:
\[ E_n = -\frac{2.18 \times 10^{-11}}{n^2} \text{ ergs} \]

### Step 2: Calculate the Energy of the First and Fifth Orbits
1. For the first orbit (n=1):
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