The electron energy in hydrogen atom is given by `E_(n)=-(2.18 xx 10^(-18))/(n^2) J`. Calculate the energy required to remove an electron completely from the n=2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?

Explanation

To solve the problem step by step, we will calculate the energy required to remove an electron from the n=2 orbit of a hydrogen atom and then find the longest wavelength of light that can cause this transition.

### Step 1: Calculate the Energy at n=2
The energy of an electron in a hydrogen atom is given by the formula:
\[ E_n = -\frac{2.18 \times 10^{-18}}{n^2} \text{ J} \]
For n=2, we substitute n into the formula:
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