A hydrogen atom in its excited state emits radiations of wavelengths 1218 Å and 974.3 Å when it finally comes to the ground state. Identify the energy levels from where transitions occur. Given Rydberg constant `R = 1.1 xx 10^7 m^(-1)`. Also specify the spectral series to which these lines belong.

Explanation

To solve the problem, we need to identify the energy levels from which the transitions occur for the given wavelengths of emitted radiation from a hydrogen atom. We will use the Rydberg formula to find the initial energy levels and specify the spectral series.

### Step-by-Step Solution:

1. **Understanding the Rydberg Formula**:
The Rydberg formula for the wavelengths of spectral lines in hydrogen is given by:
\[
\frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)
...