Final answer:
The wavelength of light emitted during the transition from n = 236 to n = 235 for a hydrogen atom is approximately 1898 nm, which falls into the infrared region of the electromagnetic spectrum.
Step-by-step explanation:
To calculate the wavelength of light emitted when a hydrogen atom undergoes a transition from n = 236 to n = 235, we use the Rydberg formula for the hydrogen emission spectrum:
\(\frac{1}{\lambda} = R \left( \frac{1}{{n_f}^2} - \frac{1}{{n_i}^2} \right)\)
where:
- \(\lambda\) is the wavelength of the emitted light,
- \(R\) is the Rydberg constant (\(1.097 \times 10^7 m^{-1}\)),
- \(n_i\) is the initial energy level (236),
- \(n_f\) is the final energy level (235).
Plugging in the values, we get:
\(\frac{1}{\lambda} = 1.097 \times 10^7 m^{-1} \left( \frac{1}{235^2} - \frac{1}{236^2} \right)\)
After calculating, we find:
\(\lambda \approx 1.898 \times 10^{-3} m\)
or
\(\lambda \approx 1898 nm\) which falls into the infrared region of the electromagnetic spectrum.