Question

The emission spectrum of an unknown atom contains six visible wavelengths (in nm):

425 573 505 645 546 484
The maximum light output (intensity) occurs at 484nm. Which of the six emission wavelengths, if any, corresponds to the largest difference in energy between the energy levels responsible for the emission? If none of the wavelengths is a choice write NOW (= none of the wavelengths).

Answer 1

The wavelength 425 nm corresponds to the largest difference in energy between the energy levels responsible for the emission in an atom's spectrum, because shorter wavelengths indicate higher energy transitions.

Step-by-step explanation:

The wavelength corresponding to the largest difference in energy between the energy levels responsible for the emission in an atom's spectrum can be determined using the relationship between energy and wavelength.

According to Planck's equation, the energy (E) of a photon is inversely proportional to its wavelength (λ), and it is given by E = hc/λ, where h is Planck's constant and c is the speed of light in a vacuum. Therefore, the shortest wavelength corresponds to the highest energy transition.

Among the provided wavelengths, 425 nm is the shortest wavelength and thus it corresponds to the largest difference in energy between the energy levels responsible for the emission. Hence, the wavelength of 425 nm would represent the transition with the greatest energy change.