The energy levels of an atom of element X are shown in the diagram. Which one of the level transitions will result in the emission of photons of wavelength 620 nm ? Support your answer with mathematical calculations.

The energy levels of an atom are as shown in Fig.1.23 Which one of these transitions will results in the emission of a photon of wavelength 275 nm? .

The energy levels of an atom are as shown in Fig.1.23 Which transition corresponds to emission of radiation of maximum wavelength? .

The energy level diagram of an element is given below. Identify by doing necessary calculations, which transitions corresponds to the emission of a spectral line of wavelength 102.7nm

A hydrogen atom initially in the ground level absorbs a photon, which excites it to the n = 4 level. Determine the wavelength and frequency of photon.

If the lowest energy X-rays have lambda=3.055xx10^(-8) m, estimate the minimum difference in energy between two Bohr's orbits such that an electronic transition would correspond to the emission of an X-ray. Assuming that the electrons in other shells exert no influence, at what Z (minimum) would a transition form the second level to the first result in the emission of an X-ray?

What is the wavelength of light emitted when the electron in hydrogen atom undergoes transition from an energy level with n = 6 to an energy level with n = 3 ?

The energy of a I,II and III energy levels of a certain atom are E,(4E)/(3) and 2E respectively. A photon of wavelength lambda is emitted during a transition from III to I. what will be the wavelength of emission for II to I?

Followig table gives information on three lines observed in the emissin spectrum of hydrogen atoms. Complete the above table by calculating the photon energy for the wavelength of 486 nm.