A ground state hydrogen atom absorbs a photon of light having a wavelength of 92.27 nm. It then gives off a photon having a wavelength of 922.7 nm. What is the final state of the hydrogen atom? Values for physical constants can be found in the Chempendix.

The energy difference between the 1st excited state (n = 2) and the 2nd excited state (n = 3) in the hydrogen atom is 1.9 eV, what is the wavelength of the emission line resulting from the electron transitions between those two levels? Give your answer in units of nanometers (nm).

Chapter 39, Problem 044 A hydrogen atom in a state having a binding energy (the energy required to remove an electron) of -1.51 eV makes a transition to a state with an excitation energy (the difference between the energy of the state and that of the ground state) of 10.200 eV. (a) What is the energy of the photon emitted as a result of the transition? What are the (b) higher quantum number and (c) lower quantum number of the transition producing this emission? Use -13.60 eV as the binding energy of an electron in the ground state. (a) Number Units (b) Number Units (c) Number Units

A hydrogen atom initially in its ground state (n=1) absorbs a photon and ends up in the state for which n = 3. What is the energy of the absorbed photon?