A photon of wavelength of 4.3408 X 10-7 meter enters a hydrogen atom whose electron is sitting at the second energy level (ni = 2). When the electron absorbs the photon, which energy level will it jump to (nf = ?)

An electron sitting in the -4eV energy level of this atom is struck with a photon of wavelength 345nm. As a result, the electron will -0.2 ev --0.4 ev -1.8 ev 4 ev O Absorb the photon and rise to the -0.4eV energy level Absorb the photon and rise to the -1.8eV energy level Not absorb the photon, and will remain in the -4eV energy level Absorb the photon and escape the atom Absorb the photon and rise to the -0.2eV energy level

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?

Give only typing answer with explanation and conclusion using the Bohr model, determine the energy in joules of the photon produced when an electron in a He+ ion moves from the orbit with n=10 to the orbit with n = 5. (assume that the Bohr constant and radius are 2.179X10^-18J and 5.292X10^-11m)