Hydrogen atoms can emit four spectral lines with visible colors between red and violet. (a) What is the longest, second longest, third longest, and shortest wavelength in the visible range? (b) What are the two quantum numbers of two states involved in the transition? (For the longest, second longest, third longest, and shortest wavelength)

Hydrogen atoms can emit four spectral lines with visible colors between red and violet. (a) What is the longest, second longest, third longest, and shortest wavelength in the visible range? (b) What are the two quantum numbers of two states involved in the transition? (For the longest, second longest, third longest, and shortest wavelength)

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter11: Gravity, Planetary Orbits, And The Hydrogen Atom

Section11.5: Atomic Spectra And The Bohr Theory Of Hydrogen

Problem 11.4QQ

See similar textbooks

Similar questions

What is the energy of the photon that, when absorbed by a hydrogen atom, could cause an electronic transition from the n = 2 state to the n = 5 state? Answer in units of eV. What energy could cause an electronic transition from the n = 5 state to the n = 8 state? Answer in units of eV.
A researcher observes hydrogen emitting photons of energy 1.89 eV. What are the quantum numbers of the two states involved in the transition that emits these photons?
What is the energy of the photon that, whenabsorbed by a hydrogen atom, could cause anelectronic transition from the n = 3 state tothe n = 5 state?Answer in units of eV. What energy could cause an electronic transition from the n = 5 state to the n = 7state?Answer in units of eV.
The hydrogen emission spectrum exhibits a line at 5.0010×10-19 J. If the final quantum state is n = 2, what is the initial quantum state of the transition corresponding to this line?
Consider photons incident on a hydrogen atom. (a) A transition from the n = 4 to the n = 7 excited-state requires the absorption of a photon of what minimum energy? eV(b) A transition from the n = 1 ground state to the n = 6 excited state requires the absorption of a photon of what minimum energy? eV
Consider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom (see Figures 6.7 and 6.10). (a) How many emission lines are possible, considering only the four quantum levels? (b) Photons of the lowest enerrgy are emitted in a transition from the level with n = _ _ _ _ to a level with n = _ _ _ _ (c) The emission line having the shortest wavelength corresponds to a transition from the level with n = _ _ _ _ to the level with n =
What is the energy of the photon that, when absorbed by a hydrogen atom, could cause an electronic transition from the n = 2 state to the n = 5 state? Answer in units of eV.
Consider only the transitions involving the first four energy levels for a hydrogen atom:a. How many emissions are possible for an electron in the n = 4 level as it goes tothe ground state?b. Which electronic transition is the lowest energy?c. Which electronic transition corresponds to the shortest wavelength emission
A hydrogen atom makes a transition from the n=3 level to the n=2 level. It then makes a transition from the n=2 level to the n=1 level. Which transition results in emission of the longest wavelengths photon?
what is the shortest wavelength of light that can be emitted by a hydrogen atom with initial configuration of 7d^1?
For what value of the principal quantum number n would the effective radius, as shown in a probability density dot plot for the hydrogen atom, be 1.0 mm? Assume that l has its maximum value of n - 1.