Question

An atom in a state with ? = 1 emits a photon with wavelenght 600 nm as it decays to a state with ? = 0. If the atom is placed in a magnetic field with magnitude B = 2.00 T, what are the shifts in the energy levels and in the wavelenght that result from the interaction between the atom’s orbital magnetic moment and the magnetic field

Answer #1

4 a) A hydrogen atom in the ground state absorbs a photon of
wavelength 97.2 nm. What energy level does the electron reach?
b) This excited atom then emits a photon of wavelength 1875.4
nm. What energy level does the electron fall to?

An atom absorbs a photon with wavelength 500 nm and subsequently
emits a photon with wavelength 660 nm.
a) Determine the energy absorbed by the atom.
b) Assume that the atom is a solid particle with mass 3.3×10−26
kg and is initially at rest. Determine the speed of the atom after
it has emitted the photon, assuming that any additional energy it
acquired only contributed to its motion.
Can you do part b step by step, which equations are
required?

An atom emits a photon (bundle) of light having wavelength 486
nm. What is the frequency of the light? What is the energy of the
photon?

A. An electron emits a photon with an energy of 424 nm as it
relaxes to (n=2) what is the initial energy level of this
electron?
B. Is energy released or absorbed a result of this transition?
Briefly explain.
C. Calculate the wavelength (nm) of the electron having the
kinetic energy (K.E. = 1/2 mv^2) of the above transition 434
nm.
D. If an electron has the following three quantum number, n=2,
l= 1, m= 0, and m=-1/2. Briefly explain...

An electron in an excited state
of a hydrogen atom emits two photons in succession, the first at
3037 nm and the second at 94.92 nm, to return to the ground state
(n=1). For a given transition, the wavelength of the emitted photon
corresponds to the difference in energy between the two energy
levels.
What were the principal quantum numbers of the initial and
intermediate excited states involved?

A hydrogen atom is in its third excited state. The atom emits a
1.88E+3nm wavelength photon. Determine the maximum possible orbital
angular momentum of the electron after emission. Express your
answer as multiples of hbar.

A hydrogen atom in the ground state absorbs a photon of
wavelength 95.0 nm.
What energy level does the electron reach?
This excited atom then emits a photon of wavelength 434.1 nm.
What energy level does the electron fall to?
-I know this question has already been asked on Chegg but each
question I go to has different calculations and I can't get the
right answer.

A hydrogen atom, initially in the 3s state, is placed in a
0.800-T magnetic field that points in the +z￼-direction. If the
atom emits a photon, what are the possible photon energies? What
are the initial and final ￼m_l values for the transition that
produces a photon with the shortest wavelength?

Originally, a H-atom is in an n=2 state.
a) After this atom absorbs a 77-nm photon, the electron is
ejected. The energy of the absorbed photon is....
b) The kinetic energy of the ejected electron is...

When N2* relaxes back to the ground state it emits a photon of
wavelength 470 nm, which makes up part of the aurora’s lights.
Calculate the energy difference between the MOs involved in the
transition.

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