Question

An electron in the n=4 state of hydrogen makes a transition to the n=3 state, that is |4??〉 → |3??〉 . List the beginning and end i8states for the allowed transitions.

Answer #1

An electron in a hydrogen atom makes a transition from the n =
68 to the n = 4 energy state. Determine the wavelength of the
emitted photon (in nm).

An electron in a hydrogen atom makes a transition from the n = 7
to the n = 2 energy state. Determine the wavelength of the emitted
photon (in nm). Enter an integer.

An electron in hydrogen is in the 3d state.
What are the allowed transition(s) if the electron moves to a
higher energy state(s) (the photon carries one unit of angular
momentum)?

(1)
Part A: If a electron in a hydrogen atom makes a transition from
ground state to n = 8 level what wavelength of light in (nm) would
be needed for the abosorbed photon to cause the transition?
Part B: If the same electron falls to a lower level by emmitting
a photon of light in the Paschen series what is the frequncy of
light in (Hz) thats emitted?
(2) When a photon have a wavelength of 195nm strikes the...

Calculate the energy of a photon produced when an electron in
hydrogen makes a transition from an excited state in the 5th n=5
level, back to the ground state, n=1. Would you expect to see
radiation from this photon? Explain.

1. We can observe the wavelengths emitted from Hydrogen. When
Hydrogen electrons transition between states, they absorb or emit a
particle of light called a photon with energy E=hf. Here f is the
frequency of light and h is a constant.
a. How much energy does an electron in the n=1 (lowest-energy)
state of Hydrogen have? Repeat for n=2 and n=3.
b. How much energy is emitted if an electron in the n=3 state
transitions to the n=2 state?
c....

Determine the wavelength of the light absorbed when an electron
in a hydrogen atom makes a transition from an orbital in which
n = 2 to an orbital in which n =
5. Determine the wavelength of light emitted when an electron in
a hydrogen atom makes a transition from an orbital in n = 6 to an
orbital in n = 5.

An electron in He+ undergoes a transition from n = 4 to n = 2
state. Calculate the (a) energy in J, (b) frequency in Hz, (c)
wavelength in nm and (d) wave number in cm-1 of the photon
emitted.

calculate delta e for the n= 4 to the n=2 transition of an electron
in a hydrogen atom. Where on the electromagnetic spectrum would
this appear? what does the sign of this value mean?

Determine the end (final) value of n in a hydrogen atom
transition, if the electron starts in n = 2 and the atom absorbs a
photon of light with a frequency of 4.57 × 10 14 Hz. (This question
has already been posted, however, the answers for it dont match the
options).

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