Question

An electron in a hydrogen atom undergoes a transition from the n = 6 level to some lower energy level. In doing so, energy is released in the form of light. a) Calculate the frequency in s-1 (to 3 significant figures) of a photon of light associated with the highest frequency transition (i.e. largest difference in frequency) possible from the n = 6 to a lower level. (HINT: Try drawing a picture first…) b) Calculate the wavelength (in nm) of this photon of light

Answer #1

(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...

An electron in a hydrogen atom makes a transition from the n =
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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.

Consider the electronic transition from n = 4 to n = 1 in a
hydrogen atom, and select the correct statement below: A photon of
97 nm wavelength and 2.05x10-18 J energy was emitted from the
hydrogen atom in this electronic transition. A photon of 97 nm
wavelength and 2.05x10-18 J energy was absorbed by the hydrogen
atom in this electronic transition. A photon of 122 nm wavelength
and 1.64x10-18 J energy was emitted from the hydrogen atom in this...

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.

1) An electron in the hydrogen atom drops from the n=5 level to
the n=1 level. What are the frequency, wavelength, and energy of
the emitted photon? In which series does this photon occur? How
much energy must be absorbed by the atom in order to kick the
electron back up to the fifth level?
2) Calculate the maximum wavelength for the initiation of a
photoelectric current in the aluminum (work function W = 4.28
eV).

7) Calculate the energy of the photon emitted when a hydrogen
atom undergoes a spin-flip transition. How many such photons would
it take to equal the energy of a single photon of wavelength 656.3
nm emitted by hydrogen (level 3 – level 2 transition)?
8) Suppose you discovered a star made purely of hydrogen and
helium. How old do you think it would be? Explain your
reasoning.

A hydrogen atom transitions from the n = 6 excited state to the
n = 3 excited state, emitting a photon.
a) What is the energy, in electron volts, of the electron in the
n = 6 state? How far from the nucleus is the electron?
b) What is the energy, in electron volts, of the photon emitted
by the hydrogen atom? What is the wavelength of this photon?
c) How many different possible photons could the n = 6...

1. a. A photon is absorbed by a hydrogen atom causing an
electron to become excited (nf = 6) from the ground state electron
configuration. What is the energy change of the electron associated
with this transition?
b. After some time in the excited state, the electron falls from
the n = 6 state back to its ground state. What is the change in
energy of the electron associated with this transition?
c. When the electron returns from its excited...

1. The energy of the electron in the lowest level of the
hydrogen atom (n=1) is -2.179×10-18 J. What is the energy of the
electron in level n=5? -8.716×10-20 J 2.The electron in a hydrogen
atom moves from level n=6 to level n=4.
a) Is a photon emitted or absorbed?
b) What is the wavelength of the photon?

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