Question

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).

Answer #1

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...

(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...

a. what is the energy of the emitted photon if an electron in
the hydrogen atom makes a transition from the n=7 state to the n=2
state?
b. Now, Imagine there is a photon with the same wavelength. What
is the speed of this photon?

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 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...

A hydrogen atom (Z=1) is in the third excited state. It makes a
transition to a different state, and a photon is either emitted or
absorbed. Answer the following conceptual questions:
What is the quantum number of the third excited state?
When an atom emits a photon, is the final quantum number of the
atom greater than or less than the initial quantum number?
When an atom absorbs a photon, is the final quantum number of
the atom greater than...

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...

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?

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...

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