Question

What is the energy of the photon that, when absorbed by a hydrogen atom, could cause the following?

(a) an electronic transition from the *n* = 2 state to
the *n* = 5 state

eV

(b) an electronic transition from the *n* = 5 state to the
*n* = 7 state

eV

Answer #1

1. What is the energy in eV and wavelength in µm of a photon
that, when absorbed by a hydrogen atom, could cause a transition
from the n= 4 to the n= 8
energy level?
a) energy in eV
b) wavelength in µm
2. The so-called Lyman-αphoton is the lowest energy photon in
the Lyman series of hydrogen and results from an electron
transitioning from the n= 2 to the n= 1 energy level. Determine the
energy in eV and...

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?

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...

A photon with an energy of 10.2eV is absorbed by a
hydrogen atom traveling in the opposite direction with a speed of
1000 m/s.
a) What is the energy in Joules of the
photon?
b) What is the wavelength, frequency and speed of the
photon
c) What is the momentum of the photon?
What is the speed of the atom after the photon is
absorbed

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...

Exercise: Consider the Bohr Theory Hydrogen atom. a) how much
energy is needed to cause a transition of an electron from the 2nd
excited state to the 3rd excited state? Remember the 2nd excited
state corresponds to n=3, etc). b) what wavelength photon just has
enough energy to initiate the transition?

Which is greater: The energy of a
photon emitted from a hydrogen atom when the electron makes a
transition from the n = 3 to the n = 1 energy
level, or
• the kinetic energy of a 2 gram Ping-Pong ball moving with a
speed of 1 m per hour?

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.

A hydrogen atom is in its ground state
(ni = 1)
when a photon impinges upon it.
The atom absorbs the photon, which has precisely the energy
required to raise the atom to the
nf = 3
state.
(a)
What was the photon's energy (in eV)?
eV
(b)
Later, the atom returns to the ground state, emitting one or
more photons in the process. Which of the following energies
describes photons that might be emitted thus? (Select all that
apply.)...

Answer the following questions using the Bohr model of the
hydrogen atom.
a) A hydrogen atom is the n = 3 excited state when its electron
absorbs a photon of energy 4.40 eV. Draw a diagram roughly to
scale, of relevant energy levels for this situation. Make sure to
show and label the initial energy of the H atom in the n=3 state,
the energy level at which this atom loses its electron, and kinetic
energy of the electron.
b)What...

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