Question

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?

Answer #1

) Describe the Bohr theory of the hydrogen atom and how it
explains the line spectrum of hydrogen. What is the
energy and wavelength of the
photon of energy that was emitted by hydrogen if one of its
electrons dropped from the n=6 state to the n=2 state. In what
region of the electromagnetic spectrum does this wavelength fall?
Which color line is this in the line spectra of hydrogen?

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...

I want you to compare particle in a box with the Bohr atom. For
the particle in the box you can assume the size is .5x10^-10 m and
the particle that is trapped is an electron. For the Bohr atom
consider a hydrogen atom.
a.) What is the energy of photon emitted when the electron drops
from 3->2 and 2->1 in the particle in a box?
b.) What is the energy of photon emitted when the electron drops
from 3->2...

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?

A hydrogen atom is in its ground state (n = 1). Using the Bohr
theory of the atom, calculate (a) the radius of the orbit. (b) the
velocity of the electron where vn = ?(kee2)/(mern) . (c) the
kinetic energy of the electron (d) the static electric potential
energy of the electron. (e) the total energy of the electron. (e)
the energy gained by moving to a state where n = 5. (g) the
wavelength, ?, of the EM waved...

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. 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?

Let's use the Bohr model equations to explore some properties of
the hydrogen atom. We will determine the kinetic, potential, and
total energies of the hydrogen atom in the n=2 state, and find the
wavelength of the photon emitted in the transition n=2?n=1.
Find the wavelength for the transition n=3 ?
n=2 for singly ionized helium, which has one electron and
a nuclear charge of 2e. (Note that the value of the
Rydberg constant is four times as great as...

Explain why a hydrogen atom with its electron in the ground
state cannot absorb a photon of just any energy when making a
transition to the second excited state (n = 3).

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