Question

Using the Rydberg formula, calculate the initial energy level
when an electron in a hydrogen atom transitions into n=2 and emits
a photon at 410.1 nm. Note: the Rydberg constant = 1.097 x
10^{7} m^{-1}

Answer #1

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?

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...

The electron in a hydrogen atom falls from an excited energy
level to the ground state in two steps, causing the emission of
photons with wavelengths of 656.5 nm and 121.6 nm (So the in the
first step the 656.5 nm photon is emitted and in the second step
the 121.6 nm photon is emitted). What is the principal quantum
number (ni) of the initial excited energy level from which the
electron falls?

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?

What is the emission wavelength for an electron falling from the
vacuum level (n=∞) to the lowest energy level in a hydrogen atom?
Use the Rydberg equation and the numerical values for the Rydberg
constant Rh given above. In which part of the
electromagnetic spectrum is this?
RH =2.17868891 x 10^–18 J = 1.09677759 x 107 m^–1

6.
a) For a hydrogen atom, if the emission energy associated when
the electron starts at n = 8 is 2.65 x 10-20 J, at what
energy level does the photon finish at?
b) What type of electromagnetic radiation is associated with
this change

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?

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...

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).

Q1)
Calculate the energy of an electron in the n =
2 level of a hydrogen atom.
Energy = _______Joules
Q2)
What would be the wavelength of radiation emitted from a
hydrogen atom when an electron moves from the n =
2 to n = 1energy level?
In what region of the spectrum does this radiation lie?
Wavelength = ________nm
Region = _________(ultraviolet or visible or infrared)

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 51 minutes ago

asked 51 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago