Question

Exercise2

The absorption spectrum of an atom consists of the wavelengths 200nm, 300 nm, and 500nm.

a) Draw the atom's energy level diagram. Label each level with the energy and the principal quantum number.

b) What wavelengths are seen in the atom's emission spectrum?

Answer #1

The allowed energies of a simple atom are 0.00 eV, 4.21 eV , and
5.63 eV .
Part A
What wavelengths appear in the atom's emission spectrum?
Enter your answers in ascending order separated by commas.
Part B
What wavelengths appear in the atom's absorption spectrum?
Enter your answers in ascending order separated by commas.

The allowed energies of a simple atom are 0.00 eV, 3.73 eV , and
5.58 eV .
Part A
What wavelengths appear in the atom's emission spectrum?
Enter your answers in ascending order separated by commas.
Part B
What wavelengths appear in the atom's absorption spectrum?
Enter your answers in ascending order separated by commas.

The allowed energies
of a simple atom are 0.00 eV, 4.05 eV , and 5.12 eV .
Part
A
What wavelengths
appear in the atom's emission spectrum?
Enter your answers in
ascending order separated by commas.
Part
B
What wavelengths
appear in the atom's absorption spectrum?
Enter your answers in
ascending order separated by comma

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?

The hydrogen emission spectrum produces light at 430 nm (blue),
480 nm (blue-green) and 650 nm (red).
Find the energy in Joules and then in eV for a photon at each of
these wavelengths:
430 nm:
480 nm:
650 nm:
A metal surface has a work function (W0) of 2.7
eV. Of the three wavelengths of light in the hydrogen
spectrum, which would be able to release electrons from the metal
surface?
Calculate the kinetic energy in eV if any, of...

An electron in a hydrogen atom relaxes to the ground state while
emitting a 93.8 nm photon.
a. Is this light visible? In what region of the electromagnetic
spectrum does it lie?
b. What was the initial principal quantum number, ni, of the
electron undergoing the transition?

The microwave spectrum of the 12C16O molecule consists of a
series of lines separated by 3.913 cm−1. Draw the corresponding
energy level diagram for this spectral line spacing for the first 5
energy levels, assuming the rigid rotor model. Give the value for
the energy gap between each level.

An excited hydrogen atom emits light with a wavelength of 397.2
nm to reach the
energy level for which n = 2. In which principal quantum level did
the electron
begin? (c = 3.00 x 108 m/s, h = 6.63 x 10-34 J•s, RH = 2.18 x
10-18J).

A hydrogen atom at rest is initially in an excited state
corresponding to n = 5.
a- Give the quantum numbers (l) and (m) which correspond to n =
5
b- What is the ionization energy of the atom in this state?
c- What is the frequency of the photon emitted when it returns
to its ground state n = 1?
d- Estimate the momentum and the kinetic energy of the atom's
recoil during the photon emission.
mH= 1.007825? 1?...

A) Sketch a separate diagram for the energy levels of the
electron in the Hydrogen atom – The diagram should be to scale.
Annotate the diagram with the ground state energy E0, the principal
quantum number n, and the ionization energy of the atom (13.6
eV).
B) It is known that a certain hydrogen atom has n=5 and m=2. How
many different states are consistent with this information?
C) Answer the same question (in terms of n and m) for...

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