Question

A hydrogen atom is in its third excited state. The atom emits a 1.88E+3nm wavelength photon. Determine the maximum possible orbital angular momentum of the electron after emission. Express your answer as multiples of hbar.

Answer #1

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 (Z = 1) is in the third excited state, and a
photon is either emitted or absorbed. Determine
(a) the quantum number nf of the final state
(b) the energy of the photon when the photon is emitted with the
shortest possible wavelength
(c) the quantum number nf of the final state
(d) the energy of the photon when the photon is emitted with the
longest possible wavelength
(e) the quantum number nf of the final state...

4 a) A hydrogen atom in the ground state absorbs a photon of
wavelength 97.2 nm. What energy level does the electron reach?
b) This excited atom then emits a photon of wavelength 1875.4
nm. What energy level does the electron fall to?

A hydrogen atom in the ground state absorbs a photon of
wavelength 95.0 nm.
What energy level does the electron reach?
This excited atom then emits a photon of wavelength 434.1 nm.
What energy level does the electron fall to?
-I know this question has already been asked on Chegg but each
question I go to has different calculations and I can't get the
right answer.

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...

Suppose that an electron is in an excited state of a Hydrogen
atom at the n = 4 energy level. (a) How
many different states are available for that electron to
occupy?(b) Suppose that the electron falls
directly to the ground state, causing a single photon to be
released from the atom. What is the photon’s wavelength?
(c) After its release, the photon collides with an
electron at rest, and scatters off at a 60o angle with
respect to its...

Suppose that an electron is in an excited state of a Hydrogen
atom at the n = 4 energy level.
(a) How many different states are available for
that electron to occupy?
(b) Suppose that the
electron falls directly to the ground state, causing a single
photon to be released from the atom. What is the photon’s
wavelength?
(c) After its
release, the photon collides with an electron at rest, and scatters
off at a 60o angle with respect to...

A hydrogen atom stays in the 3rd excited state (n = 4). Consider
of the quantum behavior of the electron, but ignore the quantum
behavior of the nucleus. (a) What are the possible values for the
quantum number l and what are the corresponding orbitals? Write
down the magnitude of each orbital angular momentum (in units of
ħ). (b) For each value of l, what are possible values for the
quantum number ml and the magnitude of the z component...

a) Determine the maximum wavelength of the photon that hydrogen
in the excited state ni = 4 can absorb. The energy of the ground
state of hydrogen is −13.6 eV, the speed of light is 2.99792 × 10^8
m/s and Planck’s constant is 6.62607 × 10^−34 J · s. Answer in
units of nm.
b) What would be the next smaller wavelength that would work?
Answer in units of nm.?

The electron in a hydrogen atom is excited to the n = 6 shell
and emits electromagnetic radiation when returning to lower energy
levels. Determine the number of spectral lines that could appear
when this electron returns to the lower energy levels, as well as
the wavelength range in nanometers.

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