Question

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?

Answer #1

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?

Q6] A hydrogen atom transitions from the ni = 5 state down to
the ground state. In the process it emits a photo of light. The
photon then strikes a photo-electric material with a work function
of Wo = 7.5eV . a) What is the wavelength of the photon emitted
from the transition of the hydrogen atom? b) What is the kinetic
energy of the electron ejected from the photo-electric
material?

(1)
Part A: If a electron in a hydrogen atom makes a transition from
ground state to n = 8 level what wavelength of light in (nm) would
be needed for the abosorbed photon to cause the transition?
Part B: If the same electron falls to a lower level by emmitting
a photon of light in the Paschen series what is the frequncy of
light in (Hz) thats emitted?
(2) When a photon have a wavelength of 195nm strikes the...

An electron in the n=6 level of the hydrogen atom relaxes to a
lower energy level, emitting light of λ=93.8nm. Find the principal
level to which the electron relaxed.

A. An electron emits a photon with an energy of 424 nm as it
relaxes to (n=2) what is the initial energy level of this
electron?
B. Is energy released or absorbed a result of this transition?
Briefly explain.
C. Calculate the wavelength (nm) of the electron having the
kinetic energy (K.E. = 1/2 mv^2) of the above transition 434
nm.
D. If an electron has the following three quantum number, n=2,
l= 1, m= 0, and m=-1/2. Briefly explain...

a ground state hydrogen atom absorbs a photon of light having a
wavelength of 93.73 nm. it then gives off a photon having a
wavelength of 410.1 nm. what is the final state of the hydrogen
atom?

(I) What is the full ground state electron configuration for a
neutral atom with ? = 22 protons?
(II) A hydrogen atom with a principal quantum number of ? =
4.
a. write all the possible values for the other quantum
numbers.
b. calculate the total number of possible quantum states that
can exist for this principal quantum state.
(III) An excited hydrogen atom is in the 6?1 state.
a. What is the principal quantum
number of the electron?
b....

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 ground state hydrogen atom absorbs a photon of light having a
wavelength of 92.57 nm. It then gives off a photon having a
wavelength of 954.3 nm. What is the final state of the hydrogen
atom? Values for physical constants can be found here.

A ground state hydrogen atom absorbs a photon of light having a
wavelength of 92.27 nm. It then gives off a photon having a
wavelength of 383.4 nm. What is the final state of the hydrogen
atom? Values for physical constants can be found here. nf=
please try to show solution

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