Question

1. What is the energy in eV and wavelength in µm of a photon
that, when absorbed by a hydrogen atom, could cause a transition
from the * n*= 4 to the

a) energy in eV

b) wavelength in µm

2. The so-called Lyman-αphoton is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n= 2 to the n= 1 energy level. Determine the energy in eV and the wavelength in nm of a Lyman-αphoton.

a) the energy in eV

b) the wavelength in nm

Answer #1

What is the energy of the photon that, when absorbed by a
hydrogen atom, could cause the following?
(a) an electronic transition from the n = 2 state to
the n = 5 state
eV
(b) an electronic transition from the n = 5 state to the
n = 7 state
eV

For a hydrogen atom, calculate the wavelength of an emitted
photon in the Lyman series that results from the transition n = 3
to n = 1. The Rydberg constant is 2.18 x 10^-18 J.

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?

(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...

Consider the electronic transition from n = 4 to n = 1 in a
hydrogen atom, and select the correct statement below: A photon of
97 nm wavelength and 2.05x10-18 J energy was emitted from the
hydrogen atom in this electronic transition. A photon of 97 nm
wavelength and 2.05x10-18 J energy was absorbed by the hydrogen
atom in this electronic transition. A photon of 122 nm wavelength
and 1.64x10-18 J energy was emitted from the hydrogen atom in this...

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).

a) What is the energy of a photon (in eV) that has a wavelength
of 466 nm? (3 digit answer)
b) What is the energy (in eV) of a photon that has a wavelength
of 460 nm?
c) What is the wavelength of a photon that has 2.1 eV of kinetic
energy? (format of a.b x 10-c m )
d) a photoelectric surface has a work function of 2.00 eV. What
is the threshold frequency of this surface? (format of
a.bc...

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?

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...

Calculate the energy of the emitted photon as well as the
wavelength and frequency of electromagnetic radiation emitted from
the hydrogen atom when the electron undergoes the transition from n
= 5 to n = 1. In what region of the spectrum does this line
occur?

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