Question

A photon is emitted when an electron transitions to a lower
energy level. If the emitted radiation has a wavelength of
2.1x10^{-11}m, find the energy (in eV) and the momentum (in
kgm/s) of the photon. What type of electromagnetic radiation is
this? Please show all work and equations used.

Answer #1

What is the wavelength of the photon emitted as the electron in
the hydrogen atom transitions from the 3rd to 2nd level? What is
the frequency of the photon and what is the energy carried by the
photon?
got -6606 A for the first one and I'm not sure if I'm doing it
right

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?

Light is emitted from a hydrogen atom as an electron in the atom
jump from the n=9 orbit to the n=3 orbit.
What is the energy of the emitted photon in eV?
(b) What are the frequency and wavelength of the photon?
(c) In which frequency range (UV, visible, IR) is the emitted
electromagnetic radiation? Justify your answer.

4. [15] Light is emitted from a hydrogen atom as an electron in
the atom jump from the n=9 orbit
to the n=3 orbit.
(a) [7] What is the energy of the emitted photon in eV?
(b) [4] What are the frequency and wavelength of the photon?
(c) [4] In which frequency range (UV, visible, IR) is the
emitted electromagnetic radiation?
Justify your answer.

The best answer for the wavelength of light emitted when an
electron transitions from the fourth energy level to the first
energy level in a hydrogen atom is:
a. 97.2 nm
b 972 nm
c. 9.72 nm
d. 9720 nm
e. .972 nm

Calculate the wavelength of a photon emitted when the electron
in a Li2+ ion relaxes from the n=8 energy level to the n=4 energy
level. (Use Bohr's model of the atom.)

Calculate the wavelength (in nanometers) of a photon emitted by
a hydrogen atom when its electron drops from the n = 4 to n = 2
state.
Consider the following energy levels of a hypothetical
atom:
E4 −1.61 ×
10−19 J
E3 −7.51 ×
10−19 J
E2 −1.35 ×
10−18 J
E1 −1.45 ×
10−18 J
(a) What is the wavelength of the photon needed to
excite an electron from E1
to E4?
____ ×10m
(b) What is the energy...

A photon is emitted from a hydrogen atom when an electron goes
from the n = 6 to the n = 2 state. What kind of electromagnetic
radiation is this? Select one:
a. Visible Light
b. Ultraviolet Light
c. Infrared Radiation
d. X-Ray Radiation
e. Microwave Radiation

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?

We can observe the differences in energy levels by observing the
light that is emitted when atoms are heated. When atoms are heated,
the electrons can jump up to a higher energy level. When one
electron falls back down to a lower energy level, a single photon
of light is emitted with an energy equal to the difference in
energy of the two levels. We call this atomic emission
spectroscopy. If an electron in an atom jumps from the n...

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