Question

7) Calculate the energy of the photon emitted when a hydrogen atom undergoes a spin-flip transition. How many such photons would it take to equal the energy of a single photon of wavelength 656.3 nm emitted by hydrogen (level 3 – level 2 transition)?

8) Suppose you discovered a star made purely of hydrogen and helium. How old do you think it would be? Explain your reasoning.

Answer #1

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...

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?

An electron in a hydrogen atom makes a transition from the n = 7
to the n = 2 energy state. Determine the wavelength of the emitted
photon (in nm). Enter an integer.

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?

An electron in a hydrogen atom undergoes a transition from the n
= 6 level to some lower energy level. In doing so, energy is
released in the form of light. a) Calculate the frequency in s-1
(to 3 significant figures) of a photon of light associated with the
highest frequency transition (i.e. largest difference in frequency)
possible from the n = 6 to a lower level. (HINT: Try drawing a
picture first…) b) Calculate the wavelength (in nm) of...

A hydrogen atom undergoes a transition from n = 5 to n = 2.
Considering the fact that it may go through intermediate steps
between 5 and 2 (for example, 5 → 3 → 2),
a) what is the shortest possible wavelength for emitted
photons?
b) what is the longest possible wavelength for emitted
photons?

Which is greater: The energy of a
photon emitted from a hydrogen atom when the electron makes a
transition from the n = 3 to the n = 1 energy
level, or
• the kinetic energy of a 2 gram Ping-Pong ball moving with a
speed of 1 m per hour?

An electron in a hydrogen atom makes a transition from the n =
68 to the n = 4 energy state. Determine the wavelength of the
emitted photon (in nm).

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.

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

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