Question

Equation 37-14b in the textbook gives the energy emitted by
Hydrogen when electrons transition between states
(E_{n}=-(13.6 eV) Z^{2}/n^{2},
n=1,2,3,...). When they do so, they absorb or emit a particle of
light called a photon with energy E=hf. Here f is the frequency of
light and h is a constant.

b) How much energy is emitted if an electron in the n=3 state transitions to the n=2 state?

Answer #1

1. We can observe the wavelengths emitted from Hydrogen. When
Hydrogen electrons transition between states, they absorb or emit a
particle of light called a photon with energy E=hf. Here f is the
frequency of light and h is a constant.
a. How much energy does an electron in the n=1 (lowest-energy)
state of Hydrogen have? Repeat for n=2 and n=3.
b. How much energy is emitted if an electron in the n=3 state
transitions to the n=2 state?
c....

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?

(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...

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...

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?

Calculate the wavelength corresponding to a transition of
electrons from the n = 6 energy level to the n = 3 level in a B4+
ion. (Use En= -R(z2/n2))
Using your answer from the question above what is the speed that
an electron would need to travel in order to display the same
wavelength?

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.

Calculate the energy of a photon produced when an electron in
hydrogen makes a transition from an excited state in the 5th n=5
level, back to the ground state, n=1. Would you expect to see
radiation from this photon? Explain.

5a) Positronium is a bound state of an electron and a positron.
What is the energy of the photon emitted in transitions of
positronium from the first excited state to the ground state? (A)
1.7 eV , (B) 5.1 eV , (C) 6.8 eV , (D) 13.6 eV, (E) 20.4 eV
5b) A new hydrogen-like atom is discovered where the particle
orbiting the proton has mass 2me and charge 2e, where me and e are
the mass and charge of...

Consider the first three energy levels of hydrogen (n = 1, 2,
3).
a) What photon energies can be observed from transitions between
these levels? Label these in increasing order as E1,
E2, and E3.
b) A hydrogen atom which is initially in the n = 2 level
collides with an aluminum atom in its ground state (the kinetic
energy of the collision is nearly zero). The hydrogen can drop to
the n = 1 level and ionize the aluminum...

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