Calculate the probability of an electron in the ground state of
the hydrogen atom being inside a sphere radius r = 2.40 ✕
10-14 m, centered around the nucleus. (Hint: Note that
r << a0.)
The
hydrogen atom electron is in the ground state. The electron absorbs
energy and makes a transition to the n=3 state. Then it returns to
the ground state by emitting two photons when going to n=2 and then
n=1 states.
A. What are the wavelengths of these photons?
B. What will be the wavelength if only one photon is
emitted?
C. What is the maximum number of electrons with ml=3 in the
shell with n=5?
D. How many electrons with...
Consider a hydrogen atom in the ground state. What is the energy
of its electron?
E= J
Consider a hydrogen atom in an excited state of 2s^1. What is
the energy of its electron?
E= J
An electron in a hydrogen atom is excited from the n = 1 ground state to the n = 4 excited state. Classify the statements about this absorption and emission process as true or false. True On average, the electron is closer to the nucleus in the n = 4 state than in the n = 1 state. The wavelength of light absorbed when the electron is excited from the ground state to n = 4 is the same as the wavelength of...
A hydrogen atom is in the ground state. It absorbs energy and
makes a transition to the n = 5 excited state. The atom returns to
the ground state by emitting two photons, one in dropping to n = 4
state, and one in further dropping to the ground state. What are
the photon wavelengths of (a) the first and (b) the second
transitions?
a hydrogen atom in the ground state absorbs a photon
of light with a wavelength of 97.3nm causing the electron to jump
to an unknown energy level. the electron then relaxes emitting a
photon of light in the visible range, what is the wavelength of the
emitted photon?
Which is not a valid quantum number for a ground state electron on
an atom of germanium?
a) n=2 l=1 ml=0 ms=+1/2
b) n=4 l=3 ml=-2 ms=-1/2
c) n=4 l=1 ml=-1 ms=+1/2
d) n=3 l=0 ml=0 ms=+1/2
e) n=3 l=2 ml=1 ms=-1/2
a) Find the energy of an electron in the n=5 state of the hydrogen atom. b) Find the energy of an electron in the n=6 state of the hydrogen atom. c) If an electron initially in the n= 6 state falls to the n= 5 state, how much energy must the electron give up? d) If an electron initially in the n= 6 state falls to the n=5 state, what is the wavelength of the photon that will be emitted?
An electron (in a hydrogen atom) in the n=5 state drops
to the n=2 state by undergoing two successive
downward jumps. What are all possible combinations of the resulting
photon wavelengths?