Calculate the energy spectrum of the n=2 states of the hydrogen
atom including the fine structure...
Calculate the energy spectrum of the n=2 states of the hydrogen
atom including the fine structure correction. How is this spectrum
changed when the atoms is placed in an external magnetic field of
2.5 Tesla?
The following is a diagram of energy states and transitions in the hydrogen atom.Match each of the responses below with the correct arrow from the figure. 1.) The emission line with the shortest wavelength. 2.) The absorption line with the longest wavelength. 3.) The emission line with the highest energy. 4.) The absorption line with the lowest energy. 5.) The emission line with the highest frequency. 6.) The line corresponding to the ionization energy of hydrogen.
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?
14: An electron in hydrogen atom at the energy level n = 7
undergo a transition to level n = 3: Find the frequency and the
energy of the emitted photon.
15: An electron jumps from higher energy level to the first
energy level with an energy difference of 2.04375 x
10-18 J. find the initial energy level. Show your
calculations,
16: A: What will be the speed of an electron at 4 th energy
level? Suppose the electron has...
An electron in a Hydrogen atom originally at n=5
energy level absorbs a photon with a frequency of 6.54×10^13 and
then proceeds to emit another photon with a frequency of
2.98×10^14. To what energy level does the electron move?
Calculate the energy (J) of the photon emitted when an electron
in the hydrogen atom falls from n=5 to n=2 .
Use 2.178 x 10-18 J for the constant in the Bohr
equation.
Answer should be in scientific notation, e.g.
3000 = 3E3
I have no idea how to get this problem help me!!
Suppose a photon is absorbed by the electron in a hydrogen atom
in an n= 2 state. What wavelength should the photon have to enable
the electron to transition to the n= 4
state? Once the photon is absorbed, what are the various
wavelengths of photons that could be emitted by the atom? (Use Bohr
approximation).
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?
The allowed energy levels of the hydrogen atom are described by
the following expression:
En=−2.17868×10^−18J(1/ n^2)
where n is the quantum number of the energy level. The Balmer
series that is observed in the line spectrum of hydrogen
corresponds to transitions that end in the n = 2 level. Determine
the wavelengths of the first 5 lines in the Balmer series.
The visible emission spectrum of hydrogen involves a transition
to n final = 2. What is initial for the line of the emission
spectrum at 434 nm? a. 5 b. 6 c. 4 d. 3 e. 7
An Electron initially in the n=2 state of a hydrogen atom is
excited by a photon to the n=5 state.
a. What is the energy of the excitatoin photon?
b. As the atom relaxes, the electron transitions to the ground
state. What is the energy of the photon released during the
electron transition?
c. What is the frequency of the released photon?
d. What is the name of the scientist who first modeled the atom
as a miniature solar system?