Model an atom as an electron in a rigid box of length , roughly twice the Bohr radius.
a. What are the four lowest energy levels of the electron?
b. Calculate all the wavelengths that would be seen in the emission spectrum of this atom due to quantum jumps between these four energy levels. Give each wavelength a label to indicate the transition.
c. Are these wavelengths in the infrared, visible, or ultraviolet portion of the spectrum?
d. The stationary states of the Bohr hydrogen atom have negative energies. The stationary states of this model of the atom have positive energies. Is this a physically significant difference? Explain.
e. Compare this model of an atom to the Bohr hydrogen atom. In what ways are the two models similar? Other than the signs of the energy levels, in what ways are they different?
We have given,
The box length =
We have to calculate the four energy levels of the electron.
The energy of the one dimensional box is given by,
Then, energy level, n
Foe ground sate,
We have to plot the transition levels diagram.
We have to find there wavelengths.
Since we know that,
yes, there are in the range of ultraviolet.
We have to find the physical significance of the positive energy.
There is not have any physical significance.
Because model is correct as found energy is also in same pattern as in the Bohr's hydrogen atom.
We have to find the difference between the one dimensional box and the Bohr hydrogen atom.
There is just one different due to electron motion.
The motion of electron in hydrogen atom is circular about the nucleus.
But in the one dimensional box it is moving too and fro translational motion.
Consider a quantum harmonic oscillator.
a. What happens to the spacing between the nodes of the wave function as |x| increases? Why?
b. What happens to the heights of the antinodes of the wave function as |x| increases? Why?
c. Sketch a reasonably accurate graph of the n=8 wave function of a quantum harmonic oscillator.
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