Question

The first four energy levels for an atom are:

E_{1} = -8.57 eV E_{2} = -2.14
eV E_{3} = -0.95 eV E_{4} = -0.54
eV

An electron with a kinetic energy of 7.74 eV collides with an electron in its ground state. After the collision, the atom is in an excited state and the electron is scattered. The kinetic energy of the scattered electron could be

I have been struggling with this question, help asap would be highly appreciated. Thank you :)))

Answer #1

Solution in the uploaded imag

Consider the first three energy levels of hydrogen (n = 1, 2,
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E2, and E3.
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Consider the following energy levels of a hypothetical
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E4 −1.51 ×
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E3 −5.11 ×
10−19 J
E2 −1.15 ×
10−18 J
E1 −1.85 ×
10−18 J
(a) What is the wavelength of the photon needed to
excite an electron from E1
to E4? (in
m)
(b) What is the energy (in joules) a photon must have in
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(c) When an electron drops from the
E3 level to the...

A. Consider a hydrogen atom with one electron and quantized
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2) For each spectral line, identify what part of the
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II(20pts). Short Problems
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