Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
Chapter 07
Quantum Theory and the Electronic Structure of Atoms
1.
In the following diagram of a wave
2. Which of the following wavelengths of electromagnetic radiation has the highest energy?
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
Topic: Quantum Theory and Atomic Structure
4.
Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10-3 m.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
5.
Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10-1 m.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
6.
Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10-16 J/photon.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
7.
Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10-18 J/photon.
8. What is the wavelength of radiation that has a frequency of 5.39 1014 s–1? (c = 2.9979
108 m/s)
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
9. What is the wavelength of radiation that has a frequency of 3.4 x 1011 s –1?
10. Calculate the frequency of visible light having a wavelength of 486 nm.
11. Calculate the frequency of visible light having a wavelength of 686 nm.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
Topic: Quantum Theory and Atomic Structure
12. What is the energy in joules of one photon of microwave radiation with a wavelength
0.122 m? (c = 2.9979 108 m/s; h = 6.626 10–34 Js)
13. What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120
nm?
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
14. What is the energy in joules of a mole of photons associated with visible light of
wavelength 486 nm?
15. What is the energy in joules of a mole of photons associated with red light of wavelength
7.00 102 nm?
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
16. What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold
frequency for photoelectrons is 2.50 1014 /s?
17. Calculate the energy, in joules, required to excite a hydrogen atom by causing an
electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy
levels of the H atom are given by
En = –2.18 10–18 J(1/n2)
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
18. Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its
electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels
of the H atom are given by
En = –2.18 10–18 J(1/n2)
19. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its
electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = –2.18
10–18 J(1/n2).
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
20. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its
electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = –2.18
10 –18 J(1/n2).
21. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its
electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = –2.18
10–18 J(1/n2).
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
22. The second line of the Balmer series occurs at a wavelength of 486.1 nm. What is the
energy difference between the initial and final levels of the hydrogen atom in this emission
process?
23. A proton is roughly 1800 times more massive than an electron. If a proton and an electron
are traveling at the same speed,
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
24. A proton is roughly 1800 times more massive than an electron. If a proton and an electron
have the same kinetic energy,
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
25. If a hydrogen atom and a helium atom are traveling at the same speed,
26. If a hydrogen atom and a helium atom have the same kinetic energy,
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
27. In an electron microscope, electrons are accelerated to great velocities. Calculate the
wavelength of an electron traveling with a velocity of 7.0 103 kilometers per second. The
mass of an electron is 9.1 10–28 g.
28. Calculate the wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 105
m/s. The atomic mass of 20Ne is 19.992 amu.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
29. Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a
neutron = 1.675 10–24 g)
30.
A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If
DH for the reaction Cl2(g) → 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine
atoms in solution?
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
Topic: Quantum Theory and Atomic Structure
31. The longest wavelength of light that causes electrons to be ejected from the surface of a
copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of
wavelength 200. nm shines on a copper plate?
32. When photons with a wavelength of 310. nm strike a magnesium plate, the maximum
velocity of the ejected electrons is 3.45 105 m/s. Calculate the binding energy of electrons to
the magnesium surface.
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
33. Electrons can be used to probe the arrangement of atoms on a solid surface if the
wavelength of the electrons is comparable with the spacing between the atoms. Which of the
following electron velocities would be appropriate for use in this application if the atoms are
separated by 0.320 nm?
34. A single pulse of a laser yields an average of 5.00 1018 photons with l= 633 nm. If
melting ice to water at 0C requires 6.01 kJ/mol, what is the fewest number of laser pulses
needed to melt 10.0 g of ice?
Chapter 07 – Quantum Theory and the Electronic Structure of Atoms
35.
Which one of the following sets of quantum numbers is not possible?