1. Thanks to: Dr. P. Bertrand Oak Ridge HS
Modern Physics
Thanks to:
Dr. P. Bertrand
Oak Ridge HS

2. Quantum Physics Physics on a very small (atomic) scale is “quantized”.
Quantized phenomena are discontinuous and discrete, and generally very small.
Quantized energy can be throught of an existing in packets of energy of specific size.
Atoms can absorb and emit quanta of energy, but the energy intervals are very tiny, and not all energy levels are “allowed” for a given atom.

3. Electromagnetic Spectrum

4. Light is a ray
We know from geometric optics that light behaves as a ray; it travels in a straight line.
When we study ray optics, we ignore the nature light, and focus on how it behaves when it hits a boundary and reflects or refracts at that boundary.

5. But light is also a wave!
We studied this earlier in the year and we will use this equation again here.
C = f l
C: 3 x 108 m/s (speed of light in a vacuum)
f: frequency (Hz or s-1)
l: wavelength (m) (distance from crest to crest)

6. In quantum physics, we focus on how light behaves as a particle!
Light has a dual nature. In addition to behaving as a wave, it also behaves as a particle.
It has energy and momentum, just like particles do. Particle behavior is pronounced on a very small level, or at very high light energies.
A particle of light is called a “photon”.

7. Calculating photon energy
The energy of a photon is calculated from the frequency of the light.
E = hf = hc / l because c = f l
E = nhf (for multiple n # of photons)
E: energy (J or eV)
h: Planck’s constant
6.625 x J s (SI system)
4.14 x eV s (convenient)
f: frequency of light (s-1, Hz)

8. Checkpoint
Which has more energy in its photons, a very bright, powerful red laser or a small key-ring red laser?
Neither! They both have the same energy per photon; the big one has more power.
Which has more energy in its photons, a red laser of a green laser?
The green one has shorter wavelength and higher frequency. It has more energy per photon.

9. Quantum Double-Slit Experiment
Dr. Quantum
Einstein – History Channel

10. The “electron volt” (eV)
The electron volt is the most useful unit on the atomic level.
If a moving electron is stopped by 1 V of electric potential, we say it has 1 electron volt (or 1 eV) of kinetic energy.
1 eV = x J

11. Sample Problem
What is the frequency and wavelength of a photon whose energy is
4.0 x J?
E = hf
f = E/h =
c = f l
l = c/f =

12. Sample Problem
The bonding energy of H2 is kcal/mol. Determine the frequency and wavelength of a photon that could split one atom of H2 into two separate atoms. (1 kcal = 4l86 J).
E = (104.2 kcal)(4186 J)( mol )
mol kcal x10 23mol’cls
E = 7.24 x J = hf
f = 7.24 x J/ x 10-34Js
f = 1.09 x 1015 Hz ***

13. Atomic Transitions
How many photons are emitted per second by a He-Ne laser that emits 3.0 mW of power at a wavelength of nm?
P = Etot /t E = hf  P = n(hf)/t
c = f l f = c/ l
P = nh(c/ l) n = (P)(t)( l )
t (c)(h)

14. Solution Find total energy in one second from power
P = W/t = E tot / t
E tot = Pt = 3.0 x J
Now see how many photons, n, will produce this energy
E = hf (one photon)
E tot = nhf (for n photons)
E = nhc/ l (since wavelength is given and not frequency)
3.0x10-3 = n (6.625x10-34Js)(3.0x108m/s)/632.8x10-9m
n = 9.55 x 1016

15. General Info re the Atom
Atoms are composed of
Nuclei (protons and neutrons) and electrons
When an atom encounters a photon
It usually ignores the photon, but sometimes absorbs the photon
If an atom absorbs a photon
The photon disappears and gives all its energy to the atom’s electrons

16. Quantized atomic energy levels
*This graph shows
allowed quantized
energy levels in a
hypothetical atom.
*The more stable states
are those in which the
atom has lower energy.
*The more negative the
state, the more stable
the atom.

17. Quantized atomic energy levels
The highest allowed
energy is 0.0 eV. Above
this level, the atom loses
its electron, This level is
called the ionization or
dissociation level.
The lowest allowed energy
is called the ground state.
This is where the atom is
most stable.
States between the highest
and lowest state are called
excited states.

18. Transitions of the
electron within the
atom must occur from
one allowed energy
level to another.
The atom CANNOT
EXIST between
energy levels.

19. Absorption of photon by atom
When a photon of light is absorbed by an atom, it causes an increase in the energy of the atom.
The photon disappears.
The energy of the atom increases by exactly the amount of energy contained in the photon.
The photon can be absorbed ONLY if it can produce an “allowed” energy increase in the atom.

20. Absorption of photon by atom
When a photon is
absorbed, it
excites the atom
to higher quantum
energy state.
The increase in
energy of the atom
is given by DE = hf.
Ground state

21. Absorption Spectrum
When an atom absorbs photons, it removes the photons from the white light striking the atom, resulting in dark bands in the spectrum.
Therefore, a spectrum with dark bands in it is called an absorption spectrum.
Absorption spectrum seen through hand held spectroscope

22. Absorption Spectrum Absorption spectra always involve atoms going
up in energy
level.

23. Emission of photon by atom
When a photon of light is emitted by an atom, it causes a decrease in the energy of the atom.
A photon of light is created.
The energy of the atom decreases by exactly the amount of energy contained in the photon that is emitted.
The photon can be emitted ONLY if it can produce an “allowed” energy decrease in an excited atom.

24. Emission of photon by atom
When a photon
Is emitted from
An atom, the
Atom drops to
A Lower
Quantum
Energy state.
The drop in
energy can be
computed by
DE = -hf.
D E = -hf

25. Emission Spectrum
When an atom emits photons, it glows! The photons cause bright lines of light in a spectrum.
Therefore, a spectrum with bright bands in it is called an emission spectrum.

26. Emission of photon by atom

27. Sample Problem

28. Solution
***

29. Photoelectric Effect #1
Sample Problem

30. Solution

31. Sample Problem

32. Solution

33. Atoms absorbing photons increase in energy

34. Question
Now, suppose a photon with TOO MUCH ENERGY encounters an atom?
If the atom is “photo-active”, a very interesting and useful phenomenon can occur…
This phenomenon is called the
Photoelectric Effect.

35. Photoelectric Effect
E = work function + K

36. Photoelectric Effect

37. Sample Problem

38. Solution

39. Photoelectric Effect #2
Sample Problem

40. Sample Problem

41. Solution

42. Review of Photoelectric Effect

43. Question

44. The Photoelectric Effect Experiment

45. Photoelectric Effect

46. Strange results in the Photoelectric Effect experiment

47. Voltage versus current for different intensities of light

48. Voltage versus current for different frequencies of light

49. Experimental determination of the Kinetic Energy of a photoelectron

50. Graph of Photoelectric Equation

51. Photoelectric simulations
This is a link for a simulated photoelectric effect experiment
Another link:
***

52. Mass of a Photon
Photon do not have “rest mass”. They must travel at speed of light and nothing can travel at the speed of light unless it has mass = zero.
A photon has a fixed amount of energy (E = hf)
We can calulate how much mass would have to be destroyed to create a photon (E=mc2)

53. Sample Problem
Calculate the mass that must be destroyed to create a photon of 340 nm light.
Emass = Ephoton
mc2 = hf = hc / l
m = h = h
cl cl
m = (6.625 x kgm2/s2 x s) =
(3x 10 8 m/s)(340 x m)

54. Momentum of Photon p = mv = mc(c/c)=mc2/c = E/c = hf/c = h/l
Photon do not have “rest mass”, yet they have momentum! This momentum is evident in that, given a large number of photons, they create a pressure?
A photon’s momentum is calculated by
p = E = hf = h
c c l

55. Experimental proof of the momentum of photons
Compton scattering
High-energy photons collided with electrons exhibit conservation of momentum
Work Compton problems just like other conservation of momentum problems - except the momentum of a photon uses a different equation.

56. Sample Problem
What is the momentum of photons that have a wavelength of 620 nm?
p = h = x kgm2/s2 x s
l x m
= __________________kgm/s
kgm/s  mass x velocity

57. Sample Problem
What is the frequency of a photon that has the same momentum as an electron with speed of 1200 m/s?
p e = p p
meve = h/l = h/c/f = hf/c
f = mevec/h
f = (9.11x kg)(1200m/s)(3x108m/s)
6.625 x kgm2/s2 x s
f = ________________s-1

58. Wave-Particle Duality
Waves act like particles sometimes and particles act like waves sometimes.
This is most easily observed for very energetic photons (gamma or x-Ray) or very tiny particles (electrons or nucleons)

59. Particles and Photons both have Energy
A moving particle has kinetic energy.
E = K = ½ mv2
A particle has most of its energy locked up in its mass.
E = mc2
A photon’s energy is calculated using its frequency.
E = hf

60. Particles and Photons both have Momentum
For a particle that is moving
p = mv
For a photon
p = h/l
Check out the units! They are those for momentum.

61. Particles and Photons both have Wavelength
For a photon
l = c/f
For a particle, which has an actual mass, this equation still works
l = h/p where p = mv
This is referred to as the deBroglie wavelength

62. Experimental proof that particles have wavelength
Davisson-Germer Experiment
Verified that electrons have wave properties by proving that they diffract
Electrons were “shone” on a nickel surface and acted like light by diffraction and interference

63. Problem
What is the momentum of photons that have a wavelength of 620 nm?

64. Sample problem
What is the wavelength of a 2,200 kg elephant running at 1.2 m/s?
p = h/l  l = h/p = h/mv
l = x Js
(2200kg)(1.2m/s)
lelephant = 2.51 x m

65. Naming a Nucleus Physicists Chemists Mass # Electronic Chg on
atom or molecule
Charge # # atoms in molec.

66. Most common isotope of carbon
Mass Number: protons plus neutrons 12 C
Element symbol 6
Atomic number: protons

67. Isotopes
Isotopes have the same atomic number but different atomic mass.
Isotopes have similar or identical chemistry.
Isotopes have different nuclear behavior.

68. Uranium Isotopes
U U
Low Radioactive Fission

69. Nuclear Particles Proton Mass: 1 amu Charge: +e Neutron Mass: 1 amu
(1 amu = 1/12 mass of Carbon 12 atom)

70. Electrons
Negative 0 e -1
Positive +1

71. Nuclear Reactions
Nuclear Decay - a spontaneous process in which an unstable nucleus ejects a particle and changes to another nucleus.
Alpha decay
Beta decay
Beta Minus
Positron
Fission - a nucleus splits into two fragments of roughly equal size
Fusion - Two nuclei combine to form a heavier nucleus.

72. Decay Reactions Alpha decay
A nucleus ejects an alpha particle, which is just a helium nucleus
Beta decay
A nucleus ejects a negative electron
Positron decay
A nucleus ejects a positive election
Simulations: Nuclear Reactions
(Bozeman)

73. Nuclear Decay
Radiation and radioactive decay (Bozeman):

74. Alpha Decay This occurs when a helium nucleus is released.
This occurs only with very heavy elements.

75. Beta (b-) Decay
A beta particle (negative electron) is released when a nucleus has too many neutrons for the protons present. A neutron converts to a proton and electron leaving a greater number of protons. An antineutrino is also released. +

76. Positron (b+) Decay
Positron decay occurs when a nucleus has too many protons for the neutrons present. A proton converts to a neutron. A neutrino is also released.

77. Neutrino and Anti-Neutrino …
Proposed to make beta and positron decay obey conservation of energy.
Possess energy and spin, but do not possess mass or charge.
Do not react easily with matter and are extremely hard to detect.

78. Neutrino & Antineutrino Production
Neutrinos are produced in nuclear reactions in the Sun when: 4protons --> alpha particle + 2p+ + 2neutrinos Antineutrinos are produced by natural radioactivity in the Earth by the decay of 238U and 232Th

79. Gamma Radiation, h
This isotope of radium has a small percentage of particles that don't have their full energy; instead the nucleus is left excited and emits gamma rays.

80. Complete the reaction and identify the type of decay:

81. Complete the reaction for the alpha decay of Thorium-232.+

82. Fission and Fusion

83. Fission
Occurs when an unstable, heavy nucleus split apart into two lighter nuclei (new elements).
Can be induced by free neutrons.
Mass is destroyed and energy produced according to E = mc2.

84. Neutron-induced fission
Produces a chain reaction
Nuclear power plants operate by harnessing the energy released in fission by controlling the chain reaction of U-235.
Nuclear weapons depend upon the initiation of an uncontrolled fission reaction

85. U-235 bombarded with a neutron eads to an exponential growth of chain reactions.

86. A single U-235 fuel pellet the size of a fingertip contains as much energy as 17,000 cubic feet of natural gas, 1,780 pounds of coal or 149 gallons of oil.
For more information:

87. Naturally occurring uranium consists of three isotopes: uranium-234, uranium-235 and uranium-238. Although all three isotopes are radioactive, only uranium-235 is a fissionable material that can be used for nuclear power.

88. Uranium-238, uranium's most common
Uranium-238, uranium's most common isotope, can be converted into plutonium- 239, a fissionable material that can also be used as a fuel in nuclear reactors. To produce plutonium-239, atoms of uranium-238 are exposed to neutrons. Uranium-239 forms when uranium-238 absorbs a neutron. Uranium-239 has a half-life of about 23 minutes and decays into neptunium-239 through beta decay. Neptunium-239 has a half-life of about 2.4 days and decays into plutonium-239, also through beta decay.

89. Critical Mass
The neutrons released from an atom that has undergone fission cannot immediately be absorbed by other nearby fissionable nuclei until they slow down to “thermal” levels.
A critical mass is the smallest amount of fissile material needed for a sustained nuclear chain reaction.

90. Nuclear Reactors
Nuclear reactors produce electrical energy through fission.
Advantages: a large amount of energy is produced without burning fossil fuels or creating greenhouse gases.
Disadvantage: produces highly radioactive waste.
Simulation:

92. Fission
Occurs only with very heavy elements since fissionable nuclei are too large to be stable.
A charge/mass calculation is performed to balance the nuclear equation.
Mass is destroyed and energy is produced according to E = mc2.

93. Problem: complete the following reaction and determine the energy released.?

94. Fusion
Occurs when 2 light nuclei come together to form a new nucleus of a new element.
The most energetic of all nuclear reactions.
Produced on the sun.
Fusion of light elements can result in non-radioactive waste.
Proton-Proton Reaction

95. Fusion
The reaction that powers the sun. It has not been reliably sustained on earth in a controlled reaction.
Advantages: tremendous energy produced and lack of radioactive waste products.
Disadvantages: too much energy to control.

96. Mass defect…
How much mass is destroyed when a nucleus is created from its component parts.
Generally much less than the mass of a proton or neutron, but it is still significant.
This loss of energy results in the creation of energy according to E = mc2.

97. Calculating energy released in nuclear reactions
Add up the mass (in atomic mass units, u_ of the reactants. Use your book.
Add up the mass ( in amu’s) of the products.
Find the difference between reactant and product mass. The missing mass has been converted into energy.
Convert mass to kg (1 u = 1.66x10-27 kg)
Use E = mc2 to calculate energy released.

98. Mass of reactants (6 neutrons, 6 protons)
What is the mass defect of 12C in atomic mass units? How does this relate to mass in kg and energy in eV and J?
6 1n + 6 1H  12C amu=1.66x10-27 kg
E =eV, e =1.6x10-19C
Mass of reactants (6 neutrons, 6 protons)
6( amu)+6( amu) =
Mass of product : 1(12.000) =
Dm =
E=1.476x10-11J=92MeV
1.6x10-19J/eV
Dm=( u)(1.66x10-27kg/u)
Dm=1.4x10-28kg
E = Dmc2 = (1.4x10-28kg)(3x108m/s)2
E = x 10-11J

99. Problem
When a free proton is fused with a free neutron to form a deuterium nucleus, how much energy is released?
Mass of 1 proton = amu
Mass of 1 neutron = amu

100. Mass on the left: 1. 008665 +1. 0078225 = 2. 0164875u On the right: 2
Mass on the left: = u On the right: Mass defect: u

101. Radioactive Decay of Bismuth-210
(T½ = 5 days)
Translation: “The half life of Bismuth-210 is 5 days.”

102. Radioactive Decay of Bismuth-210 (T½ = 5 days)
The half life for bismuth is 5 days.
At the end of 5 days there is 50 g remaining
After 10 days 25 g
After 15 days 12.5 g
What is happening to the radioactive bismuth?

104. Half Life Problem
Tritium (H-3) has a half life of 12.3 yr. How much of a 1.0 g sample will remain after 24.6 yr? 24.6yr 1 h.l. = 2 h.l yr Sample = 1.0 g = 0.25 g remaining 2 xh.l. 2 2h.l.