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

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

2 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 3 Electromagnetic Spectrum

4 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 5 But light is also a wave! We studied this earlier in the year and we will use this equation again here. C = f C: 3 x 10 8 m/s (speed of light in a vacuum) f: frequency (Hz or s -1 ) : wavelength (m) (distance from crest to crest)

6 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 7 Calculating photon energy The energy of a photon is calculated from the frequency of the light. E = hf = hc / because c = f E = nhf (for multiple n # of photons) E: energy (J or eV) h: Planck’s constant 6.625 x 10 -34 J s (SI system) 4.14 x 10 -15 eV s (convenient) f: frequency of light (s -1, Hz)

8 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 9 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 = 1.602 x 10 -19 J

10 10 Sample Problem What is the frequency and wavelength of a photon whose energy is 4.0 x 10 -19 J? E = hf f = E/h = c = f = c/f =

11 11 Sample Problem The bonding energy of H 2 is 104.2 kcal/mol. Determine the frequency and wavelength of a photon that could split one atom of H 2 into two separate atoms. (1 kcal = 4l86 J). E = (104.2 kcal)(4186 J)( 1 mol ) mol kcal 6.02x10 23 mol’cls E = 7.24 x 10 -19 J = hf f = 7.24 x 10 -19 J/ 6.625 x 10 -34 Js f = 1.09 x 10 15 Hz ***

12 12 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 632.8 nm? P = E tot /t E = hf  P = n(hf)/t c = f  f = c/ P = nh(c/ ) n = (P)(t)(  ) t (c)(h)

13 13 Solution Find total energy in one second from power P = W/t = E tot / t E tot = Pt = 3.0 x 10 -3 J Now see how many photons, n, will produce this energy E = hf (one photon) E tot = nhf (for n photons) E = nhc/ (since wavelength is given and not frequency) 3.0x10 -3 = n (6.625x10 -34 Js)(3.0x10 8 m/s)/632.8x10 -9 m n = 9.55 x 10 16

14 14 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

15 15 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.

16 16 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.

17 17 Transitions of the electron within the atom must occur from one allowed energy level to another. The atom CANNOT EXIST between energy levels.

18 18 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.

19 19 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  E = hf. Ground state

20 20 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

21 21 Absorption Spectrum Absorption spectra always involve atoms going up in energy level.

22 22 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.

23 23 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  E = -hf.  E = -hf

24 24 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.

25 25 Emission of photon by atom

26 26 Sample Problem

27 27 Solution ***

28 28 Photoelectric Effect #1 Sample Problem

29 29 Solution

30 30 Sample Problem

31 31 Solution

32 32 Atoms absorbing photons increase in energy

33 33 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.

34 34 Photoelectric Effect E = work function + K

35 35 Photoelectric Effect

36 36 Sample Problem

37 37 Solution

38 38 Photoelectric Effect #2 Sample Problem

39 39 Sample Problem

40 40 Solution

41 41 Review of Photoelectric Effect

42 42 Question

43 43 The Photoelectric Effect Experiment

44 44 Photoelectric Effect

45 45 Strange results in the Photoelectric Effect experiment

46 46 Voltage versus current for different intensities of light

47 47 Voltage versus current for different frequencies of light

48 48 Experimental determination of the Kinetic Energy of a photoelectron

49 49 Graph of Photoelectric Equation

50 50 Photoelectric simulations toEffect/photo.htm toEffect/photo.htm This is a link for a simulated photoelectric effect experiment Another link: tra.html ***

51 51 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=mc 2 )

52 52 Sample Problem Calculate the mass that must be destroyed to create a photon of 340 nm light. E mass = E photon mc 2 = hf = hc / m = h = h c m = (6.625 x 10 -34 kgm 2 /s 2 x s) = (3x 10 8 m/s)(340 x 10 -4 m)

53 53 Momentum of Photon p = mv = mc(c/c)=mc 2 /c = E/c = hf/c = h/ 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

54 54 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.

55 55 Sample Problem What is the momentum of photons that have a wavelength of 620 nm? p = h = 6.625 x 10 -34 kgm 2 /s 2 x s  620 x 10 -9 m = __________________kgm/s kgm/s  mass x velocity

56 56 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 m e v e = h/ = h/c/f = hf/c f = m e v e c/h f = (9.11x10 -31 kg)(1200m/s)(3x10 8 m/s) 6.625 x 10 -34 kgm 2 /s 2 x s f = ________________s -1

57 57 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)

58 58 Particles and Photons both have Energy A moving particle has kinetic energy. – E = K = ½ mv 2 A particle has most of its energy locked up in its mass. – E = mc 2 A photon’s energy is calculated using its frequency. – E = hf

59 59 Particles and Photons both have Momentum For a particle that is moving – p = mv For a photon – p = h/ – Check out the units! They are those for momentum.

60 60 Particles and Photons both have Wavelength For a photon – = c/f For a particle, which has an actual mass, this equation still works – = h/p where p = mv – This is referred to as the deBroglie wavelength

61 61 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

62 62 Problem What is the momentum of photons that have a wavelength of 620 nm?

63 63 Sample problem What is the wavelength of a 2,200 kg elephant running at 1.2 m/s? p = h/  = h/p = h/mv = 6.625 x 10 -34 Js (2200kg)(1.2m/s) elephant = 2.51 x 10 -37 m

64 64 Nuclear Decay e.htm e.htm

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

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

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

68 68 Uranium Isotopes 238 235 U 92 92 Low Radioactive Fission

69 69 Nuclear Particles Proton Mass: 1 amu Charge: +e Neutron Mass: 1 amu Charge: 0 (1 amu = 1/12 mass of Carbon 12 atom)

70 70 Electrons Negative 0 e Positive 0 e +1

71 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 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 – ctivity/radioactivity.html ctivity/radioactivity.html

73 73 Alpha Decay This occurs when a helium nucleus is released. This occurs only with very heavy elements.

74 74 Beta (  - ) 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. +

75 75 Positron (  + ) 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.

76 76 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.

77 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 238 U and 232 Th 77

78 78 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.

79 79 Calculating energy released in nuclear reactions 1.Add up the mass (in atomic mass units, u_ of the reactants. Use your book. 2.Add up the mass ( in amu’s) of the products. 3.Find the difference between reactant and product mass. The missing mass has been converted into energy. 4.Convert mass to kg (1 u = 1.66x10 -27 kg) 5.Use E = mc 2 to calculate energy released.

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

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

82 82 Nuclear Bombardment htm htm

83 83 Fission and Fusion

84 84 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 = mc 2. n.html n.html

85 85 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

86 86 U-235 bombarded with a neutron eads to an exponential growth of chain reactions.

87 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: powerplantfuel/ powerplantfuel/ 87

88 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. 12.3 yr Sample = 1.0 g = 0.25 g remaining 2 xh.l. 2 2h.l. 88

89 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.isotopes 89

90 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.plutonium half-life neptuniumbeta decay 90

91 91 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.fissilenuclear chain reaction

92 92 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: ?q=nuclear+power+plant+operation& hl=en&emb=1&aq=f# ?q=nuclear+power+plant+operation& hl=en&emb=1&aq=f# ar-power.htm

93 93

94 94 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 = mc 2.

95 95 Problem: complete the following reaction and determine the energy released. ?

96 96 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

97 97 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.

98 98 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 = mc 2.

99 99 What is the mass defect of 12 C in atomic mass units? How does this relate to mass in kg and energy in eV and J? 6 1 n + 6 1 H  12 C 1amu=1.66x10 -27 kg 0 1 E =eV, e =1.6x10 -19 C Mass of reactants (6 neutrons, 6 protons) 6(1.008665 amu)+6(1.0078225 amu ) =12.09894 Mass of product : 1(12.000) =12.00000  m = 0.09894 E=1.476x10 -11 J=92MeV 1.6x10 -19 J/eV  m=(0.09894u)(1.66x10 -27 kg/u)  m=1.4x10 -28 kg E =  mc 2 = (1.4x10 -28 kg)(3x10 8 m/s)2 E = 1.476 x 10 -11 J

100 100 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 = 1.0078225 amu Mass of 1 neutron = 1.008665 amu

101 Mass on the left: 1.008665 +1.0078225 = 2.0164875u On the right: 2.000 Mass defect: 0.0164875 u 101

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

103 Radioactive Decay of Bismuth-210 (T ½ = 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 See page 809 in book also

105 105

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