1 My Chapter 27 Lecture

2 Chapter 27: Early Quantum Physics and the Photon Blackbody Radiation The Photoelectric Effect Compton Scattering Early Models of the Atom The Bohr Model for the Hydrogen Atom Pair Production/Annihilation

3 §27.1 Quantization A quantity is quantized if its possible values are limited to a discrete set. An example from classical physics is the allowed frequencies of standing waves on a stretched string. Only integer multiples of the fundamental frequency produce standing waves.

4 §27.2 Blackbody Radiation A blackbody emits a continuous spectrum of radiation. The spectrum is determined only by the temperature of the blackbody.

5 To correctly explain the shape of the blackbody spectrum Planck proposed that the energy absorbed or emitted by oscillating charges came in discrete bundles called quanta. The energy of the quanta are where h =  J s is called Planck’s constant. The quantum of EM radiation is the photon.

6 §27.3 The Photoelectric Effect Under certain circumstances EM radiation incident on a metal will eject electrons from the metal. This is the photoelectric effect.

7 Experiments show: 1.Brighter light causes more electrons to be ejected, but not with more kinetic energy. 2.The maximum KE of ejected electrons depends on the frequency of the incident light. 3.The frequency of the incident light must exceed a certain threshold, otherwise no electrons are ejected. 4.Electrons are ejected with no observed time delay regardless of the intensity of the incident light.

8 The wave theory of light says EM waves carry energy. The energy is absorbed by electrons in the metal target which are then ejected when they accumulate enough energy to escape. However the wave theory is unable to completely explain the photoelectric effect. Einstein proposed a particle theory of light.

9 Wave theory predicts a more intense beam of light, having more energy, should cause more electrons to be emitted and they should have more kinetic energy. Particle theory predicts a more intense beam of light to have more photons so more electrons should be emitted, but since the energy of a photon does not change with beam intensity, the kinetic energy of the ejected electrons should not change. The particle theory is consistent with observation 1. Observation 1

10 Wave theory cannot explain the frequency dependence of the maximum kinetic energy. Particle theory predicts the maximum kinetic energy of the ejected electrons to show a dependence on the frequency of the incident light. Each electron in the metal absorbs a whole photon: some of the energy is used to eject the electron and the rest goes into the KE of the electron. Observation 2 The particle theory is consistent with observation 2.

11 The maximum KE of an ejected electron is where  is called the work function and is the energy needed to break the bond between the electron and the metal.

12 Particle theory predicts a threshold frequency is needed. Only the incident photons with f > f threshold will have enough energy to free the electron from the metal. Wave theory can offer no explanation. Observation 3 The particle theory is consistent with observation 3.

13 The electron is ejected from the metal when the energy supplied by the photon exactly equals the work function. This defines the threshold frequency. Here it is often convenient to use h =  eV s.

14 Wave theory predicts that if the intensity of the light is low, then it will take some time before an electron absorbs enough energy to be ejected from the metal. Particle theory predicts a low intensity light beam will just have a low number of photons, but as long as f > f threshold an electron that absorbs a whole photon will be ejected; no time delay should be observed. Observation 4 The particle theory is consistent with observation 4.

15 The particle theory of light is needed to explain the photoelectric effect (and Compton scattering and pair production). A wave theory of light is needed to explain interference patterns. Both are correct (wave-particle duality).

16 Example (text problem 27.1): A 200 W infrared laser emits photons with a wavelength of 2.0  m while a 200 W ultraviolet laser emits photons with a wavelength of 7.0  m. The UV photon has the greater energy; its wavelength is smallest. (b) What is the energy of a single infrared photon and the energy of a single ultraviolet photon? (a) Which has greater energy, a single infrared photon or a single ultraviolet photon?

17 Example (text problem 27.4): The photoelectric threshold frequency of silver is 1.04  Hz. What is the minimum energy required to remove an electron from silver?

18 Example (text problem 27.11): Two different monochromatic light sources, one yellow (580 nm) and one violet (425 nm), are used in a photoelectric effect experiment. The metal surface has a photoelectric threshold frequency of 6.20  Hz. The frequency of each source is Only the violet light is above the threshold frequency. (a) Are both sources able to eject photoelectrons from the metal? Explain.

19 (b) How much energy is required to eject an electron from the metal? Example continued:

20 §27.5 Compton Scattering x y Before Collision After Collision Photon (E 0, p 0 ) Free electron at rest Photon (E 1, p 1 ) Free electron (K, p)  

21 Conserve momentum and energy during the collision: E=pc for a photon

22 The Compton wavelength  is the Compton shift. Manipulating the previous expressions gives

23 Example (text problem 27.27): A photon is incident on an electron at rest. The scattered photon has a wavelength of 2.81 pm and moves at an angle of 29.5  with respect to the direction of the incident photon. The Compton shift is The incident wavelength is (a) What is the wavelength of the incident photon?

24 Example continued: (b) What is the final kinetic energy of the electron? The final kinetic energy of the electron is equal to the change in the photon’s energy.

25 §27.6 Spectroscopy and Early Models of the Atom A hot, solid object will emit a continuous spectrum. A hot gas will show an emission or line spectrum (dark background with bright lines). Each element has its own unique set of spectral lines.

26 An absorption spectrum (bright background with dark lines) is seen if a hot source is viewed though a gas. Examples of emission spectra:

27 Before the structure of the atom was known, an empirical result was derived for the wavelengths of the spectral lines of hydrogen in the visible portion of the spectrum (the Balmer series). Where R =  10 7, m -1 is the Rydberg constant and n  3.

28 The Thomson model of the atom had a volume of positive charge with the negatively charged electrons embedded within the volume. Scattering experiments by Rutherford led to the conclusion that an atom had a very small nucleus of positive charge (10 -5 times the size of the atom containing nearly all of the mass) that was surrounded by the electrons.

29 It was thought that the electrons in their orbits should radiate (they are accelerated) causing the electron’s orbit to decay, implying that atoms are not stable. This is obviously false. Any model of the atom must also explain the line spectra of the elements.

30 §27.7 The Bohr Model of the Hydrogen Atom The Bohr model assumes: The electron is allowed to be in only one of a discrete set of states called stationary states. The electron orbits have quantized radii, energy, and angular momentum.

31 Newtonian physics applies to an electron in a stationary state. The electron can transition between one stationary state and another provided it can absorb/emit a photon of energy equal to the energy difference between the states.  E = hf. The stationary states have quantized angular momentum in the amount n is an integer.

32 The allowed radii are where a 0 = 52.9 pm is the Bohr radius.

33 The energy levels are given by where E 1 =  13.6 eV is the energy of the ground state, the lowest possible energy of the electron. When n > 1 the electron is in an excited state. The quantity n is an integer and is the principal quantum number.

34 Energy level diagram for hydrogen

35 The energy of a photon emitted (absorbed) by an electron during a transition is where is the Rydberg constant. When n f =2, the above result reduces to the Balmer formula.

36 The Bohr model correctly predicted the wavelengths of the spectral lines of hydrogen in the visible. There are several problems with the Bohr model.

37 Bohr’s model, while successful at predicting the spectrum of hydrogen, fails at predicting the spectra of most other elements. Only hydrogenic atoms (atoms that only have one electron; Li 2+ for example) can have their spectra computed using the Bohr model. The allowed radii are The energy levels are where Z is the atomic number of the atom and E 1H =  13.6 eV.

38 Example (text problem 27.34): Find the Bohr radius of doubly ionized lithium (Li 2+ ). What is r 1 ? The inner most energy level is closer to the nucleus than in an H atom.

39 Example (text problem 27.35): Find the energy in eV required to remove the remaining electron from a doubly ionized lithium (Li 2+ ) atom. The electron is in the ground state (n = 1), so To remove the electron will require the electron be given 122 eV of energy.

40 Example (text problem 27.43): A hydrogen atom has an electron in the n = 5 level. One photon; the electron may transition from the n = 5 level to the n = 1 level. (b) What is the maximum number that might be emitted? Four photons; the electron may cascade from n = 5 to 4 to 3 to 2 to n = 1. (a) If the electron returns to the ground state, what is the minimum number of photons that can be emitted?

41 §27.8 Pair Annihilation and Pair Production A photon can interact with an atomic nucleus and change itself into an electron-positron pair (or some particle- antiparticle pair.) A positron is an antielectron. The nucleus is needed to ensure that momentum is conserved.

42 The energy of the photon must be at least 2m e c 2. If E > 2m e c 2, then the additional energy goes into the kinetic energy of the electron-positron pair. This is pair production. The inverse process is

43 The process of pair production created protons, neutrons, and electrons in the earliest moments after the Big Bang. To have enough energy, the photons must be “hot” enough. Electrons need T~10 10 K and for protons/neutrons T~10 13 K. The early Universe must have been much hotter than it is today. Pair production creates equal amounts of matter and antimatter. Where in the Universe is all of the antimatter?

44 Example (text problem 27.57): A muon and an antimuon, each with mass 207 times greater than an electron, were at rest when they annihilated and produced two photons of equal energy. What is the wavelength of each of the photons? For an electron-positron pair For a muon-antimuon pair

45 Example continued: The created photons each have 106 MeV of energy. Their wavelengths are

46 Summary Quantization The Photoelectric Effect Compton Scattering Pair Production/Annihilation Spectroscopy Bohr Model for Hydrogen } These processes are explained by light behaving like a particle, not as a wave.