* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Quantum and Nuclear Physics
Internal energy wikipedia , lookup
Elementary particle wikipedia , lookup
Quantum vacuum thruster wikipedia , lookup
Introduction to gauge theory wikipedia , lookup
Renormalization wikipedia , lookup
History of subatomic physics wikipedia , lookup
Photon polarization wikipedia , lookup
Time in physics wikipedia , lookup
Nuclear structure wikipedia , lookup
Conservation of energy wikipedia , lookup
Quantum electrodynamics wikipedia , lookup
Density of states wikipedia , lookup
Atomic nucleus wikipedia , lookup
Bohr–Einstein debates wikipedia , lookup
Old quantum theory wikipedia , lookup
Nuclear physics wikipedia , lookup
Hydrogen atom wikipedia , lookup
Matter wave wikipedia , lookup
Introduction to quantum mechanics wikipedia , lookup
Wave–particle duality wikipedia , lookup
Theoretical and experimental justification for the Schrödinger equation wikipedia , lookup
Quantum and Nuclear Physics The quantum nature of radiation (particle nature of waves) 1901: Max Plank found that atoms can only adsorb and emit energy in distinct quantities; this showed that energy displayed particle-like properties. 1905: Albert Einstein suggested that energy itself is quantized and can be viewed as a string of particles called photons. He established that energy has mass. The Photoelectric effect The Photoelectric effect Coconut shy Bowling ball Cricket ball Table tennis ball In this analogy, how do we model the; The photon energy? Work function? The max kinetic energy of the photoelectrons? How are the electrons released? Powerful red laser No electrons released Photoelectron Energy …and some energy is given to the electron as kinetic energy. - Some energy is needed to release the electron (the work function φ)… Photon Energy = work function + kinetic energy of electron Photoelectron emission Stopping potential Determining Planck’s constant • Add different filters under the light source Photoelectric experiment • Take measurements of stopping potential and wavelength to determine Planck’s constant and the threshold frequency Plot a graph of stopping potential versus frequency Photoelectric Effect: Vstop vs. Frequency eVstop hf Vstop 0 fmin /e hf min Slope = h/e Planck’s constant Determining “h” from the graph hf EK max Photoelectric Effect: IV Curve Dependence Intensity I dependence Vstop= Constant f1 > f2 > f3 Frequency f dependence f1 f2 Vstop f f3 Is light a wave or a particle? =Φ E max= V= Stopping voltage 1. The work function for lithium is 4.6 x 10-19 J. (a) Calculate the lowest frequency of light that will cause photoelectric emission. (6.9 x 1014 Hz ) (b) What is the maximum energy of the electrons emitted when light of 7.3 x 1014 Hz is used? (0.24 x 10-19 J ) 2. A frequency of 2.4 x 1015 Hz is used on magnesium with work function of 3.7 eV. (a) What is energy transferred by each photon? (b) Calculate the maximum KE of the ejected electrons. (c) The maximum speed of the electrons. (d) The stopping potential for the electrons. (a) 1.6 x 10-18 J (b) 1.0x 10-18 J (c) v = 1.5 x 106 m s-1 (d) Vs = 6.3 V Questions Hamper HL page 231 Q’s 1-4. IB revision pack Q’s 1,7,9,13,15,17,20. Tsokos page 396 q’s 1-7. The wave nature of matter Can particles be waves? Review of Bohr and deBroglie • Background: – Balmer found equation for Hydrogen spectrum but didn’t know what it meant. – Rutherford found that atoms had a nucleus, but didn’t know why electrons didn’t spiral in. • Bohr postulates that the orbit can fit an integral number of wavelengths associated with the electron, therefore has quantized energy levels, and predicts Balmer’s equation. • deBroglie postulates that electrons are waves, and predicts Bohr’s quantized energy levels. • Note: no experimental difference between Bohr model and deBroglie model, but deBroglie is a lot more satisfying. Davisson and Germer -- VERY clean nickel crystal. Interference is electron scattering off Ni atoms. e e e e e e Ni e e det. e e scatter off atoms e e move detector around, see what angle electrons coming off See peak!! so probability of angle where detect electron determined by interference of deBroglie waves! # e’s 0 e e e e 500 scatt. angle e e det. e e e Ni Observe pattern of scattering electrons off atoms Looks like …. Wave! An Accident at the Phone Company Makes Everything Crystal Clear There was an accident at the Bell Telephone Laboratories in April 1925. Clinton Davisson and L. H. Germer, looking for ways to improve vacuum tubes, were watching how electrons from an electron gun in a vacuum tube scattered off a flat nickel surface. Suddenly, while the experiment was running and the nickel target was very hot, a bottle of liquid air near the apparatus exploded, smashing one of the vacuum pipes, and air rushed into the apparatus. The hot nickel target oxidized immediately. The layer of oxide made their target useless for further investigations. They decided to clean off the oxide by heating the nickel in a hydrogen atmosphere then in vacuum. After doing this for a prolonged period, the nickel looked good, and they resumed the investigation. To their amazement, the pattern of electron scattering from the newly cleaned nickel target was completely different from that before the accident. What had changed? On examining their newly cleaned crystal carefully, they found a clue. The original target was polycrystalline -- made up of a multitude of tiny crystals, oriented randomly. During the prolonged heating of the cleaning process, the nickel had re-crystallized into a few large crystals. Electron diffraction Diffraction rings Calculating the De Broglie λ λ = h/p (= h/(2Ekm)1/2 ) h = Planck’s constant p = Momentum In 1923, French Prince Louis de Broglie, generalised Einstein's work from the specific case of light to cover all other types of particles. This work was presented in his doctoral thesis when he was 31. His thesis was greeted with consternation by his examining committee. Luckily, Einstein had received a copy in advance and vouched for de Broglie. He passed! de Broglie questions • Calculate the wavelengths of the “deBroglie” waves associated with • a)a 1kg mass moving at 50ms-1 • b)an electron which has been accelerated by a p.d. of 500V. a)Discuss briefly deBroglie’s hypothesis and mention one experiment which gives evidence to support it. b)Calculate the wavelength of the “deBroglie wave” associated with an electron in the lowest energy Bohr orbit. (The radius of the lowest energy orbit according to the Bohr theory is 5·3×10-11m.) Questions Hamper HL page 235 Q’s 9,10. IB revision pack Q’s Tsokos page 396 q’s 8-10 History of Quantum Mechanics Max Planck's work on the 'Black Body' problem started the quantum revolution in 1900. He showed that energy cannot take any value but is arranged in discrete lumps – later called photons by Einstein. In 1913, Niels Bohr proposed a model of the atom with quantised electron orbits. Although a great step forward, quantum physics was still in its infancy and was not yet a consistent theory. It was more like a collection of classical theories with quantum ideas applied. Starting in 1925 a true 'quantum mechanics' – a set of mathematically and conceptual 'tools' – was born. At first, three different incantations of the same theory were proposed independently and were then shown to be consistent. Quantum mechanics reached its final form (essentially unchanged from today) in 1928. Participants of the 5th Solvay Congress, Brussels, October 1927 E. Schrödinger W. Pauli W. Heisenberg N. Bohr M. Planck M Curie A. Einstein L.V. de Broglie Models of the Atom • Thomson – Plum Pudding – – – – – – Why? Known that negative charges can be removed from atom. – Problem: just a random guess • Rutherford – Solar System – Why? Scattering showed hard core. – Problem: electrons should spiral into nucleus in ~10-11 sec. + • Bohr – fixed energy levels – Why? Explains spectral lines. – Problem: No reason for fixed energy levels + • deBroglie – electron standing waves – Why? Explains fixed energy levels – Problem: still only works for Hydrogen. • Schrodinger – will save the day!! + – Visualising the models Hyperlink Different view of atoms The Bohr Atom Electrons are only allowed to have discrete energy values and these correspond to changes in orbit. The Bohr postulate The Schrodinger Atom Electrons behave like stationary Amplitude waves. Only certain types of wave fit the atom, and these correspond to fixed energy states. The square of the amplitude gives the probability of finding the electron at that point + 0eV Models of the Atom • Thomson – Plum Pudding – – – – – – Why? Known that negative charges can be removed from atom. – Problem: just a random guess • Rutherford – Solar System – Why? Scattering showed hard core. – Problem: electrons should spiral into nucleus in ~10-11 sec. + • Bohr – fixed energy levels – Why? Explains spectral lines. – Problem: No reason for fixed energy levels + • deBroglie – electron standing waves – Why? Explains fixed energy levels – Problem: still only works for Hydrogen. • Schrodinger – will save the day!! + – Schrödinger model Schrödinger set out to develop an alternate formulation of quantum mechanics based on matter waves, à la de Broglie. At 36, he was somewhat older than his contemporaries but still succeeded in deriving the now famous 'Schrödinger Wave Equation.' The solution of the equation is known as a wave function and describes the behavior of a quantum mechanical object, like an electron. At first, it was unclear what the wave function actually represented. How was the wave function related to the electron? At first, Schrödinger said that the wave function represented a 'shadow wave' which somehow described the position of the electron. Then he changed his mind and said that it described the electric charge density of the electron. He struggled to interpret his new work until Max Born came to his rescue and suggested that the wave function represented a probability – more precisely, the square of the absolute magnitude of the wavefunction is proportional to the probability that the electron appears in a particular position. So, Schrödinger's theory gave no exact answers… just the chance for something to happen. Even identical measurements on the same system would not necessarily yield the same results! Born's key role in deciphering the meaning of the theory won him the Nobel Prize in Physics in 1954. Quantum Mechanical tunneling In the classical world the positively charged alpha particle needs enough energy to overcome the positive potential barrier which originates from protons in the nucleus. In the quantum world an alpha particle with less energy can tunnel through the potential barrier and escape the nucleus. Electron in a box model Electrons will form standing waves of wavelength 2L/n Standing waves and energy levels Kinetic Energy of an electron in a box • When the momentum expression for the particle in a box : • • is used to calculate the energy associated with the particle Consider a ball in a hole: When the ball is here it has its lowest gravitational potential energy. Spectra 5J We can give it potential energy by lifting it up: If it falls down again it will lose this gpe: 5J 30J 20J Spectra A similar thing happens to electrons. We can “excite” them and raise their energy level: 0eV -0.85eV -1.5eV -3.4eV -13.6eV An electron at this energy level would be “free” – it’s been “ionised”. These energy levels are negative because an electron here would have less energy than if its ionised. This is called “The ground state” Spectra If we illuminate the atom we can excite the electron: Q. What wavelength of light would be needed to excite this electron to ionise it? 0eV -0.85eV -1.5eV -3.4eV Light Energy change = 3.4eV = 5.44x10-19J. Using E=hc/λ wavelength = 3.66x10-7m -13.6eV (In other words, ultra violet light) Example questions 1) State the ionisation energy of this atom in eV. 2) Calculate this ionisation energy in joules. 2.17x10-18J 3) Calculate the wavelength of light needed to ionise the atom. 94ηm 0eV -0.85eV -1.5eV -3.4eV 4) An electron falls from the -1.5eV to the 3.4eV level. What wavelength of light does it emit and what is the colour? 654ηm 5) Light of frequency 1x1014Hz is incident upon the atom. Will it be able to ionise the atom? -13.6eV Spectra Continuous spectrum Absorption spectrum Emission spectrum Emission Spectra Hydrogen Helium Sodium Observing the Spectra Microscope (to observe the spectrum) Collimator (to produce parallel light) Light source Gas Diffraction grating (to separate the colours) Emission spectrum Absorption spectrum Questions Hamper HL page 232 Q’s 5-8. IB revision pack Q’s Tsokos page 405 q’s 1-7. Outline the Heisenberg uncertainty principle with regard to position–momentum and time–energy. Students should be aware that the conjugate quantities, position–momentum and time–energy, cannot be known precisely at the same time. They should know of the link between the uncertainty principle and the de Broglie hypothesis. For example, students should know that, if a particle has a uniquely defined de Broglie wavelength, then its momentum is known precisely but all knowledge of its position is lost. Heisenberg uncertainty principle Heisenberg made one fundamental and long-lasting contribution to the quantum world – the uncertainty principle. He showed that quantum mechanics implied that there was a fundamental limitation on the accuracy to which pairs of variables, such as (position and momentum) and (energy and time) could be determined. If a 'large' object with a mass of, say, 1g has its position measured to an accuracy of 1 , then the uncertainty on the object's velocity is a minute 10-25 m/s. The uncertainty principle simply does not concern us in everyday life. In the quantum world the story is completely different. If we try to localize an electron within an atom of diameter 10-10 m the resulting uncertainty on its velocity is 106 m/s! Heisenberg uncertainty principle Questions Hamper HL page 232 Q’s 5-8. IB revision pack Q’s 3,11,16,22. Nuclear physics Determining the size of the nucleus Approach of alpha particle to nucleus Z = 79 (gold) 25 20 15 10 5 0 0 2 4 6 distance from nucleus / 8 10–14 10 m 1. Make an arithmetical check to show that at distance r = 1.0x10–14 m, the electrical potential energy, is between 20 MeV and 25 MeV, as shown by the graph. 2.How does the electrical potential energy change if the distance r is doubled? 3.From the graph, at what distance r, will an alpha particle with initial kinetic energy 5 MeV colliding head-on with the nucleus, come to rest momentarily? 1. Substituting values gives EP = 2. 3. 2 79 1.6 10 19 C 4 8.85 10 12 C 2 J 1 m 1 1.0 10 14 m 10 6 22 .7 MeV. Halves, because the potential energy is proportional to 1/r. About 4.6x10–14 m, where the graph reaches 5 MeV. Charge in a magnetic field Recall: + + Circular paths 2 protons, 2 neutrons, therefore charge = +2 - 1 electron, therefore charge = -1 Because of this charge, they will be deflected by magnetic fields: These paths are circular, so Bqv = mv2/r, or r =mv Bq Bainbridge mass spectrometer Ions are formed at D and pass through the cathode C and then through a slit S1 A particle with a charge q Hyperlink and velocity v will only pass through the next slit S2 if the resultant force on it is zero – that is it is traveling in a straight line. That is if: Velocity selector Therefore Mass selector In the region of the Mag field r = Mv/(Bq) Bqv = Mv2/r Therefore Nuclear energy levels There are 2 distinct length of tracks in this Alpha decay Therefore, the energy levels in the nucleus are discrete The existence of Neutrinos How can a 2 body system create a spectrum of energies? There must be a 3rd particle The Neutrino was postulated A 2 body system only has one solution A 3 body system has many solutions Changes in Mass and Proton Number Beta - decay: 90 Sr 38 90 Y 39 + 0 β + ν -1 “positron” Beta + decay: 11 6 C 11 B 5 + 0 +1 β+ ν Questions Hamper HL page 239 Q’s 11-17. IB revision pack Q’s 14,21. Radioactive Decay Law dN/N = -λdt which when integrated, gives Taking antilogs of both sides gives: Half life and the radioactive decay constant When N = No/2 the number of radioactive nuclei will have halved Therefore when t = T1/2 N = No/2 = Noe-λT1/2 and so 1/2 = e-λT1/2 . Taking the inverse gives 2 = eλT1/2 and so: Measuring long half lives • If the half life is very long, then the activity (A) is constant • Analysis of a decay curve cannot give the half life. • If the mass of the substance is measured, then • A = -λN, so a measurement of the activity enables Measuring long half lives to be calculated (N from mass). • T1/2 can be calculated from λ. Measuring short half lives • Each decay can cause an ionisation • This can generate an electric current • If the current is displayed on an oscilloscope, then • The limit is the response time of the oscilloscope (typically µs). Questions Hamper HL page 255. Q’s 27-31. IB revision pack Q’s 2,4,10,23.