Introduction to Nuclei I
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1 Introduction to Nuclei I (The Discovery) The opposite of a correct statement is a false statement. But the opposite of a profound truth may well be another profound truth - Niels Bohr
2 The Atom (as we know it today) ATOM is the smallest particle that characterize a chemical element. A heavy NUCLEUS with a POSITIVE electric charge surrounded by a swarm of much lighter particles, the NEGATIVELY charged ELECTRONS.
3 Atom in 1900 Amidst buzzing electricity and glowing tubes, J.J. Thomson discovered the electron (1897) negatively charged, Electron Proposes a model of Atom Thomson s plum pudding model Positively charged background
4 Explaining the spectrum of light emitted from Atom One of the most important problems of early 20 th Century Physics
5 1909, The α scattering experiment (The dawn of Nuclear Physics) Ernest Rutherford ( ) Geiger, and Marsden bombarded a thin gold foil with alpha particles (a helium atom with its electron stripped off). Rutherford s Scattering Experiment (1909)
6 Experiment of Geiger and Marsden (1909) A good number of α particles were scattered from thin goldleaf targets at backward angles (greater than 90 )!
7 It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back and hit you - E. Rutherford
8 What could have caused the α particles to scatter to such large angles? Electron Could it be the electrons? Maximum scattering angle from electron corresponding to the maximum momentum change. p = max 2m ev α θ max = pα 2mevα = = too small! p M v α α α
9 Could it be the multiple scattering of electrons? If an α particle is scattered by N atoms: N = the number of atoms across the thin gold layer, t = m: n= The distance between atoms, d = n-1/3, is: N=t/d still too small!
10 Ernest Rutherford ( ) 1911, Rutherford s Atomic Model (The Nucleus is born) even if the α particle is scattered from all 79 electrons in each atom of gold. Atom should have a positively charged core (nucleus) surrounded by the negative electrons - Rutherford Ernest Rutherford ( )
11 Rutherford s model can explain the experimental scattering data Rutherford s Scattering Formula
12 Structure of Atom in 1911? A positively charged core Nucleus surrounded by Electrons.
13 1915, Bohr put Thomson s electron into orbit (Planetary Model of the Atom) Electron Nucleus Niels Bohr ( ) - Bohr s Planetary Model could explain the Hydrogen Atom - Atomic Excitation by Electrons - Quantum mechanical treatment and the Shell model of Atom - Spin of the electron (Stern Gerlach experiment) - Closed shell & Magic numbers : 2, 8, 20, 28, 50 - Pauli exclusion principle for the electrons - Characteristic X-Ray s and Atomic Spectra,.
14 Atomic Nucleus in 1915? What is the nucleus made of? What is its composition?
15 Proton is discovered (1918) (The philosopher s stone) Alpha particle shot into Nitrogen gas. Hydrogen nuclei detected in Scintillation detector. Rutherford concluded that Nitrogen must contain hydrogen nuclei. Suggested that the hydrogen nucleus, which was known to have Atomic number of 1, was an elementary particle. Called this particle as, Proton.
16 The discovery of Neutron (1932) (The last piece of the puzzle) 1930, Bothe & Becker, bombarded the element beryllium (Be) with alphaparticles. This reaction emitted a very penetrating neutral radiation. They thought it was gamma-rays. J. Chadwick proposed (1932) that the unknown radiation was a new type of particle NEUTRON, - charge neutral & roughly the same mass as proton Chadwick explained the process occurring in the experiment as: Neutron
17 The proton-neutron model of the Nucleus The nucleus consists of Protons and Neutrons, together called Nucleons. The number of Protons in the nucleus is called the Atomic number (Z) of the nucleus. The total number of Protons and Neutrons in the nucleus is called the Mass number (A) of the nucleus. Each nucleus is represented as where X = element symbol (e.g., Na, Co, U), Z = Atomic number and A = Mass number. Is still the basic model of the atomic nucleus today.
18 Few Nuclear Terms Nuclides with the same Z are called Isotopes. They have the same chemical properties. Nuclides with the same N are called Isotones. Nuclides with the same A are called Isobars and have approximately the same mass. Nuclides with N and Z interchanged are called mirror nuclides.
19 What holds the nucleons in the nucleus together? The Nuclear Force Yukawa s theory of meson exchange, 1934
20 Binding energy of the nucleus Energy required to break the nucleus into its constituent nucleons. B = (Z m p + N m n M)c 2 Greater the binding energy, more difficult it is to break a nucleus into its separate constituents
21 Semi-empirical Binding energy formula (V. Weiszsacher, 1935)
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23 Liquid drop model cannot explain the fine structures in the Binding energy curves Peaks appear in binding energy curve for nucleus with magic numbers of protons and/or neutrons, just like in electronic structure of electrons Evidence for shell structure in the nucleus
24 The Shell Model of the Nucleus (1933, 1948) Similar to that used in the electronic structure of atom (Bartlett et al, 1933) Could explain only the first 3 magic numbers 2, 8, 20 All efforts to explain the nucleus using shell model abandoned 1948, M. Mayer, and independently Haxel, Jensen & Suess revived the Shell model of nucleus Growing evidence from experimental data for a shell like structure of atomic nucleus Spin-orbit coupling introduced Could explain all the magic numbers Maria Goppert-Mayer ( ) Spin-orbit coupling occurs when two motions are coupled together, such as the earth spinning on its axis as it orbits the sun. In an atom, the electron spins on an axis as it orbits the nucleus.
25 Shell Model of the Nucleus Each proton or neutron in the nucleus feels an average force from the other nucleons. This force can be modeled as a potential well. Nuclear energy levels
26 Shell Model of the Nucleus The nucleons exist in certain energy levels within the nucleus, So-called magic numbers have been found: 2,8, 20, 50, 82, isotopes containing these number of protons or neutrons have unusual stability in their structure. Nucleons can be excited to higher energy levels just like electrons in atoms. Gamma rays emitted.
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