Introduction to Nuclei I (The discovery)
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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 Atomic Nucleus An atom is the smallest particle that characterize a chemical element. It consists of a heavy NUCLEUS with a POSITIVE electric charge, which is surrounded by a swarm of much lighter particles, the NEGATIVELY charged ELECTRONS.
3 Knowledge of atoms in 1900 Thomson s Atomic Model Electron (discovered in 1897) Thomson s plum-pudding model of the atom had the positive charges spread uniformly throughout a sphere the size of the atom, with electrons embedded in the uniform background. But cannot explain the discrete lines in atomic spectra Positively charged background
4 Discovery of Nucleus : The dawn of Nuclear Physics Rutherford s Scattering Experiment (1909) Ernest Rutherford ( ) Geiger, and Marsden bombarded a thin gold foil with alpha particles (a helium atom with its electron stripped off).
5 Experiments of Geiger and Marsden (1909) They found that many α particles were scattered from thin goldleaf targets at backward angles greater than 90.
6 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
7 Electrons can t backscatter α particles. Electron Calculate the maximum scattering angle corresponding to the maximum momentum change. Δp = max 2m ev α θ max = Δpα 2mevα = = too small! p M v α α α
8 Try multiple scattering 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!
9 Rutherford s s Atomic Model (1911) even if the α particle is scattered from all 79 electrons in each atom of gold. Ernest Rutherford ( ) Rutherford proposed that an atom should have a positively charged core (nucleus) surrounded by the negative electrons.
10 Rutherford Scattering Formula The number of particles scattered per unit area is:
11 Structure of atom in 1911?? What is a nucleus made of? What is its composition?
12 Planetary Model of the Atom (1915) Electron Nucleus Niels Bohr ( ) - The Bohr Planetary Model of 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 Spectras,.
13 Knowledge of atoms in 1911? What is a nucleus made of? What is its composition?
14 The discovery of neutron (1932) In 1930, two German physicists, Bothe & Becker, bombarded the elements beryllium (Be) with alpha-particles. These elements, emitted a very penetrating form of radiation that was much more energetic than gamma-rays. J. Chadwick proposed (1932) that the unknown radiation was a new type of particle NEUTRON, it has to be charge neutral with roughly the same mass as proton Chadwick explained the process occurring in the experiment as: neutron
15 The proton-neutron neutron model of nucleus Following Chadwick s discovery of the neutron, a new model of the nucleus. The nucleus consists of protons and neutrons. Together they are called nucleons The number of protons in the nucleus is called the atomic number of the nucleus. The total number of protons and neutrons in the nucleus is called the mass number of the nucleus. Each nucleus can be represented as where X = element symbol (eg Na, Co, U), Z = atomic number and A = mass number. The proton-neutron model of the nucleus is still the basic model used today.
16 Few Nuclear Terminology 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.
17 What holds the nucleons together? There must be some force to hold them together in a nucleus The force responsible for holding all nucleons together is the strong nuclear force (H. Yukawa, 1934) Yukawa s theory of meson exchange
18 Binding energy of a nucleus B = (Z M p + N M n M)C 2 It is the energy required to break a nucleus into its constituent nucleons It determines the stability of the nucleus Larger the binding energy, more difficult it is to break a nucleus into its separate constituents
19 Semi-emperical emperical Binding energy formula (Weiszsacher,, 1935)
20
21 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
22 The Shell Model of Nucleus (1933, 1948) Bartlett et al propose shell model, similar to that used to study electronic structure of atom, for the nucleus (1933) Could explain only the first 3 magic numbers 2, 8, 10 All efforts to explain the nucleus using shell model abandoned 1948, M. Mayer, and independently Haxel, Jensen & Suess revived the Shell model of nucleus Maria Goppert-Mayer ( ) Growing evidence from experimental data for a shell like structure of atomic nucleus Spin-orbit coupling introduced Could explain all the magic numbers 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.
23 Shell Structure 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
24 Shell Model of the Nucleus The various nucleons exist in certain energy levels within the nucleus, So-called magic numbers have been found:,2,8, 20, 50, 82, 126- 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. Gamma rays emitted.
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