The constitution of nucleus

1. The constitution of nucleus Third lecture

2. The proton-electron hypothesis of the constitution of the nucleus • Prout: suggest that all atomic weights must be integral multiples of the atomic weight of hydrogen and all elements might be built up of hydrogen . But it was found that atomic weight of some elements are fractional as Cl , Cu . • Nevertheless, so many elements have atomic weights are seemed to be some basis for Prout's hypothesis. The idea that all elements are built up from one basic substance received supports after the discovery of isotopes. • Also, It was found that most elements are mixtures of isotopes, and the different isotopes of an element have the same number and the arrangements of electrons, and consequently their spectra have the same general structure. They are distinguished from one another by their different atomic masses.

3. Aston: formulate his whole numbers rule, which is modified from Prout's hypothesis. •  According to Aston's rule: • “All atomic weights are very close to integers, and the fractional atomic weights are caused by the presence of two or more isotopes each of which has a nearly integral atomic weight”. •  The combination of the whole number rule and the properties of the hydrogen nucleus lead to assumption that atomic nuclei are built up of hydrogen nuclei, and the hydrogen nucleus was given the name proton. • The proton-electron hypothesis of nucleus seemed to be consistent with the emission of α and β particles by the atoms of radioactive elements. The interpretation of radioactivity showed that both α and β particles were ejected from the nuclei of the atoms undergoing transformation and the presence of electrons in the nucleus made it seem reasonable under same conditions, one of them might be ejected. • It was also assumed that the α-particle could be formed in the nucleus by the combination of four protons and two electrons.

4. The angular momentum of the nucleus; Failure of the proton – electron hypothesis: • One of the failures of the hypothesis was associated with an unknown property of the nucleus, the angular momentum. • The discovery that the nucleus has an angular momentum, or spin which is associated with a magnetic moment was a result of a detailed study of spectral lines. • The splitting of a spectral line into a number of lines lying close together, is called hyperfine structure. • The properties associated with the hyperfine structure are the mass and angular momentum of the nucleus.

5. The isotope effect is not enough to explain the hyperfine structure. The hyperfine structure can be accounted for quantitatively assuming that the nucleus has an angular momentum. •  The nuclear angular momentum is a vector, I, of magnitude • |I|= sqrt [i(i+1)] h/2π • Where iis the quantum number defines I • According to the rule • Iz = i h/2π • The value of I has been found experimentally to depend on the mass number A of the nucleus. • If A is even: I is an integer or0,1,2,3,… • If A is odd:I is an odd half integral value 1/2, 3/2 ,5/2 ,…. • This rule leads to one of the failures of the proton-electron hypothesis.

6. Example: 7N14 • Atomic no. =7 , mass no. = 14 • It's nucleus would have 14 protons and 7 electrons under this hypothesis. • A =14 (even numbers) → The contribution of the protons to the angular momentum should be an integral multiple of h/2π . An electron has spin ½ ћ so the contribution of 7 electrons is an odd half integral multiple of h/2π , and the total integral momentum of nitrogen nucleus should be an odd half - integral multiple of h/2π . • Butthe angular momentum of nitrogen nucleus has been found experimentally to be I = 1 , an integer , In contradiction to the value obtained by the proton-electron hypothesis

7. The discovery of the neutron • Rutherford in 1920 suggested that, an electron and proton might be so closely combined as to form a neutral particle which is given the name neutron. • All the methods used for detection of P or e depend on the deflection of the charged particle by M.F or E.F. So, it is difficult to detect the nº. • Chadwick in 1932 demonstrated the existence of neutrons. This discovery led to presently accepted idea that the nucleus is built of protons and neutrons. • 2He4 + 4Be9 → 6C12 + 0n1 • Chadwick detected the neutrons, since these particles, unlike protons, produce no tracks in the cloud chamber and no ionization in the ionization chamber. • These properties + the penetrating power of these particles show that the charge of these particles must be zero, and was identified as Rutherford's neutron.

8. The proton-neutron hypothesis • The discovery of neutron, led to the assumption that every atomic nucleus consist of protons and neutrons. • The neutron-proton hypothesis is consistent with the phenomena of radioactivity. Since there are several there reasons why electrons can not be present in the nucleus, it must be concluded that in β-radioactivity, the electron is created in the act of emission. i.e. as a result of a change of a neutron within the nucleus into a proton, an electron, and a new particle called neutrino. • Exchange of mesons. • In free state they are unstable: • P+n0 + +ve meson (e+) • n0 P+ + -ve meson (e-) • An αparticle can be formed by the combination of two protons and two neutrons. electrons.

9. Note: • The neutron is not regarded as a composite system formed by a proton and an electron. The neutron is a fundamental particle in the same sense that the proton is. The two are sometimes called nucleons in order to indicate their function as the building blocks of nuclei.

10. Additional properties of atomic nucleiThe first property is the statistics to which nuclei are subjected • The properties of protons, neutrons, and electrons (atomic nuclei) cannot be described on the basis of classical statistics, so, two new forms of statistics have been devised, based on quantum mechanics rather than on classical mechanics. • There are the Bose-Einstein statistics. • And Fermi-Dirac statistics. • A nucleon is described by a function of its 3 space coordinates and the value of its spin. (1/2ћ or -1/2ћ) • The Fermi- Dirac statistics apply to systems of particles for which the wave function of the systems is anti symmetrical • I.e. It (changes sign when all of the coordinates of two identical particles are interchanged). • It has been deduced from experiments that: • All nuclei of odd mass no. (A) → obeys the Fermi-Dirac statistics. • And all nuclei of even mass no. → obey the Bose-Einstein statistics.

11. The second property is the parity • A good approximation, the wave function of a nucleus may be expressed as the product of a function of the space coordinates and a function depending only on the spin orientation. •  The motion of the nucleus is said to have even parity if its wave function is unchanged when the space coordinates (x, y, z) are replaced by (-x, -y, -z). I.e. when the nucleus position is reflected about the origin of the x, y, z system of axis. The motion of the nucleus is said to have odd parity if the of its wave function is changed when the space coordinates (x, y, z) are replaced by (-x, -y, -z)

12. Radiation Radiation: The process of emitting energy in the form of waves or particles. Where does radiation come from? Radiation is generally produced when particles interact or decay.A large contribution of the radiationon earth is from the sun (solar) or from radioactive isotopes of the elements . Radiation is going through you atthis very moment! http://www.atral.com/U238.html

13. Radioactivity • By the end of the 1800s, it was known that certain isotopes emit penetrating rays. Three types of radiation were known: • Alpha particles (a) • Beta particles (b) • Gamma-rays (g)

14. Where do these particles come from ? • These particles generally come from the nuclei of atomic isotopes which are not stable. • The decay chain of Uranium produces all three of these formsof radiation. • Let’s look at them in more detail…

15. Note: This is themass number, whichis the number ofprotons plus neutrons Alpha Particles (a) Radium R226 Radon Rn222 p + n n p a (4He) 88 protons 138 neutrons 86 protons 136 neutrons 2 protons 2 neutrons alpha-particle(a) is a Helium nucleus. It’s the same as the element Helium, with the electrons stripped off!

16. Beta Particles (b) Carbon C14 Nitrogen N14 + e- electron (beta-particle) 6 protons 8 neutrons 7 protons 7 neutrons We see that one of the neutrons from the C14 nucleus “converted” into a proton, and an electron was ejected. The remaining nucleus contains 7p and 7n, which is a nitrogen nucleus. In symbolic notation, the following process occurred: n  p + e ( + n) Yes, the same neutrino we saw previously

17. Gamma particles (g) In much the same way that electrons in atoms can be in an excited state, so can a nucleus. Neon Ne20 Neon Ne20 + 10 protons 10 neutrons(in excited state) 10 protons 10 neutrons(lowest energy state) gamma A gamma is a high energy light particle. It is NOT visible by your naked eye because it is not in the visible part of the EM spectrum.

18. Gamma Rays Neon Ne20 Neon Ne20 + The gamma from nuclear decayis in the X-ray/ Gamma ray part of the EM spectrum(very energetic!)

19. Natural radioactivity • It was found that, the product of radioactive decay is it self radioactive. • Radioactive A • Parent • λ1 • Radioactive B • Daughter • B behaves chemically in a different • manner to A and C. • Radioactive C

20. How do these particles differ ? * m = E / c2

21. Types of Ionizing Radiation Alpha Particles Stopped by a sheet of paper Radiation Source hazard Beta Particles Stopped by a layer of clothing or less than an inch of a substance (e.g. plastic) Gamma Rays Stopped by inches to feet of concrete or less than an inch of lead

22. Radiation Types - Alpha • An alpha particle consists of two protons and two neutrons • Very large on an atomic scale • Positively charged • Penetration in materials • Outside the body, an alpha emitter is not a hazard unless it is on the skin • Inside the body, an alpha emitter is a bigger hazard if it deposits its energy in sensitive tissue

23. Radiation Types - Alpha • Common alpha-particle emitters • Radon-222 gas in the environment • Uranium-234 and -238) in the environment • Polonium-210 in tobacco • Common alpha-particle emitter uses • Smoke detectors • Cigarettes/cigars • Static eliminators

24. Radiation Types - Beta • A beta particle is a charged electron • Has the size and weight of an electron • Can be positively or negatively charged • Penetration in materials • At low energies, a beta particle is not very penetrating – stopped by the outer layer of skin or a piece of paper • At higher energies, a beta particle may penetrate to the live layer of skin and may need 0.5” of plexiglass to be stopped

25. Radiation Types - Beta • Penetration in materials, continued • Inside the body, a beta particle is not as hazardous as an alpha particle because it is not as big • Because it is not as big, it travels farther, interacting with more tissue (but each small piece of tissue gets less energy deposited)

26. Radiation Types - Beta • Common beta-particle emitters • Tritium (hydrogen-3) in the environment • Carbon (14) in the environment • Phosphorus (32) used in research and medicine • Common beta-particle emitter uses • Carbon dating • Basic research • Cancer treatment

27. Radiation Types - Photon • A photon is an x or gamma ray • Has no weight • Has no charge • Penetration in materials • At low energies, a photon can be stopped by a very thin (almost flexible) layer of lead or several centimeters of tissue • At higher energies, inches of lead might be necessary to stop a photon and they can pass right through a human

28. Radiation Types - Photon • Common photon emitters • Cesium (137) • Technetium (99m) used in medicine • Iodine (131) used in medicine • Common photon emitter uses • Determining the density of soil • Diagnosing disease • Cancer treatment

29. Photon Decay 99Tc 99mTc Gamma ray Stable Nucleus Excited Nucleus