Lecture 1: RDCH 702 Introduction

1. Lecture 1: RDCH 702 Introduction • Class organization • Outcomes • Grading • Chart of the nuclides • Description and use of chart • Data • Radiochemistry introduction • Atomic properties • Nuclear nomenclature • X-rays • Types of decays • Forces

2. RDCH 702: Introduction • Outcomes for RDCH 702 • Understand chemical properties in radiation and radiochemistry • Use and application of chemical kinetics and thermodynamics to evaluate radionuclide speciation • Understand the influence of radiolysis on the chemistry of radioisotopes • Understand and evaluate radioisotope production • Evaluate and compare radiochemical separations • Utilization of radioisotope nuclear properties in evaluating chemical behavior • Use and explain the application of radionuclides in research • Discuss and understand ongoing radiochemistry research

3. Grading • Homework (25 %) • Weekly homework questions • Develop tools for research (spreadsheets) • Two exams (30 % each) • Oral exam • 30 minutes each • 1st exam on question from course information • 2nd exam on literature • Classroom participation (15 %) • Bring chart of the nuclides! • Class developed to assist and compliment research activities

4. Chart of the Nuclides • Presentation of data on nuclides • Information on chemical element • Nuclide information • Spin and parity (0+ for even-even nuclides) • Fission yield • Stable isotope • Isotopic abundance • Reaction cross sections • Mass • Radioactive isotope • Half-life • Modes of decay and energies • Beta disintegration energies • Isomeric states • Natural decay series • Reaction cross sections

5. Chart of Nuclides • Decay modes • Alpha • Beta • Positron • Photon • Electron capture • Isomeric transition • Internal conversion • Spontaneous fission • Cluster decay

6. Introduction • Radiochemistry • Chemistry of the radioactive isotopes and elements • Utilization of nuclear properties in evaluating and understanding chemistry • Intersection of chart of the nuclides and periodic table • Atom • Z and N in nucleus (10-14 m) • Electron interaction with nucleus basis of chemical properties (10-10 m) • Electrons can be excited • Higher energy orbitals • Ionization • Binding energy of electron effects ionization • Isotopes • Same Z different N • Isobar • Same A (sum of Z and N) • Isotone • Same N, different Z • Isomer • Nuclide in excited state • 99mTc

7. X-rays • Electron from a lower level is removed • electrons of the higher levels can come to occupy resulting vacancy • energy is returned to the external medium as electromagnetic radiation • radiation called an X-ray • discovered by Roentgen in 1895 • In studying x-rays radiation emitted by uranium ores Becquerel et. al. (P. and M. Curie) discovered radioactivity in 1896

8. X-rays • Removal of K shell electrons • Electrons coming from the higher levels will emit photons while falling to this K shell • series of rays (frequency n or wavelength l) are noted as Ka, Kb, Kg • If the removed electrons are from the L shell, noted as La, Lb, Lg • In 1913 Moseley studied these frequencies n, showing that: • where Z is the atomic number and, A and Z0 are constants depending on the observed transition. • K series, Z0 = 1, L series, Z0 = 7.4.

10. Absorption Spectra • Edge keV A • K 115.6061 0.1072 • L-I 21.7574 0.5698 • L-II 20.9476 0.5919 • L-III 17.1663 0.7223 • M1 5.5480 2.2348 • M2 5.1822 2.3925 • M3 4.3034 2.8811 • M4 3.7276 3.3261 • M5 3.5517 3.4908 • N1 1.4408 8.6052 • N2 1.2726 9.7426 • N3 1.0449 11.8657 U absorption edges and scattering coefficients

11. Fundamentals of x-rays • X-rays • X-ray wavelengths from 1E-5 angstrom to 100 angstrom • De-acceleration of high energy electrons • Electron transitions from inner orbitals • Bombardment of metal with high energy electrons • Secondary x-ray fluorescence by primary x-rays • Radioactive sources • Synchrotron sources

12. Types of Decay 1.  decay (occurs among the heavier elements) 2.  decay 3. Positron emission 4. Electron capture 5. Spontaneous fission

13. Half Lives for the condition: N/No=1/2=e-t N=Noe- t =(ln 2)/t1/2 Rate of decay of 131I as a function of time. http://genchem.chem.wisc.edu/sstutorial/FunChem.htm

14. Forces in nature • Four fundamental forces in nature • All interactions in the universe are the result of these forces • Gravity • Weakest force • most significant when the interacting objects are massive, such as planets, stars, etc. • Weak interaction • Beta decay • Electromagnetic force • Most observable interactions • Strong interaction • Nuclear properties

15. Fundamental Forces

16. Classic and relativistic

17. Use of relativistic terms • relativistic expressions • photons, neutrinos • Electrons > 50 keV • nucleons when the kinetic energy/nucleon exceeds 100 MeV

18. Wavelengths and energy • Planck evaluated minimum from DExDt when he studied the radiation emitted by a black body at a given temperature • Quantum called Planck’s constant h (h = 6.6 10-34 J.s). • radiation conveys energy E in the form of quanta E = hn • n the frequency of the emitted radiation • Based on the wave mechanics worked out by de Broglie • l = h/p • l is the wavelength associated with any moving particle with the momentum p

19. Wavelengths • Photon relationships

20. Particle Physics • fundamental particles of nature and interaction symmetries • Particles classified as fermions or bosons • Fermions obey the Pauli principle • antisymmetric wave functions • half-integer spins • Neutrons, protons and electrons • Bosons do not obey Pauli principle • symmetric wave functions and integer spins • Photons

22. Particle physics • Particle groups divided • leptons (electron) • hadrons (neutron and proton) • hadrons can interact via the strong interaction • Both can interact with other forces • Fermionic Hadrons comprised of quarks