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1. 1. Dr. Kamal K. Ali University of Baghdad College of science Geology 2nd year Radioactivity & Isotopes geology Lecture 1• Atom stracture.• Nuclides• Elements , isobars, isotones, isotopes
2. 2. Matter is made up of very small particles called atoms • Each atom has a very small and very dense core called nucleus. • Most of the mass of atom is contained in the nucleus• A proton has a unit positive charge.• A neutron is an uncharged particle.• An electron has a negative charge.
3. 3. • The electrons move in orbits around the nucleus. • There are a lot of empty spaces within atom • A Atom nucleus consists of a number of protons and neutrons. • Protons and neutrons also known as mass number (nucleons).Nucleus Z electrons Z protons Nucleus structure A Z X A mass number (nucleons) = Z + N N neutrons
4. 4. Dimentions Diameter of Nucleus isand range of 1.75 fm- 15 fm fm=10-15mDistance 1cm 100m 500m
5. 5. Neutron slightly heavier than protonMasses Mass n=1.67495x10-27 Kg Mass p= 1.67265x10-27 kg Mass p> mass e about 1836 timesSuppose the mass of the electron 1g… … then the mass of the nucleus is 108 Tonnes
6. 6. What is nuclide?• A nuclide is an atom of a particular structure. Each element has nucleus with a specific number of protons. A• Nuclide notation 12• Example 6C , ZX1• Proton 1p , Neutron 0 n , electron -1e 1 0
7. 7. Elements- Isotopes-IsobarNumber of p (Z) = atomic number. It determines the chemical element.Ex. Z=92 is Uranium, Z=90 is Thorium Z= 86 Radium Z=27 CobaltNumber of Neutron (N)Mass number OR nucleon number(A)=Z+NNumber of electron=number of proton(It impacts chemical reaction)
8. 8. • Thommson,1914, Aston, 1919:(There are different mass number(A) for a given (Z) for an element. That is mean they have different (N)……..THEY ARE ISOTOPES.Isotopes: Greek phrase : isos topos meaning :“The same place” isotopes of the same elements occupy the same position in periodic table.
9. 9. Isotopes
10. 10. Oxygen (3 isotopes) 17 Nucleon number = 17 Atomic number = 8Nucleon number = 16 Atomic number = 8 Nucleon number = 18 Atomic number = 8
11. 11. Hydrogen (3 isotopes) Nucleon number = 2 Atomic number = 1Nucleon number =1Atomic number = 1 Nucleon number = 3 Atomic number = 1
13. 13. Nuclides with same mass(nucleon) numbers(A)but with slightly different # of protons(Z). 87• Ex: Rubidium 37Rb&Strontium38Sr. 87 12 12• Carbon -12 6C and Boron-12 5B
14. 14. 3 basic Location charge commentsparticlesprotonneutronElectron
15. 15. Number of No. of No. of Term (Z) (A) (N)isotopesisobarsisotones
16. 16. • Isotopes either Stable or Unstable(Radioactive) 59• Co, H, H, O, O : 1 2 16 18 Stable Isotopes; 60• Co, H,: Radioactive 3 (Radioisotope)
17. 17. Radioactivity• Radioactivity was discovered and studied by Henri Becquerel and then Pierre and Marie Curie from 1896 to 1902.• Radioactivity is the phenomenon by which certain nuclei transform (transmute) spontaneously into other nuclei and give off particles or radiation to satisfy the laws of conservation of energy and mass.• Proton is made of pieces called quarks(2up, 1down).• When proton breaks apart it produces high energitic pieces.• So radioactivity is explosion of the nucleus of an atom.
18. 18. Radioactivity and Radiation• When we have a radioactive nucleus exploding, the pieces is going flying out with energy a typically have 1 MeV. And some with 2MeV., WHILE IN CHEMICAL REACTION of hydrogen and oxygen the energy product about 1 eV.• This the dangerous of radioactivity and this is the advantage of radioactivity.• The pieces come out when a nucleus explode we called them radiation.(radioactivity=explosion, Radiation=pieces come out).
19. 19. Lecture 3: Mechanism of radioactive decay and types of radiation• Radioactive decay is a nuclear process and is independent of chemical and physical states of nuclide. It depends on the neutron/proton ratio and on the mass-energy relationship of the parent, daughter and emitted particles.• For the nuclides of low atomic mass, the greatest stability is achieved when the number of neutrons and protons are approximately equal(N=Z), but as atomic mass increase, the neutron/proton ratio increase until N/Z=1.5
20. 20. Lecture 2: Radioactivity and Stability Elements for which Z is an even number have far more isotopes than elements for which Z is an odd number. Fluorine (Z=9), sodium (Z=11), phosphorus (Z=15), and scandium(Z=21) have just a single isotope.The distribution of natural stable isotopes in the neutron–protondiagram. After N=20, the zone of stable nuclei moves away from thediagonal for which the number of neutrons equals the number ofprotons. For N>20, the number of neutrons then exceeds the number ofprotons. This zone is called the valley of stability as it corresponds to aminimum energy level of the nuclides.
21. 21. Mechanism of radioactive ,Type of Radiation 41-Alpha particle (a helium nucleus 2He) • For the nuclides of high atomic mass such as U-238 are unstable. U-238 have 146 neutrons and 92 protons. So its nucleus emits Alpha particles (α) to reach the stability. Alpha particle is (two protons and two neutrons) positive charge(+2). In this case number of protons and neutrons in the nucleus reduces by two for each. So it becomes 90 proton and 144 neutron and the new nuclide is Thorium-234. we can express it as follow: 234 92U α + 90Th 2:146 2:92 238 4 2
22. 22. Alpha particles• The particles have large kinetic energies but are rapidly slowed down by collisions with other atomic nuclei. At thermal energies they soon gain two orbital electrons and become indistinguishable from other helium atoms.• The average distance travelled in solid rock before this occurs is measured in fractions of a millimeter.
23. 23. Beta-minus particle• Alpha emission produces nucleus rich in neutrons and deficient in protons and still unstable. So a neutron disintegrates into a proton and an electron. The electron expelled from the nucleus as a negative particles called Beta particle(β-), They differ from other electrons only in having higher kinetic energies. To satisfy the law of conservation of energy and mass, it is assumed that the nucleus emits energy particles has no mass nor charge called an antineutrino along with the electron. The decay equation is written : 1 1• 0n p + β- + v 1• neutron -------------- proton + electron + antineutrino.• So in Th-234 it decays to Pa-234 by emitting β- as follow: 234 234 90 Th 91 Pa + β- + v
24. 24. Gamma ray• In many cases the nuclide produced by beta minus decay is left in an exited state, which subsequently decay to the ground state nuclide by release of energy. This may be lost as gamma (γ) ray(electromagnetic ray) of discrete energy. A A z P* z P + e- (mission of photon)• The metastable state or “ Isomers” of the product nuclide are denoted by super fix ‘m’
25. 25. Beta-plus and electron capture• Nuclides deficient in neutrons e.g. K-38 may decay by two different processes: positron emissionElectron capture.Both processes yield a product nuclide that isobar of the parent, by transformation of a proton into neutron1 1 p n + β+ + v 1 0proton neutron + β+ + neutrino
26. 26. Electron capture• A nuclear proton is transform into a neutron by capture of an orbital electron, usually from the inner shells. 1 1 p + e- n + β+ + v 1 0Outer orbital electron falls into the vacancy produced by electron capture, emitting a characteristic X-ray. The product nucleus may be left in exited state, in which case it decays to the ground state by gamma emission (γ).Gamma rays and X- rays are both electromagnetic rays , they are differ where they are produced.
27. 27. Isotopes measurement The Mass Spectrometer (MS)• “There would be no isotope geology without MS”.• The principle of MS. Atoms of the chemical element whose isotopic composition is to be measured are ionized in a vacuum chamber. The ions produced are accelerated by using a potential difference of 3-20 kV. This produces a stream of ions , and so an electric current. This electric current is passed through a magnetic field.
28. 28. Isotopes measurement The Mass Spectrometer (MS)The magnetic field exert a force perpendicular to the electric current and so bends the beam of ions.The lighter ions are deflected more than the heavier ones and so the ions can be sorted according to their mass.So, the relative abundance of each isotope can be measured from the relative values of the electron currents produced by each stream of ions separated out by this way.
29. 29. The Mass Spectrometer (MS)1. The source: 2. Magnet: It deviates the ions andTo generate ions from atoms. this deflection separates them byTo accelerate the ion by potential mass. differences. 3. Collectors: collect and integrateTo shape the beam, through the ion charges so generating an calibrated slits in the high electric current. voltage plates. all of which are maintained under vacuum.
30. 30. Short Quiz• Decide which of these nuclei are stable or unstable: 235 223 12 241. 92 U 2.88 Ra 3. C 4. Mg 6 12 128 225. 53 I 6. 10Ne
31. 31. Isotopes measurement The Mass Spectrometer (MS)• Suppose atoms of the element in question have been ionized. The ion acceleration is: 2eV =1/2mν eV : electric energy 2e:ion charge 1/2mν : kinetic energym: mass of the ionν: its speed…………….then 1/2ν = (2eV/m)
32. 32. The Mass Spectrometer (MS)• Magnetic deflection is given by equating the magnetic force Beν to centripetal acceleration (ν2/R)multiplied by mass m, where B is the magnetic field and R the radius of curvature of the deflected path:Beν=(ν2/R)m……where B=magnetic fieldNote: when a charge particle moves through a magnetic field: Magnetic force F= magetic field(B) X electical charge(e) X its velocity(ν)………THEN:νBeR= ν2m
33. 33. The Mass Spectrometer (MS)ν= BeR/m ….. Then 1/2BeR/m= (2eV/m) B2 e2 R2/m2= 2eV/m …. B2 e2 R2m= m22eVm/e= B2R2/2VIn which B in tesla, R in meters, m in atomic mass, and V in Volts. Atomic mass unit m= 1.6605402 X10-27 kg Electron charge e = 1.60219 X10-19 coulombs
34. 34. Exercises• A mass spectrometer has a radius of 0.3m and an acceleration voltage of 10 000 V. The magnetic field is adjusted to the various masses to be measured. Calculate the atomic mass corresponding to a field of 0.5 T.• Answer: Just apply the formula with suitable units:• m= (B2R2/20721V) X 1012 = (0.5)2x(0.3)2x1012/20721x10000=108.58
35. 35. Exercises• If hydrogen ions (mass number=1) are accelerated with a voltage of 10 kV, at what speed are they emitted from the source? 1/2• Answer Just apply the formula : ν = (2eV/m) Atomic mass unit m= 1.6605402 X10-27 kg Electron charge e = 1.60219 X10-19 coulombsν= (1.9272x1012)1/2 = 1388 km/s
36. 36. Ionization techniques1. Thermal-ionization mass spectrometry.2. Electronic bombardment.3. Inductively coupled plasma mass spectrometry(ICP-MS).4. Ionic bombardment in secondary ion mass spectrometry(SIMS)
37. 37. Short Quiz• Two of the isotopes of the element whose atomic number is 10 have mass numbers of 20 and 22.• Write the symbol of each isotope. – How many protons does each of the isotopes have? – How many neutrons does the isotope with mass number 20 have? How about for the other one?
38. 38. R = Abundance of Heavy isotope (rare)/ abundance of light isotope
39. 39. sample standard standard
40. 40. 3 Tritium H• Tritium H values reported as 3 absolute concentration called Tritium Unit (TU), where on TU corresponded to I tritium atom per 108 hydrogen atoms. Tritium values may also be expressed in terms of activity (pCi/l), where 1TU= 3.2 pCi= 7.2 dpm/l
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