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1. 1. <ul><li>TRUE OR FALSE </li></ul><ul><ul><li>1. As the sample of radioactive </li></ul></ul><ul><ul><li>decays, it half life decreases. </li></ul></ul>
2. 2. <ul><li>TRUE OR FALSE </li></ul><ul><ul><li>2. As the half life increasers the mass of the radioactive material increases </li></ul></ul>
3. 3. <ul><li>TRUE OR FALSE </li></ul><ul><ul><li>3. The time required for half a radioactive sample to disintegrate is called half life. </li></ul></ul>
4. 4. <ul><li>TRUE OR FALSE </li></ul><ul><li>5. Half life is constant to all </li></ul><ul><li>radioactive substance </li></ul>
5. 5. <ul><li>TRUE OR FALSE </li></ul><ul><li>4. Decay constant defined as the fraction of the number of atom decay in a unit time. </li></ul>
6. 6. Nuclear Decay
7. 7. The Atom- Review <ul><li>The atom consists of two parts: </li></ul>1. The nucleus which contains: 2. Orbiting electrons. protons neutrons <ul><li>Atom of different elements contain different numbers of protons. </li></ul><ul><li>The mass of an atom is due to the number of protons and neutrons. </li></ul>
8. 8. X A Z Mass number Atomic number Element symbol = number of protons + number of neutrons = number of protons Isotope Symbol Review A = number of protons + number of neutrons Z = number of protons A – Z = number of neutrons **Number of neutrons = Mass Number – Atomic Number**
9. 9. Fill in the chart for each isotope 235 92 92 143 92 92 238 146 Isotopes of any particular element contain the same number of protons, but different numbers of neutrons. U 235 92 U 238 92 A Z Number of protons Number of neutrons A Z Number of protons Number of neutrons
10. 10. <ul><li>Most of the isotopes which occur naturally are stable . </li></ul><ul><li>A few naturally occurring isotopes and all of the man-made isotopes are unstable . </li></ul><ul><li>Unstable isotopes can become stable by releasing different types of particles. </li></ul><ul><li>This process is called radioactive decay and the elements which undergo this process are called radioisotopes. </li></ul><ul><li>The products of this decay are called daughter isotopes </li></ul>
11. 11. Radioactive decay results in the emission of either: <ul><li>an alpha particle (  ), </li></ul><ul><li>a negative beta particle (electron) (   ), </li></ul><ul><li>or a gamma ray  </li></ul>Radioactive Decay <ul><li>a positive beta particle (positron) (   ), </li></ul>In a nuclear reaction the MASS and ATOMIC NUMBER must be the SAME on both sides of the equations
12. 12. An alpha particle is identical to that of a helium nucleus. It contains two protons and two neutrons. Alpha Decay unstable atom more stable atom alpha particle X A Z Y A - 4 Z - 2 + He 4 2
13. 13. Alpha Decay + Loss of 2 protons & 2 neutrons: Atomic # decreases by 2 Mass # decreases by 4 Ra 226 88 Rn 222 86 He 4 2
14. 14. Write your own Alpha Decay What is Y? X A Z Y A - 4 Z - 2 + He 4 2 Rn 222 86 + Y A Z He 4 2 Rn 222 86 He 4 2 + Po 218 84 He 4 2
15. 15. Write the equation for the alpha decay of Uranium-234 U 234 + He 4 2 U 234 92 + Th 230 90 He 4 2
16. 16. Find the missing starting material X A Z + Pb 214 82 He 4 2 He 4 2 + Pb 214 82 He 4 2 Po 218 84
17. 17. Beta Emission A beta particle is a fast moving electron which is emitted from the nucleus of an atom undergoing radioactive decay. Beta emission occurs when a neutron changes into a proton and an electron . b eta particle (electron) proton stays in nucleus X A Z Y A Z + 1 + e 0 -1
18. 18. Beta Emission + <ul><li>Neutron splits emitting negative particle leaving a proton. </li></ul><ul><ul><li>Atomic # increases by 1 </li></ul></ul><ul><ul><li>Mass # stays the same </li></ul></ul><ul><li>(electrons have no mass) </li></ul>Po 218 84 e 0 -1 At 218 85
19. 19. Write your own Beta Emission What is Y? X A Z Y A Z + 1 + e 0 -1 Th 234 90 Y A Z + e 0 -1 Th 234 90 Pa 234 91 + e 0 -1
20. 20. Write the equation for the beta e mission of carbon-14 C 14 + C 14 N 14 7 + e 0 -1
21. 21. Find the missing starting material X A Z Bi 214 83 + e 0 -1 Pb 214 82 Bi 214 83 + e 0 -1
22. 22. Electron Capture is the opposite of Beta Emission Electron Capture The capture of the electron allows a proton to turn into a neutron X A Z e 0 -1 + Y A Z-1
23. 23. Electron Capture + <ul><li>Capture negative particle, forming a neutron from a proton </li></ul><ul><ul><li>Atomic # decreases by 1 </li></ul></ul><ul><ul><li>Mass # stays the same </li></ul></ul><ul><li>(electrons have no mass) </li></ul>Po 218 84 e 0 -1 At 218 85
24. 24. Write your own Electron Capture What is Y? X A Z e 0 -1 + Y A Z-1 Ar 37 18 e 0 -1 + Y A Z-1 Ar 37 18 e 0 -1 + Cl 37 17
25. 25. Write the equation for electron c apture of nickel-59 Ni 59 + Ni 59 28 e 0 -1 + Co 59 27
26. 26. Find the missing starting material X A Z e 0 -1 + C 14 6 N 14 7 e 0 -1 + C 14 6
27. 27. Positron Emission A positron is like an electron but it has a positive charge. During positron emission a proton changes into a neutron and the excess positive charge is emitted . positron mass stays in nucleus X A Z Y A Z - 1 + e 0 +1
28. 28. Positron Emission + <ul><li>Proton splits emitting positive particle leaving a neutron. </li></ul><ul><ul><li>Atomic # decreases by 1 </li></ul></ul><ul><ul><li>Mass # stays the same </li></ul></ul><ul><li>(positrons, like electrons, have no mass) </li></ul>Po 218 84 e 0 +1 At 218 85
29. 29. Write your own Positron Emission What is Y? X A Z Y A Z - 1 + e 0 +1 B 8 5 Y A Z + e 0 +1 B 8 5 Be 8 4 + e 0 +1
30. 30. Write the equation for the positron e mission of oxygen-16 O 16 + O 16 N 16 7 + e 0 +1
31. 31. Find the missing starting material X A Z Cu 66 29 + e 0 +1 Zn 66 30 Cu 66 29 + e 0 +1
32. 32. Gamma Decay <ul><li>Gamma rays are not charged particles like  and  particles. </li></ul><ul><li>Gamma rays are high energy radiation </li></ul><ul><li>When atoms decay by emitting  or  particles to form a new atom, the nuclei of the new atom formed may still have too much energy to be completely stable. These atoms will emit gamma rays to release that energy. </li></ul><ul><li>There is no change in mass or atomic number </li></ul>X A Z X A Z +  0 0
33. 33. Summary Reaction What happens? Mass # Atomic # Alpha Decay  Lose Helium Nucleus -4 -2 Beta Decay  - Lose electron from nucleus (neutron turns into proton) No change +1 Electron Capture Gain electron in nucleus (proton turns into neutron) No change -1 Positron Emission   Lose positron (proton turns into neutron) No change -1 Gammy Decay  Emit high energy gamma ray No change No change
34. 34. Nuclear Stability <ul><li>The strong nuclear force holds all nuclei together </li></ul><ul><ul><li>Otherwise protons would repel each other </li></ul></ul><ul><ul><li>Neutrons space out protons and make nucleus stable </li></ul></ul><ul><li>Not all isotopes are radioactive </li></ul><ul><li>Only unstable nuclei decay </li></ul><ul><li>In smaller atoms stable isotopes have equal numbers of protons and neutrons </li></ul><ul><li>In larger atoms stable isotopes will have more neutrons than protons </li></ul><ul><li>Too many or too few neutrons makes the nucleus unstable </li></ul>
35. 35. Nuclear Stability Graph Dark band = stable nucleus Areas off line = radioactive
36. 36. Fission <ul><li>Fission is when a nucleus splits </li></ul><ul><ul><li>This is what happens in nuclear power plants </li></ul></ul><ul><li>Neutrons emitted during fission reactions can cause other fission reactions </li></ul><ul><ul><li>This is a chain reaction </li></ul></ul><ul><li>In a nuclear reactor the chain reaction is controlled with control rods </li></ul>
37. 37. Chain Reaction <ul><li>Each reaction allows multiple other reactions to occur </li></ul><ul><li>Controlled vs Uncontrolled </li></ul>
38. 38. Fusion <ul><li>When two or more elements fuse (combine) to form one new heavier element </li></ul><ul><li>The energy released by the sun and all stars is due to fusion reactions in the core </li></ul><ul><li>This process releases more energy than fission </li></ul><ul><li>Fusion reactions are hard to contain because the reactants are a plasma and at very high temperatures, no solid material can contain a plasma </li></ul>
39. 39. Fission Fusion Nuclei combine Nucleus splits End product is heavier than reactants End product is lighter than reactants Energy is released LOTS of energy released Can’t contain reaction Reaction can be harnessed Nuclear Change