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Isotopes.ppt
- 1. Isotopes atoms of a given element that differ in the number of neutrons …and consequently in mass.
- 2. Definition of Isotopes Isotopes are atoms of the same element which contains the same number of protons but different number of neutrons.
- 3. Isotopes 16 8 mass number proton number OO O Oxygen-16 n = 8 Oxygen-17 Oxygen-18 17 18 8 8 n = 17 – 8 = 9 n = 18 – 8 = 10
- 4. Isotopes Isotopes have the same chemical properties but slightly different physical properties
- 5. element have the Q. Do all isotopes of the same same mass?
- 6. Working with Atomic Notation A zX Atomic Number Chemical Symbol Atomic Mass (of Isotope)
- 7. Example #1 12 6C Atomic Number Chemical Symbol Atomic Mass (of Isotope)
- 8. Example #2 13 6C Atomic Number Chemical Symbol Atomic Mass (of Isotope)
- 9. Example #3 14 6C Atomic Number Chemical Symbol Atomic Mass (of Isotope)
- 10. Some isotopes of carbon 12 6C 13 6C 14 6C
- 11. Isotopes of Some Elements and Their Atomic Mass
- 13. Various ways of identifying Isotopes • Using atomic notation, Example: 12 6 C or simply 12 C •Using the mass notation. Example: Carbon-12 or C-12 (read “carbon twelve” or “C twelve”)
- 14. Some Isotopes of Carbon mass notation atomic notation # of p+ # of e- # of no C-11 11C 6 6 C-12 12C 6 6 C-13 13C 6 6 C-14 14C 6 6
- 15. Another example of isotopes 1 1H 2 1H 3 1H or H-1 H-2 H-3
- 16. The Isotopes of Hydrogen mass notation atomic notation # of p+ # of e- # of no Hydrogen-1 1H 1 1 Hydrogen-2 2H 1 1 Hydrogen-3 3H 1 1
- 17. p+ = no = e- = p+ = no = e- = p+ = no = e- = Figure #1 Figure #2 Figure #3
- 18. Isotopes atoms of a given element that differ in the number of neutrons …and consequently in mass.
- 19. Keep in mind: It is not possible to determine how many different isotopes exist by looking at the periodic table. It is not possible to determine the frequency of various nuclides by looking at the periodic table.
- 20. (parenthesis) on the Periodic Table indicate the most stable isotope stable means “longest living” Parenthesis also suggest the element of interest is radioactive.
- 21. Review problem #1 Represent the following using atomic notation. 92 U Uranium 238.0289
- 22. Review problem #2 Represent the following using mass notation. 10 Ne Neon 20.1797
- 23. Review problem #4 How many total subatomic particles are in the following “neutral” atoms of Fe-55 and Fe-57?
- 24. RADIO ISOTOPES Parent isotope Radioactive decay heat Daughter isotope
- 25. Stable vs. Unstable • A stable isotope does NOT undergo radioactive (or nuclear) decay. • An unstable isotope undergoes radioactive (or nuclear) decay. Unstable isotopes are also known as radioisotopes or radionucleides
- 26. Stable vs. Unstable • Stable isotopes: • They do not naturally decay but exist in natural materials in differing proportions. • Unstable isotope • Isotopes that continuously break down into lower atomic weight isotopes.
- 27. Uses of Radioactive Isotopes • Food irradiation • Archaeological dating (carbon- dating) • Smoke detectors • Radioactive tracers
- 30. Represent the following using ATOMIC NOTATION 17 Cl Chlorine 37.65 8 O Oxygen 17.999 92 U Uranium 235.0289 6 C Caarbon 14.011 9 F Flourine 14.998
- 31. Represent the following using MASS NOTATION 27 Co Cobalt 60.998 33 As Arsenic 72.922 92 U Uranium 235.0289 53 I Iodine 131.404 11 Na Sodium 24.989
- 32. The Isotopes How many total subatomic particles are in the following: Complete the table. mass notation atomic notation # of p+ # of e- # of no Lead-208 82 199Au Bismuth-211 83
- 34. The Isotopes How many total subatomic particles are in the following: Complete the table. mass notation atomic notation # of p+ # of e- # of no Lead-208 208Pb 82 82 126 Gold-199 199Au 79 79 120 Bismuth-211 211Bi 83 83 128