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Do Now

Do Now. Draw a bohr model for Boron. Do Now. Describe what makes a source reliable and accurate?. Atomic Number, Atomic Mass, and Isotopes. Happy Pt Tuesday!!!!. By the end of the class today I will be able to…. Student will understand the symbol for an isotope.

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Do Now

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  1. Do Now • Draw a bohr model for Boron

  2. Do Now • Describe what makes a source reliable and accurate?

  3. Atomic Number, Atomic Mass, and Isotopes Happy Pt Tuesday!!!!

  4. By the end of the class today I will be able to… • Student will understand the symbol for an isotope

  5. If we made a scale model of an atom and wanted to use Cowboy Stadium as our electron cloud, the nucleus of the atom would be the size of the eraser on the end of your pencil. An electron would still be smaller than the point on a straight pin.

  6. What do these boxes mean?? Number of protons/ Atomic Number All atoms of the same element have the same number of protons

  7. Mass Number p+ e- n0 Number of Protons, Neutrons, & Electrons # Protons = How to Use the Periodic Table # Electrons = # Neutrons = - = Example 1: Argon

  8. Isotope Symbol X: element symbol

  9. Isotope Symbol A: Mass Number #protons + # neutrons in the nucleus Always larger than Z

  10. Isotope Symbol Z: Atomic number #protons

  11. 2 Ways to write Isotope Symbol Or Sodium-23 Na 23 11

  12. Isotopes of Sodium Na Na 23 24 11 11

  13. Example Problem • Write the nuclear notation for the chemical element that has 6 protons and 8 neutrons

  14. #1 • Write the Nuclear notation for the chemical element that has 17 protons and 16 neutrons (in your table) Clor Chlorine-33 33 17

  15. #2 How many protons are in the isotope 54Cr? (Chromium-54) (add it to your table) 24 (like every atom of Chromium)

  16. #3 How many neutrons are in the isotope 42Ca? Number or protons? (add it to your table) 22 neutrons

  17. #4 How many electrons are in the isotope 23Na? Write it’s nuclear notation (add to table) 11 electrons

  18. Average Mass of Subatomic Particles Atomic Mass Unit 1 amu= 1.66 x 10-24 g

  19. x # e- # p+ # n0 Mass of n0 Mass of p+ Protons Example Example 7: Mass of Beryllium x x + + + + = = Mass of e- Neutrons Electrons 4 Protons 4 Electrons 5 Neutrons

  20. Example 2 & 3 Sodium Fluorine

  21. Gallery walk • Walk around to the different pictures of isotopes • Identify which isotope it is and fill out the information in your packet • Figure out – WHAT IS THE DIFFERENCE?

  22. Definition Examples Isotope Non-Examples Drawing or Traits iSOTOPE

  23. Atoms of the same element with different numbers of neutrons (therefore have different masses). Isotopes

  24. COMPARE/CONTRAST

  25. Four Isotopes of helium What sub-atomic particle(s) are the same for the isotopes of Helium? What sub-atomic particle(s) are different for the isotopes of Helium? Are these four isotopes neutral? Why or Why not?

  26. Workout! Write the following as an isotope symbol… 4. Copper-63 5. Copper-64 6. Lithium-7 7. Lithium-6

  27. Example Problem • How many neutrons are in the isotope of 26Mg? Number of Neutrons = A-Z

  28. #1 How many neutrons are in the isotope 48Ti? 26 neutrons

  29. Example Problem How many electrons are in the isotope 23Na? (you can assume the atom is neutral) 11 electrons

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