10/13 Review: What is electronegativity and ionization energy?

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10/13 Review: What is electronegativity and ionization energy?

  1. 1. Launch   Grab your binder and immediately take a seat   Answer the following questions: 1.  Using arrows, draw the trend for atomic radius. 2.  Which atoms below have a larger atomic radius than aluminum (Al)? i)  Cl iii) Si v) Na ii) B iv) He vi) Ca
  2. 2. Weekly Schedule   Monday: Atomic Radius   Tuesday: Electronegativity & Ionization Energy   Wednesday: Metals, nonmetals, special groups   Thursday: Atomic structure & nuclear processes   Friday: Mid-Term Exam We don’t have much time! If you don’t understand something, ask!
  3. 3. What is the trend in ionization energy/ electronegativity? Mr. Heffner 10/13/09
  4. 4. Ionization Energy   Ionization energy is…   how much energy it takes to steal an electron
  5. 5. Electronegativity   Electronegativity is…   how good an atom is at stealing electrons
  6. 6. Ionization Energy/Electronegativity   The trend: 1.  IE/E increases across a period (LR) 2.  IE/E decreases down a group (Top  Bottom) Increases Decreases
  7. 7. Example #1 Which has higher amount of ionization energy, oxygen (O) or carbon (C)?   Step #1: Find the elements
  8. 8. Example Which has higher amount of ionization energy, oxygen (O) or carbon (C)?   Step #2: Look at the keywords Which has a higher amount of ionization energy, oxygen (O) or carbon (C)?
  9. 9. Example Which has higher amount of ionization energy, oxygen (O) or carbon (C)?   Step #3: Identify which is closest to He
  10. 10. Example Which is less electronegative, Beryllium (Be) or potassium (K)?   Step #1: Find the elements
  11. 11. Example Which is less electronegative, Beryllium (Be) or potassium (K)?   Step #2: Look at the keyword Which is less electronegative, Beryllium (Be) or potassium (K)?
  12. 12. Example Which is less electronegative, Beryllium (Be) or potassium (K)?   Step #3: Identify which is closest to Fr
  13. 13. Practice Questions   Review Worksheet #2   Use the 3-step method!
  14. 14. Ionization Energy/Electronegativity   The trend: 1.  IE/E increases across a period (LR) 2.  IE/E decreases down a group (Top  Bottom) Increases Decreases
  15. 15. Atomic Radius   The trend: 1.  Atomic radius decreases across a period (LR) 2.  Atomic radius increases down a group (Top  Bottom) Decreases Increases
  16. 16. Exit Slip 1. Which of the following atoms has the largest atomic radius? a. oxygen (O) b. phosphorus (P) c. sulfur (S) d. chlorine (Cl)
  17. 17. Exit Slip 2. In general, how does ionization energy vary throughout the periodic table? a. it decreases across a period from left to right, and decreases down a group from top to bottom b. it increases across a period from left to right, and increases down a group from top to bottom c. it increases across a period from left to right, and decreases down a group from top to bottom d. It decreases across a period from left to right, and increases down a group from top to bottom
  18. 18. Exit Slip 3. Which of the following atoms has the smallest first ionization energy? a. lithium (Li) b. beryllium (Be) c. sodium (Na) d. potassium (K)
  19. 19. Exit Slip 4. Electronegativity is the a. energy it takes to remove an electron from an atom. b. number of protons and neutrons in an atom. c. measure of how good an atom is at stealing electrons. d. distance from the nucleus to the valence ring.
  20. 20. Exit Slip 5.  Which of the following correctly lists the elements in order of increasing electronegativity (least to most)? a.  O < P < Al < Na b.  Na < Al < P < O c.  P < O < Na < Al d.  Al < P < O < Na
  21. 21. Homework   Finish Review Worksheet #2   Make a mind map – double points!   In center oval: “periodic trends”   In 3 ovals around:   “atomic radius”   “electronegativity”   “ionization energy”   In 3 boxes for each:   definition of term   trend   picture

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