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2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
2 9 Chemical Bonding Benchmark Review   Part Ii
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2 9 Chemical Bonding Benchmark Review Part Ii

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  1. Launch: 2/8   Grab your binder and immediately take a seat!   Place launch paper and yesterday’s practice questions on your desk.   Friday’s Quiz Data: 90%!   Today’s Objectives: I can draw a Lewis structure.
  2. Launch 2/8 1.  Look around the classroom and make a list of all the new things you can see.
  3. Launch 2/8 2.  Which of the following is true about the Kinetic Molecular Theory? a) It can be used to measure the speed of molecules. b) It states that gas molecules more slower at high temperatures. c) It states that the motion of a gas particle is fast and random d) All of the above.
  4. Launch 2/8 3.  Pressure is created by a) the diffusion of two or more gases. b) the random motion of molecules and their collisions with a surface. c)  the phase change that occurs at 0°C. d) the force of a solid exerted on the interior of a gas.
  5. Announcements   Quiz scores handed out at the end of class   New items in the classroom   Positive consequences   Negative consequences   Word wall   Data wall   Shout Outs!   Change in schedule!   Surprise benchmark
  6. February Calendar Quiz! Today Benchmark Quiz! Exam!
  7. Opening   Today’s Objective: I can classify a chemical bond as either ionic, covalent, or metallic.
  8. Chemical Bonding Review: Part II Mr. Heffner 2//09
  9. What are Lewis structures?   Lewis structures are…   pictures of covalent molecules • •  • •  Covalent Bond F- F 2 electrons = dash • •  • •  Lewis Structure • •  • • 
  10. Example #1 Draw the Lewis symbol for carbon.   Step 1: Place element’s symbol in center C
  11. Example #1 Draw the Lewis symbol for carbon.   Step 2: # of valence electrons?
  12. Example #1 Draw the Lewis symbol for carbon.   Step 2: # of valence electrons? “The Trick”: Group # Drop the 1! group # = 14 # valence electrons = 4
  13. Example #1 Draw the Lewis symbol for carbon.   Step 3: Place electrons around symbol   One on each of the 4 sides   No doubling up! •  •  C •  • 
  14. What is a Lewis structure?   There is a 3-step process for creating Lewis structures: 1.  Draw Lewis symbol for each atom and count dots 2.  Arrange atoms so they all have a full octet   If more than 2 atoms, place first atom in center 3.  Count dots and convert shared pairs to bonds
  15. Example Draw the Lewis structure for Cl2   Step 1: Draw Lewis symbol for each atom and count • •  • •  dots Cl Cl •  • •  • •  •  • •  14 dots • • 
  16. Example Draw the Lewis structure for Cl2   Step 2: Arrange atoms so they have a full octet • •  • •  Cl Cl • •  • •  • •  • =•  8• •  8 =
  17. Example Draw the Lewis symbol for Cl2   Step 3: Count dots and convert shared pairs to dashes • •  • •  Covalent Bond Cl-Cl 2 electrons = dash • •  • •  • •  • •  • •  dots 14
  18. Example Draw the Lewis structure for NH3   Step 1: Draw Lewis symbol for each atom and count • •  dots •  •  •  N HHH •  •  •  8 dots
  19. Example Draw the Lewis structure for NH3   Step 2: Arrange atoms so they have a full octet   If more than two atoms, place first atom in center • •  HN H • •  H is an exception to •  • •  •  H the octet rule 2= 8=
  20. Example Draw the Lewis symbol for Cl2   Step 3: Count dots and convert shared pairs to dashes • •  H-N-H • •  • •  •  - •  H 8 dots
  21. Example Draw the Lewis structure for CH4
  22. Practice Questions   Review worksheet
  23. Exit Slip 1.  In covalent bonding, a.  valence electrons are exchanged. b.  only metals interact with other metals. c.  valence electrons are shared d.  atoms become less stable due to the octet rule.
  24. Exit Slip 2.  Covalent bonds form between which two types of elements? a.  metals and metals b.  metals and nonmetals c.  nonmetals and nonmetals d.  none of the above
  25. Exit Slip 3.  Ionic bonds form between which two types of elements? a.  alkali and alkaline earth metals b.  halogens and other halogens c.  metals and nonmetals d.  nonmetals and other nonmetals
  26. Exit Slip 4.  What type of compound is H2SO4? a.  metallic b.  covalent c.  ionic d.  none of the above
  27. Exit Slip 5.  Which of the following is an example of an ionic compound? a.  AlCl3 b.  CCl4 c.  O2 d.  Zn2+
  28. Homework   Finish the review worksheet   Study hard for Tuesday’s exam!

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