1. Monday and Tuesday March 26 and 27

2. Lewis Dot Structures

3. Review? 1.What is a valence electron? 2.What is the lewis dot structure of: a)Lithium b)Bromine Do your best to answer on your own.

4. Valence Electrons The valence electrons are the electrons in the last shell or energy level of an atom. Why are they important? -BONDING!

5. Valence Electrons How many for each element? www.chemprofessor.com/ptable5.gif

6. Lewis Dot Structures What is the lewis dot structure of: a)Lithium b) Bromine

7. Lewis Dot Structures Draw the lewis dot structure for lithium bromide: Draw the lewis dot structure of calcium chloride: Draw the lewis dot structure of methane (CH 4 ): Identify the lone pairs and bonding pairs! **NO LONELY ELECTRONS!! Draw the lewis dot structure of oxygen gas:

8. Chemical Bonding Types of Bonds, Polarity, and Dipoles

9. What is electronegativity? The ability of an element to steal an electron from another element

10. What are BONDS? The attraction between atoms Causes shape and structure of chemicals

11. Types of Bonds Non-polar (Covalent) 0.0 Polar (Covalent) 0.1 to 1.9 Ionic 2.0 or higher

12. Nonpolar Covalent Bond Electronegativity Difference of 0.0 Electrons are shared equally

13. Polar Covalent Bond Electronegativity Difference of 0.1 – 1.6 Electrons are shared, however, they favor one side of the molecule.

14. Copyright © 2006 by the Regents of the University of California.

16. Two types of Covalent Bonds NONPOLAR POLAR

17. Ionic Bond Electronegativity Difference of 1.7 or higher Electrons are transferred to the other element.

18. Types of Bonds Non-polar (Covalent) 0.0 Polar (Covalent) 0.1 to 1.9 Ionic 2.0 or higher

19. Practice Draw the lewis dot structure for the formulas below and identify the bond type: Potassium Bromide Carbon Disulfide Nitrogen Trifluoride

20. Wednesday 3/28 and Thursday 3/29

21. Modeling Lab

22. Friday 3/30

23. How are molecular shapes determined? VSEPR

24. Lewis Structures & VSEPR Valence Shell Electron Pair Repulsion electron pairs spread apart as far as possible

25. Electron Pair Geometry: Linear Molecular Geometry: Linear Number of Lone Pairs: 0 Number of Bonds: 2 Angle: 180 ̊

26. Electron Pair Geometry: Trigonal Planar Molecular Geometry: Trigonal Planar Number of Lone Pairs: 0 Number of Bonds: 3 Angle: 120 ̊

27. Electron Pair Geometry: Trigonal Planar Molecular Geometry: Bent Number of Lone Pairs: 1 Number of Bonds: 2 Angle: 117 ̊

28. Electron Pair Geometry: Tetrahedral Molecular Geometry: Tetrahedral Number of Lone Pairs: 0 Number of Bonds: 4 Angle: 109.5 ̊

29. Number of Lone Pairs: 1 Number of Bonds: 3 Electron Pair Geometry: Tetrahedral Molecular Geometry: Trigonal Pyramidal Angle: ~107 ̊

30. Electron Pair Geometry: Tetrahedral Molecular Geometry: Bent Number of Lone Pairs: 2 Number of Bonds: 2 Angle: 104.5 ̊

31. Questions on shape?

32. Dipoles Contains a positive end and a negative end.

33. Copyright © 2006 by the Regents of the University of California.

38. Practice CO 2 NH 3 BF 3 Li 2 O