1. Chemical Bonding Molecular Polarity Vector Sum of Bond Polarities Why are some molecules polar but others are not?

2. Molecular Polarity HCl is POLAR (or dipolar). It has a DIPOLE MOMENT. The polar HCl molecule will turn to align with an electric field.

3. Molecular Polarity Molecules will be polar if a)bonds are polar AND b)the molecule is NOT “symmetric” All above are NOT polar

4. Chemical Bonding Carbon Dioxide CO 2 is NOT polar even though the CO bonds are polar. CO 2 is symmetrical. +1.5-0.75-0.75 Positive C atom is reason CO 2 + H 2 O gives H 2 CO 3

5. Chemical Bonding Molecular Polarity, BF 3 B atom is positive and F atoms are negative. B—F bonds in BF 3 are polar. But molecule is symmetrical and NOT polar

6. Chemical Bonding Molecular Polarity, HBF 2 B atom is positive but H & F atoms are negative. B-F and B-H bonds in HBF 2 are polar. But molecule is NOT symmetrical and is polar. -- ++

7. Chemical Bonding Is Methane, CH 4, Polar? Methane is symmetrical and is  NOT polar.

8. Chemical Bonding Is CH 3 F Polar? C—F bond is very polar. Molecule is not symmetrical and so is polar.

9. Chemical Bonding Drawing Lewis Structures The Octet Rule Concept of Formal Charge © 2009, Prentice-Hall, Inc.

10. Chemical Bonding © 2009, Prentice-Hall, Inc. Lewis Structures Lewis structures are representations of molecules showing all valence electrons, bonding and nonbonding.

11. Chemical Bonding The Octet Rule The most important requirement for the formation of a stable compound is that the atoms achieve a noble gas electron configuration. © 2009, Prentice-Hall, Inc.

12. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures 1.Find the sum of valence electrons of all atoms in the polyatomic ion or molecule.  If it is an anion, add one electron for each negative charge.  If it is a cation, subtract one electron for each positive charge. PCl 3 5 + 3(7) = 26

13. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures 2.The central atom is the least electronegative element that isn’t hydrogen. Connect the outer atoms to it by single bonds. Keep track of the electrons: 26 - 6 = 20

14. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures 3.Fill the octets of the outer atoms. Keep track of the electrons: 26 - 6 = 20; 20 - 18 = 2

15. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures 4.Fill the octet of the central atom. Keep track of the electrons: 26 - 6 = 20; 20 - 18 = 2; 2 - 2 = 0

16. Chemical Bonding Exercise 8.2 Draw the Lewis Structures for …  CsI  H 2 O  NH 3  CH 4 © 2009, Prentice-Hall, Inc.

17. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures 5.If you run out of electrons before the central atom has an octet… …form multiple bonds until it does. Usually occurs with carbon, nitrogen, oxygen

18. Chemical Bonding Exercise 8.3 Write Lewis Structures for…  Ethene, C 2 H 4  Acetic Acid, CH 3 COOH  Oxygen, O 2  Nitrogen, N 2

19. Chemical Bonding Resonance Structures More than One Lewis Structure © 2009, Prentice-Hall, Inc.

20. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance This is the Lewis structure we would draw for ozone, O 3. -

21. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance But this is at odds with the true, observed structure of ozone, in which…  …both O-O bonds are the same length.  …both outer oxygens have a charge of -1/2.

22. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance One Lewis structure cannot accurately depict a molecule like ozone. We use multiple structures, resonance structures, to describe the molecule.

23. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance Just as green is a synthesis of blue and yellow… …ozone is a synthesis of these two resonance structures.

24. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance In truth, the electrons that form the second C-O bond in the double bonds below do not always sit between that C and that O, but rather can move among the two oxygens and the carbon. They are not localized; they are delocalized.

25. Chemical Bonding © 2009, Prentice-Hall, Inc. Resonance The organic compound benzene, C 6 H 6, has two resonance structures. It is commonly depicted as a hexagon with a circle inside to signify the delocalized electrons in the ring.

26. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures (Formal Charge) Then assign formal charges.  For each atom, count the electrons in lone pairs and half the electrons it shares with other atoms.  Subtract that from the number of valence electrons for that atom: the difference is its formal charge.

27. Chemical Bonding © 2009, Prentice-Hall, Inc. Writing Lewis Structures The best Lewis structure…  …is the one with the fewest charges.  …puts a negative charge on the most electronegative atom.

28. Chemical Bonding Exercise 8.4 Considering formal charge write the correct Lewis Structures for…  Thiocyanate Ion, [SCN] -  Sulfate Ion, [SO 4 ] 2-

29. Chemical Bonding Exceptions to the Octet Rule © 2009, Prentice-Hall, Inc.

30. Chemical Bonding © 2009, Prentice-Hall, Inc. Exceptions to the Octet Rule There are three types of ions or molecules that do not follow the octet rule:  Ions or molecules with an odd number of electrons  Ions or molecules with less than an octet  Ions or molecules with more than eight valence electrons (an expanded octet)

31. Chemical Bonding © 2009, Prentice-Hall, Inc. Odd Number of Electrons Though relatively rare and usually quite unstable and reactive, there are ions and molecules with an odd number of electrons.

32. Chemical Bonding © 2009, Prentice-Hall, Inc. Fewer Than Eight Electrons Consider BF 3 :  Giving boron a filled octet places a negative charge on the boron and a positive charge on fluorine.  This would not be an accurate picture of the distribution of electrons in BF 3.

33. Chemical Bonding © 2009, Prentice-Hall, Inc. Fewer Than Eight Electrons Therefore, structures that put a double bond between boron and fluorine are much less important than the one that leaves boron with only 6 valence electrons.

34. Chemical Bonding © 2009, Prentice-Hall, Inc. Fewer Than Eight Electrons The lesson is: if filling the octet of the central atom results in a negative charge on the central atom and a positive charge on the more electronegative outer atom, don’t fill the octet of the central atom.

35. Chemical Bonding © 2009, Prentice-Hall, Inc. More Than Eight Electrons The only way PCl 5 can exist is if phosphorus has 10 electrons around it. It is allowed to expand the octet of atoms on the 3rd row or below.  Presumably d orbitals in these atoms participate in bonding.

36. Chemical Bonding © 2009, Prentice-Hall, Inc. More Than Eight Electrons Even though we can draw a Lewis structure for the phosphate ion that has only 8 electrons around the central phosphorus, the better structure puts a double bond between the phosphorus and one of the oxygens.

37. Chemical Bonding © 2009, Prentice-Hall, Inc. More Than Eight Electrons This eliminates the charge on the phosphorus and the charge on one of the oxygens. The lesson is: when the central atom in on the 3rd row or below and expanding its octet eliminates some formal charges, do so.