1. Covalent bonding

2. Covalent bonds  Nonmetals hold onto their valence electrons.  They can’t give away electrons to bond.  Still want noble gas configuration (full outer energy level).  Get it by sharing valence electrons with each other.  By sharing, both atoms get to count the electrons toward noble gas configuration.

3. How does H 2 form? ++ The nuclei repel But they are attracted to electrons They share the electrons

4. Electron Dot diagrams  A way of keeping track of valence electrons.  How to write them 1)Write the symbol. 2)Put one dot for each valence electron 3)Don’t pair up until they have to X

5. The Electron Dot diagram for Nitrogen l Nitrogen has 5 valence electrons. l First we write the symbol. N l Then add 1 electron at a time to each side... l Until they are forced to pair up.

6. Your Turn to Try  Fill in the chart on the top of page 5 in your packet.

7. Electron Dot Notation Bonding Sites: H, 1* Be, 2* B, 3* C, 4 N, 3 O, 2 F, 1 Ne, 0 He, 0Electron Dot Notation Bonding Sites: H, 1* Be, 2* B, 3* C, 4 N, 3 O, 2 F, 1 Ne, 0 He, 0

8. Covalent bonding  Fluorine has seven valence electrons F A second atom also has seven F By sharing electrons …both end with full orbitals 8 Valence electrons 8 Valence electrons

9. Single Covalent Bond  A sharing of two valence electrons.  Only nonmetals and Hydrogen.  Different from an ionic bond because they actually form molecules.  Two specific atoms are joined.

10. How to show how they formed  It’s like a jigsaw puzzle.  I have to tell you what the final formula is.  You put the pieces together to end up with the right formula.  For example- show how water is formed with covalent bonds.

11. Water H O Each hydrogen has 1 valence electron Each hydrogen wants 1 more The oxygen has 6 valence electrons The oxygen wants 2 more They share to make each other happy

12. Water  Put the pieces together  The first hydrogen is happy  The oxygen still wants one more H O

13. Water  The second hydrogen attaches  Every atom has full energy levels H O H

14. Multiple Bonds  Sometimes atoms share more than one pair of valence electrons.  A double bond is when atoms share two pair (4) of electrons.  A triple bond is when atoms share three pair (6) of electrons.

15. Carbon dioxide  CO 2 - Carbon is central atom  Carbon has 4 valence electrons  Wants 4 more  Oxygen has 6 valence electrons  Wants 2 more O C

16. Carbon dioxide  Attaching 1 oxygen leaves the oxygen 1 short and the carbon 3 short O C

17. Carbon dioxide l Attaching the second oxygen leaves both oxygen 1 short and the carbon 2 short O C O

18. Carbon dioxide l The only solution is to share more O C O

19. Carbon dioxide l The only solution is to share more O C O

20. Carbon dioxide l The only solution is to share more O CO

21. Carbon dioxide l The only solution is to share more O CO

22. Carbon dioxide l The only solution is to share more O CO

23. Carbon dioxide l The only solution is to share more O CO

24. Carbon dioxide l The only solution is to share more l Requires two double bonds l Each atom gets to count all the atoms in the bond O CO

25. Carbon dioxide l The only solution is to share more l Requires two double bonds l Each atom gets to count all the atoms in the bond O CO 8 valence electrons

26. Carbon dioxide l The only solution is to share more l Requires two double bonds l Each atom gets to count all the atoms in the bond O CO 8 valence electrons

27. Carbon dioxide l The only solution is to share more l Requires two double bonds l Each atom gets to count all the atoms in the bond O CO 8 valence electrons

28. How to draw them  Add up all the valence electrons.  Count up the total number of electrons to make all atoms happy (i.e. # of bonding sites)  Subtract.  Divide by 2  Tells you how many bonds - draw them.  Fill in the rest of the valence electrons to fill atoms up.

29. Examples  NH 3  N - has 5 valence e -, wants 8  H - has 1 valence e -, wants 2  NH 3 has 5+1(x 3) = 8 e -  NH 3 wants 8+2(x3) = 14 e -  (14-8)/2= 3 bonds  4 atoms with 3 bonds N H

30. NHH H Examples  Draw in the bonds  All 8 electrons are accounted for  Everything is full, Nitrogen has a lone pair of electrons

31. Examples  HCN C is central atom  N - has 5 valence electrons wants 8  C - has 4 valence electrons wants 8  H - has 1 valence electrons wants 2  HCN has 5+4+1 = 10  HCN wants 8+8+2 = 18  (18-10)/2= 4 bonds  3 atoms with 4 bonds -will require multiple bonds - not to H

32. HCN  Put in single bonds  Need 2 more bonds  Must go between C and N NHC

33. HCN l Put in single bonds l Need 2 more bonds l Must go between C and N l Uses 8 electrons - 2 more to add NHC

34. HCN l Put in single bonds l Need 2 more bonds l Must go between C and N l Uses 8 electrons - 2 more to add l Must go on N to fill octet NHC

35. Another way of indicating bonds  Often use a line to indicate a bond  Called a structural formula  Each line is 2 valence electrons HHO = HHO

36. Structural Examples H CN C O H H  C has 8 electrons because each line is 2 electrons  Ditto for N  Ditto for C here  Ditto for O

37. Ionic Compounds electron dot structures  Write as an equation.  Reactants-EACH atom with dots Products-EACH ion with its charge and dots  Example:

38. Lewis Dots Ionic Compounds  For homework tonight, use the “equation” method for question 38, p 176 if it helps you determine the products.  The ONLY thing required for an answer would be the products….