4.  The bond that forms from the sharing of valence electrons

5. AtomsPrefix 1mono- 2di- 3tri- 4tetra- 5penta- 6hexa- 7hepta- 8octa- 9nona- 10deca-

6.  Name first element  Name the second element and add –ide  Use prefixes to indicate the number of atoms in the molecule  Exception…if there is only one of the first atom, mono is left out!

8. N2F6N2F6 CO 2 SiF 4 CBr 4 NCl 3 P2S3P2S3 CO NO 2 SF 2 PF 5 SO 2 NO CCl 4 P2O5P2O5 Dinitrogen Hexafluoride Carbon Dioxide Silicon Tetrafluoride Carbon Tetrabromide Nitrogen Trichloride Diphosphorous Trisulfide Carbon Monoxide Nitrogen Dioxide Sulfur Difluoride Phosphorous Pentafluoride Sulfur Dioxide Nitrogen Monoxide carbon tetrachloride diphosphorus pentoxide

9.  Antimony tribromide  Hexaboron monosilicide  Chlorine dioxide  Hydrogen monoiodide  Iodine pentafluoride  Dinitrogen trioxide  Phosphorus triiodide SbBr 3 B 6 Si ClO 2 HI IF 5 N 2 O 3 PI 3

10.  Ammonia – NH 3  Water - H 2 O  Methane - CH 4

12.  Electron dot notation is used to shown how electrons are shared  Molecules are formed  Each molecule has 8 valence electrons  Except Hydrogen!

13. Each line represents the sharing of 2 electrons

14. Lone Pair

15.  PH 3  H 2 S  HCl  CCl 4  SiH 4

16.  H 2  HF  F 2

17.  Single Bonds  Symbol : σ

19.  Draw O 3

20.  Draw O 2

21.  N 2  C 2 H 2  CO 2

22.  Xe,Si, P, S, Cl, Br, and I  Sometimes have more than 8 electrons  PF 5  Be and B often only have 6 electrons  BeCl 3

23.  Draw C 2 H 4  Label all bonds as sigma or pi

24.  A single electron, not paired

25.  As the number of shared electrons increases, bond length decreases  Breaking the bond of a short bond is larger than a long bond

26.  What is an ionic bond and how does it differ from a covalent bond?  What is the difference between a sigma bond and a pi bond?  Predict the bond energy of each of the bonds in CH 2.

27. nitrate ion CHO 2 -1 O 3