1. Covalent Bonding Diagrams
Chapter 16 Notes, Part I
Covalent Bonding Diagrams

2. An Addendum to Lewis Structures
Carbon and silicon are exceptions to the pattern of how to place electrons in a Lewis Dot Structure.
This is because they have hybrid orbitals (where the s and p sublevels blend together and have four equal energy orbitals.)

3. Covalent Bonding A covalent bond occurs between two non-metals
Electrostatic bonding does not occur—in other words, there is no “give and take” of electrons

4. It ends up being a “tug of war” of electrons
Where the electrons end up somewhere in the middle.

5. Single Bonds
A single bond occurs when one pair of electrons is shared by two atoms.
This pair of bonded electrons is called a shared pair.

6. Double and Triple Bonds
Double bonds occur when two atoms have two shared pair of electrons
Triple bonds occur when two atoms share three pair of electrons

7. Ionic compounds bonded together don’t really exist, but molecular compounds do!

8. Covalent Bonding Diagrams
Like the ionic bonding diagrams, first draw the dot diagram for each element
Now, however, the electrons are not being given away or taken, but shared; so signify a pair being shared by circling both electrons.
Every element should have eight electrons (count each shared pair as two).

9. Covalent Bonding Diagrams
If there is more than one of each element in the compound, you have to have a central atom.
It will be the one with the most spots to bond to.

10. Hydrogen
Since hydrogen is in the first energy level, it will not need 8 valence electrons to be stable—it will only need 2.

12. H2

13. H2O

14. Cl2

15. O2

16. N2

17. CCl4

18. CO2

19. HCN

20. PCl3

21. H2O2

22. C2H4

23. CSF2

24. SiS2

25. Covalent Bonding and Polyatomic ions
A polyatomic ion is just a charged molecule that bonds covalently.
The charge signifies how many electrons are given/taken away.

26. OH1-

27. NO21-

28. CO32-

29. PO33-