1. Covalent Bonding
Molecular Bonds

2. Chemistry Joke
Q: What happened to the man who was stopped for having sodium chloride and a nine-volt in his car?
A: He was arrested for a salt and battery!

3. A little review… Ionic Bonds Between a metal and a nonmetal
The metal completely loses electrons that the nonmetal gains.
The elements are held together (bonded) by an electrostatic charge, positive attracted to negative.
Lewis Dot Diagrams
We use dots to represent the number of valence electrons an atom has.
Can have up to 8 electrons (dots).

4. A new kind of bond…
Fluorine has seven valence electrons. F

5. A new kind of bond…
A second F atom also has seven. F F

6. Covalent bonding F F

7. Covalent bonding F F

8. Covalent bonding F F

9. Covalent bonding F F

10. Covalent bonding
Covalent Bond F F

11. Covalent Bonding
By sharing electrons, both fluorine atoms end up with a full octet of electrons and stable orbitals. F F

12. Covalent bonding
By sharing electrons, both fluorine atoms end up with a full octet of electrons and stable orbitals. F F
8 Valence electrons

13. Covalent bonding
By sharing electrons, both fluorine atoms end up with a full octet of electrons and stable orbitals. F F
8 Valence electrons

14. Covalent Bond
A bond in which two atoms share pairs of electrons so that each can achieve stability.

15. Covalent Compounds Made from 2 or more non-metals
Are usually liquids and gases (or solids with low melting points)
Propane - C3H8

16. Covalent vs Ionic Compounds
Chemical formulas called molecules.
Nonmetal bonds with nonmetal.
Chemical formula begins with a nonmetal.
Bonds formed by sharing electron pairs.
Chemical formula represents actual number of atoms in the compound.
Chemical formulas called formula units.
Metal bonds with nonmetal.
Chemical formula begins with a metal.
Bonds formed by attraction of positive cation to negative anion.
Chemical formula represents the lowest whole # ratio of elements in the compound.

17. Lewis Dot Diagrams
Remember: Atoms form compounds to create a full shell of valence electrons.
So, think Lewis Dot…
Hydrogen needs how many more electrons to have a filled energy level? H H 1 O O
How many more electrons does oxygen need? 2

18. H O Water Each H atom has 1 valence electron.
The O atom has 6 valence electrons. H O

19. H O Water The first hydrogen wants one more electron.
The oxygen wants two more electrons. H O

20. Water H O

21. Water H O
Covalent bond

22. H O H Water The first hydrogen is happy. A second hydrogen enters…
Covalent bond H

23. Water H O H
Covalent bond

24. H O H Water The second hydrogen attaches
Every atom has stable energy levels H O H

25. We can use Lewis Dot Structures to represent covalent compounds!
Add up the valence electrons of all the atoms in the compound.
Write the symbols for the elements and connect them with a line(s).
Least electronegative element goes in the center (for example: carbon). H is always on the outside.
The other elements usually surround the center one.
Subtract 2 from the total for each line drawn and arrange the remaining electrons (dots) in pairs around the outer elements first so that each atom has an octet. (H likes 2. Boron is happy with 6.)
Check for happiness (stability)!

26. Example…NH3 Ammonia N is in group 5A, so it has 5 valence electrons.
H is in group 1A so it has 1 valence electron
The compound NH3 has1 N and 3 Hs, so 5 + (3 x 1) gives a total of 8 valence electrons for the whole compound.
Subtracting 2 from the total for each line drawn: 8 – 6 = 2 remaining. H N H N
Check for happiness!
N is surrounded by 8 electrons, and each H has 2 electrons.
Each “line” in the dot structure represents 2 electrons.

27. You try… HF
H2O F2

28. Double and Triple Bonds
DOUBLE and TRIPLE bonds are formed when atoms share 2 or 3 pairs of electrons to attain a stable, noble gas configuration.
These bonds are represented with multiple lines in a dot diagram.

29. EXAMPLE: Nitrogen molecule, N2
Count the total number of valence electrons, 5 for each nitrogen atom giving a total of 10.
Draw the atoms connected with a line. N N
Then, subtract 2 for each bond (line). 10 – 2 = 8 remaining. Place the 8 remaining electrons in pairs around the 2 nitrogens.
But, the Ns aren’t happy. They only have 6 electrons each. What can we do?? N

30. N N N Multiple Bonds Needed! We can share more than one pair.
Now each N has 8 electrons and is happy.

31. Let’s try a couple together…
C2H2

32. Coordinate Covalent Bonds
Formed when one atom contributes both bonding electrons so that each atom can achieve a noble gas configuration.
To represent this type of bond, we use an arrow going FROM the donor TO the atom who is receiving the electrons.

33. Coordinate Covalent Bonds
Let’s look at the compound carbon monoxide. C O
O donates a full pair of electrons for sharing, forming a COORDINATE COVALENT BOND and allowing each atom to achieve noble gas configuration.
Notice the arrow going from the O to the C.

34. Resonance Structures
Structures that occur when it is possible to write 2 or more valid electron dot structures that have the same # of electron pairs for a molecule or an ion.

35. Example: O3, Ozone O O

36. Let’s try one together…
NO2-
The structures of ions are enclosed in brackets with the charge written on the outside.
Negative ions add electrons to the total count; positive ions take away electrons.

37. Stop for today.

38. Chemistry Joke
Q: What happened to the chemist who was reading a book about helium?
A: He just couldn’t put it down!