1. Bonding - Atoms interact (with their electrons) to form compounds.
Bonding and Chemical Formulas
Bonding - Atoms interact (with their electrons) to form compounds.
Sodium
Chlorine

2. Three Kinds of Bonds: Metal (+) Nonmetal (-) Ionic Nonmetal Nonmetal
Metal transfers electrons to make opposites attract.
Nonmetal
Nonmetal
Covalent
The sharing of electrons creates a strong bond.
electrons
Metal
Metal
Metal
Metallic
All electrons are shared in a “sea of electrons.”

3. Independent Practice Fill in the the blanks C - Covalent M - Metallic
I - Ionic

4. Proton Neutron Electron + +
To understand how bonding works, we need to understand electrons.
Proton
Positive Charge +
Neutron +
No Charge
Electron
Negative Charge

5. Valence Electrons The electrons on the outer energy level of an atom
How many valence electrons do each of these have? 6 3 5 5 1 4 2 1

6. Do you remember what the atomic number represents? 21 H
1.0079
Do you remember what the atomic number represents? 2 He
4.003 2 3 Li
6.941 4 Be
9.012 5 B
10.811 6 C
12.011 7 N
14.007 8 O
15.999 9 F
18.998 10 Ne
1.0079 8
It is the number of protons & 11 Na
22.990 12 Mg
24.305
electrons. 13 Al
26.982 14 Si
28.086 15 P
30.974 16 S
32.066 17 Cl
35.453 18 Ar
39.948 8 19 K
39.098 20 Ca
40.08
Page down if necessary. Have them look at the top numbers (atomic numbers) as they go across. It is likely that they will not be able to see them very well so you might have to read them aloud. Page up to do it again if necessary.
Explain that the atomic number tells us how many protons an atoms has. You might ask the question (using the classroom periodic table) How many protons does carbon have. And them switch back and say, “If an atom has 5 protons, what is it it?” Continue questioning until you feel that they understand.
Explain the atom mass is the total weight (on average…). Ask them how much a proton weighs (1 amu), how much an electron weighs (too small to weigh) and neutron weighs (1 amu).
Page down to the next slide.

7. Energy Level 1 2 electrons fitH
1.0079 2 He
4.003
Energy Level 1
2 electrons fit
How many valence electrons does hydrogen have?
How many valence electrons does helium have?
Fill in the periodic table on your paper.

8. Fill in the periodic table on your paper.
Energy Level 2
8 electrons fit: 3 Li
6.941 4 Be
9.012 5 B
10.811 6 C
12.011 7 N
14.007 8 O
15.999 9 F
18.998 10 Ne
1.0079
How many valence electrons do each of the elements above have?
Fill in the periodic table on your paper.

9. Fill in the periodic table on your paper.
Energy Level 3
8 electrons fit 11 Na
22.990 12 Mg
24.305 13 Al
26.982 14 Si
28.086 15 P
30.974 16 S
32.066 17 Cl
35.453 18 Ar
39.948
How many valence electrons do each of the elements above have?
Fill in the periodic table on your paper.

10. Look at the periodic table. Do you notice a pattern?
What is it?

11. This is true all the way down the periodic table:
You should have noticed that each column has the same number of valence electrons.
This is true all the way down the periodic table: 1 8 2 3 4 5 6 7

12. Which other atoms are FULL?
But there is something you need to know about electrons and the energy levels where they live.
Some are happier, more stable than others.
You see, energy levels like to be FULL.
These are “HAPPY” or “Stable” atoms. 10 Ne
1.0079 18 Ar
39.948 2 He
4.003
Which other atoms are FULL?

13. Everyone wants to be happy--
so, all atoms try to get happy.
But alas, they cannot do it alone. They must find other atom friends to make them happy.
But the right kind of friend is hard to find -- if you know what I mean.
Someone that understands you.
One who is willing to give you what you need most -- a part of himself.

14. More on electrons:
Atoms get happy (stable) by filling up their outer shell of electrons.
Atoms with 4 or more valence electrons will not give them up!
friend in need 
No, and don’t ask again!
Which columns on the periodic table will NOT give away electrons?
Atoms with less than 4 valence electrons are very generous.
Generous Friend 
Which columns on the periodic table will give away electrons?
Yes, is there anything else?

15. Even MORE about electrons:
However this affects their charge…Remember normally:
ATOMS
Have the same
# of Protons (+) = Electrons (-)
If the the blue atom gives up an electron, it becomes (+).
If the yellow atom gives up an electron, it becomes (-).
Generous friend helps a friend in need.
Lose -e makes +
Gain -e makes -

16. Write the oxidation numbers
Because of this, we assign a group of elements an oxidation number. Compare this number to the valence electrons. 1 8 1+ 2 3 4 5 6 7 H 2+ 3+ 4 3- 2- 1- He
Write the oxidation numbers
on your periodic table. Be B C N O F

17. Fill in the the chart on your paper.
Independent Practice
Fill in the the chart on your paper.

18. Na Cl
N H H H
Bonding An atom’s outer electron energy level is filled by either exchanging or sharing electrons.
NH3
NaCl H N H Na Cl H

19. Ionic Bonds Metal to Nonmetal19
Ionic Bonds Metal to Nonmetal
Electrons either taken or given away
Sodium
Chlorine +
Opposites attract

20. Ionic Bonds Metal to Nonmetal
Sodium gives Chlorine 1 electron. Na Cl
Sodium is happy at energy level 2.
Chlorine is happy at energy level 3.
NaCl
Sodium
Chlorine
Sodium Chloride

21. Covalent NH3 Ammonia Nitrogen Hydrogen Hydrogen Hydrogen
non-metal + nonmetal
Nitrogen
Electrons are shared.
Hydrogen
Hydrogen
Hydrogen H N H
Energy level HAPPY or stable... H
NH3 Ammonia

22. Metallic Ag+ Ag+ Ag+ Ag+ Ag+ Ag+ Ag+ Ag+ Ag+
electrons
metal
Metallic
Share in a sea of electrons
Ag+
Ag+
Ag+ -e -e -e -e -e
Ag+
Ag+
Ag+ -e -e -e
Ag+
Ag+
Ag+ -e -e -e -e -e

23. Fill in the the chart on your paper.
Independent Practice
Fill in the the chart on your paper.

24. Oxidation Number Varies1+ 2+ 3+ 4 3- 2- 1-
When you combine atoms, you use the oxidation numbers to help you figure out the ratio.
Oxidation Number Varies
Simply switch the oxidation number to get the correct subscript. Put the #s in lowest terms if necessary.
Mg+2
Cl-1
Mg+2
O-2
Fe+3
O-2 1 2 2 = 2 2 3
MgCl2
MgO
Fe2O3

25. Fill in the the chart on your paper.
Independent Practice
Fill in the the chart on your paper.

26. Polyatomic Compounds: Compounds that Act as a Unit
Mg+2
PO4-3
Li+2
SO4-2
Fe+3
NO4-2 3 2 2 2 2 3
Fe2 (NO4)3
Mg3(PO4)2
LiSO4
Note the ( ) on multiple polyatomic ions.

27. Fill in the the chart on your paper.
Independent Practice
Fill in the the chart on your paper.

28. Naming Compounds Potassium Bromide Bromine Example: KBr
Rules for naming binary (meaning 2 types of atoms) ionic compounds:
Example: KBr
1. Write the name of the metal first.
2. Write the name of the nonmetal changing the ending to “ide.”
Potassium
Bromide
Bromine

29. Independent Practice
Fill in the blanks.

30. Naming Compounds Copper (I) Chloride Chlorine Example: CuCl
Rules for naming binary ionic compounds:
(Binary means 2 types of atoms.)
Example: CuCl
1. Write the name of the metal first.
2. Write the name of the nonmetal changing the ending to “ide.”
3. If the metal is a “transition metal,” the oxidation number varies. Therefore, to name the compound we must put the ionic charge in parentheses. For example:
Copper
(I)
Chloride
Chlorine
because the oxidation of chlorine is 1.

31. Independent Practice
Fill in the blanks.

32. Naming Compounds Potassium Sulfate Polyatomic Example: K2 SO4
Rules for naming polyatomic ionic compounds:
1. Write the name of the metal first.
2. Write the name of the polyatomic nonmetal from the chart.
Example: K2 SO4
Potassium
Sulfate

33. Rules for naming polyatomic ionic compounds:
Naming Compounds
Ionic
Rules for naming polyatomic ionic compounds:
If the polyatomic ion is first, then:
1. Use the chart above to name the metal.
2. Write the name of the nonmetal changing the ending to “ide.”
Example: NH4Cl
Ammonium
Chloride