2. Have you ever heard the word bonding before?
If so, where did you hear it and what does it mean?
If you have never heard it before write down what you think it means?

3. Bonding is what keeps elements and ions of compounds together!!!
Do the salty 8’s game here if you have time!

4. What’s the difference between an Element and a Compound
What’s the difference between an Element and a Compound? Give an example of each and explain why.

5. Elements
An element is a substance that cannot be broken down into different substances.
It is the smallest form of matter that has the same characteristics of that substance.
Examples: Au (gold), Na (sodium) etc.

6. COMPOUNDS
Define what a compound is?
Two or more DIFFERENT atoms (elements) that are chemically bonded together because of a chemical reaction.
We use chemical formulas to represent compounds. Can you think of any…?
H2O (Wudder) CO2 (Carbon Dioxide)
CH3COOH + NaHCO3 ===> CH3COONa + H2O + CO2

7. D Mixture of Compounds C Mix of Elements1 2 3
D Mixture of Compounds
A Element
B Compounds 4 5 6
E Mix of Elements/ Compounds
C Mix of Elements
A Elements

8. A New Language
Let’s do the Vial Lab!

9. We will talk about 4 TYPES OF BONDS
IONIC
COVALENT
METALLIC
HYDROGEN
(Ions)
(Sharing
valence electrons)
(Metals)
(Ions)

10. IONIC BONDS
Form between ions with opposite charges: + and -. (a metal and a non-metal)
They bond because the opposite charges are attracted to each other. (Think magnets!!!)

11. IONIC BONDS
Like charges repel each other! Ions and ionic bonds form because electrons are transferred from one atom to the other

12. Properties of IONIC BONDS
Ionic compounds have high melting and boiling points.
These are very strong bonds.
An example is Na+1 + Cl-1
= NaCl (salt)
NaCl Melting point 801 °C NaCl Boiling point1465 °C

13. IONIC BONDS
Only certain ratios (combinations) of elements result in the formation of Ionic compounds.
For ex: Lithium (Li) will react with Fluorine (F) to form LiF.
BUT, it will NOT form LiF2, LiF3, etc.
Magnesium (Mg) will react with Fluorine to form MgF2.
BUT, it will NOT form MgF, MgF3, etc.

14. IONIC BONDS When writing a chemical formula for an ionic compound:
*The charges have to balance
to create a neutral compound.*

15. IONIC BONDS For example: - With salt the charges are
both 1: Na+1 and Cl-1
So we just need one of each ion to make the compound neutral
= the ratio is 1:1
= NaCl

16. IONIC BONDS What if the charges are not the same number???
- Like Li+1 + O-2
Here you will not have a 1:1 ratio. You need to balance the chemical formula…

17. IONIC BONDS
What could you do to get the charges to cancel out if you wanted to form this ionic compound???
Li+1 + O-2
ANSWER: You would need to use
2 Li+1 for every O-2!!!
= Li2O

18. IONIC BONDS Let’s Practice!!! Write chemical formulas for:
1.) K and N
2.) Ca and F
3.) Li and Cl
4.) Mg and Si
5.) Al and O
1.) K3N
2.) CaF2
3.) LiCl
4.) Mg2Si
5.) Al2O3

19. IONIC BONDS 6.) CaCl2 6.) Ca and Cl 7.) K3P 7.) K and P 8.) MgCl2
8.) Mg and Cl
9.) Li and P
10.) K and O
6.) CaCl2
7.) K3P
8.) MgCl2
9.) Li3P
10.) K2O

20. Copy down this table for your answers.
Chemical Formulas
Rb and Cl Na and S Li and P
1. Hints: The metal comes first, the non-metal comes second
Change the end of the name of the second element to “ide”
Copy down this table for your answers.
Metal
Nonmetal
Chemical Formula
Compound Name
2. If you mix Calcium Chloride (CaCl2) into a glass of water until it dissolves, what is the chemical formula?

21. Chemical Formulas
Rb and Cl Na and S Li and P
1. Hints: The metal comes first, the non-metal comes second
Change the end of the name of the second element to “ide”
Metal
Nonmetal
Chemical Formula
Compound Name Rb +1 Cl -1
RbCl
Rubidium Chloride Na +1 S -2
Na2S
Sodium Sulfide Li +1 P -3
Li3P
Lithium Phosphide
2. If you mix Calcium Chloride (CaCl2) into a glass of water until it dissolves, what is the chemical formula?
CaCl2 (aq)

22. Ionic Bonds Practice Write the chemical formulas for the compounds formed when these ions bond:
11.) Al & S
12.) Rb & O
13.) Be & F
14.) Al & Cl
15.) Ca & N
16.) Ga & Se
11.) Al2S3
12.) Rb2O
13.) BeF2
14.) AlCl3
15.) Ca3N2
16.) Ga2Se3

23. COVALENT BONDS Form between two non-metals
They bond because the outer electron rings are not full so they share valence electrons!
(The atoms are NOT stable.)

24. Properties of COVALENT BONDS
Covalent compounds will have low melting and boiling points.
These are usually weak bonds.
Some examples are H2O (water/ wudder), and CO2 (Carbon Dioxide)

25. COVALENT BONDS The reason H2O is covalent:
Remember H can be a metal or a non-metal!!!
Here H is behaving like a non-metal.
Hydrogen is usually a non-metal!

26. Let’s Practice! Write the following compounds and determine if they are Ionic or Covalent?
1.) NH ) AlCl3
2.) NaCl ) P2O5
3.) CH ) Li3P
4.) CO ) BN
5.) CaCl ) N2O
6.) KBr ) MgS

27. ANSWERS… 1.) NH3 Covalent 2.) NaCl Ionic 3.) CH4 Covalent
4.) CO2 Covalent
5.) CaCl2 Ionic
6.) KBr Ionic
7.) AlCl3 Ionic
8.) P2O5 Covalent
9.) Li3P Ionic
10.) BN Covalent
11.) N2O Covalent
12.) MgS Ionic

28. Lewis Structures Electron Dot Diagrams
We can show how the atoms share or transfer electrons by drawing electron dot diagrams.
You will only use the valence e- for dot diagrams.

29. Dot Diagrams
Start the dot diagram by writing the atomic symbol for the atom.
Ex: Mg
The symbol has 4 sides…

30. Dot Diagrams Each side can hold up to 2e-
You cannot pair the electrons until there is one on each side. 1 3 4

31. Dot Diagrams Mg Mg only has 2 valence e-.
So it’s dot diagram looks like this:
Let’s try… Si
how about… S 1 3 4

32. Dot Diagrams Practice!!! Draw the Dot Diagrams for:
1.) Cl
2.) Al
3.) Na
4.) Sn
5.) Ar

33. Metals always donate their electrons!
Dot Diagrams
Now we can put individual diagrams together to show whether atoms transfer or share their valence e-!!!
Who donates their electrons,
metals or non-metals?
Metals always donate their electrons!

34. Dot Diagrams for Ionic Bonds
In an Ionic Bond, atoms are transferring their valence e- …
To show this “transferring” , we draw arrows between the Atomic Symbols to represent the transferring of e-.
We can show this w/ dot diagrams.
For Ex: (Li + Cl = LiCl) Cl Li

35. Dot Diagram Practice for Ionic Bonds
BeO
NaCl
MgS
CaCl2
LiP
AlCl

36. Dot Diagrams for Covalent Bonds
In a Covalent Bond, atoms are sharing their valence e- …
To show this “sharing”, we draw a BAR between the Atomic Symbols to represent the sharing of e-.
One bar = 2 e-.
For Ex: H2O

37. Dot Diagrams for Covalent Bonds
One bar = 2 e-.
For Ex: H2O (draw out the individual dot
diagrams first.)
H O H
***H’s ALWAYS have to go on the ENDS.

38. Dot Diagram Practice for Covalent BondsCH SO NH
SiO CF

39. Bonding Dot Diagram Steps
1.) Identify the type of bond you have. (Covalent or Ionic)
2.) Separate the individual elements and put them in a line. Put the atomic symbol w/ least amount of valance electrons in CENTER!!!
3.) Except the Hydrogen’s!!!! Remember H’s have to be on ENDS!!!
4.) Draw the “dots” for each atomic symbol.

40. Bonding Dot Diagram Steps
5.) Show either the transferring or sharing of e- with arrows or bars.
6.) If sharing (covalent bonds)…connect the “lonely” dots between DIFFERENT symbols!!!
7.) Count the e- around each atomic symbol to make sure there are 8!!! (ONLY 2 for H!)

41. **This works for COVALENT bonds only**
1234 HONC
Based on your prior knowledge of atoms and their valance electrons, what in the world does
1234 HONC mean?
Hydrogen, Oxygen, Nitrogen, Carbon
Based on their valance electrons, how many atoms can bond to each of them?
H O N C
H= can form one bond.
O= can form two bonds.
N= can form three bonds.
C= can form four bonds.
**This works for COVALENT bonds only**

42. Dot Diagram Practice 1.) NF3 2.) Sr3N2 3.) Rb2O 4.) CH3Cl 5.) Al2S3
6.) Na3N

43. Dot Diagram Practice
3.) Rb2O
4.) CH3Cl

44. Dot Diagram Practice
5.) Al2S3
6.) Na3N

45. Dot Diagram Practice 7.) CH3Br 8.) NH2Cl 9.) PCl3 10.) CH4 11.) Br2O
12. IBr

46. Dot Diagram Practice
7.) CH3Br
8.) NH2Cl

47. Dot Diagram Practice
9.) PCl3
10.) CH4

48. Dot Diagram Practice
11.) Br2O
12. IBr

49. Quick Quiz Covalent bonds form because…
They share valence electrons
Like charges attract
They gain neutrons
Opposite charges attract
They share protons

50. The compound C6H12O6 has Ionic bonds Covalent bonds Nuclear bonds
Metallic bonds
Hydrogen bonds

51. Covalent bonds mostly occur with atoms on the right side of the periodic table.
True
False

52. Ionic bonds have… Strong bonds, low boiling and melting points
Weak bonds, low boiling and melting points
Strong bonds, high boiling and melting points
Weak bonds, low boiling points and high melting points

53. Ionic bonds are formed because
Opposite charges attract
Share valence electrons
Electrons are transferred
Protons are transferred
Both A & C
Both C & D

54. Which compound has ionic bonds? *
CuSO4 O2
CH4

55. The Law of Conservation of Mass
The Law of Conservation of Mass states that in a chemical reaction, mass cannot be created or destroyed, but it can change forms!
So this means that the mass before the reaction has to be the same as the mass after the reaction.

56. Does this equation go against the Law of Conservation of Mass
Does this equation go against the Law of Conservation of Mass? (count the atoms of each element)
Photosynthesis
6CO2 + 6H2O C6H12O6 + 6O2
Chemical Reaction
Reactants
Products
Give them Quiz #II

57. Now, Does this equation go against the Law of Conservation of Mass?
6CO2 + 6H2O C6H12O6 + 6O2 6C
12 O
12 H
6 O 6C
12 H
6 O
12 O
This does not violate the Law of Conservation of Mass

58. “reactant(s) = product(s)”
Balancing Equations
Due to the Law of Conservation of Mass each type of element needs the same amount before the reaction and after the reaction.
“reactant(s) = product(s)”
But, you can’t change the elements that participate in the reaction, so you must write a number in front of (to the left of) each material in the reaction to make sure every type of element has the same number on each side of the reaction.

59. How molecules are symbolized
Cl2
2Cl
2Cl2 Cl Cl Cl Cl Cl Cl Cl Cl
How is the middle picture different from the other two?

60. You will NEVER add a subscript
Balancing Equations
CaCl2  Subscript
The little two tells you that there are 2 Cl. It only applies to the Cl.
But… 2CaCl2
When you have a Coefficient 2CaCl2
CaCl2
+CaCl2
The 2 tells you that there are 2Ca and 4Cl
It applies to everything behind it in the compound.
You will NEVER add a subscript
only Coefficients!

61. Understanding Chemical Compounds
How many atoms are in each chemical compound?
C6H12O6
2H2O2
6CuNO3
6 C
12 H
6 O
4 H
4 O
6 Cu
6 N
18 O

62. Understanding Chemical Compounds
How many atoms are in each chemical compound?
C20H30O2
3C6H12S2
2K3PO4
2C3H7NO2
2Al2S3
4KClO3
20 C
30 H
2 O
18 C
36 H
6 S
6 K
2 P
8 O
6 C
14 H
2 N
4 O
4 Al
6 S
4 K
4 Cl
12 O

63. Bonding What is the chemical formula for each one and WHY? 1.) 2.) 3.)
1.) 3Na2 (3 pairs chemically bonded)
2.) Na2 (1 pair chemically bonded)
3.) 2Na (not chemically bonded) Na Na Na Na

64. Balancing Equations What’s the difference between… A2 + B2 and A2B2 ?
A2 + B2 = Not chemically bonded, so its not a compound! These are elements.
A2B2 = This is chemically bonded because it is a compound.

65. Balancing Equations  + Let’s look at an example:
Element Mg will bond with element O in the chemical reaction below:
Mg + O MgO
Are there the same amount of O’s on the left as there are on the right???
NO!!! We must balance this equation!!! O Mg +  Mg O

66. Balancing Equations  + O O
How can we make there be the same # of each element on both sides???
Mg + O2  MgO
“reactants = product”
By putting a coefficient in FRONT...
Mg + O2  2MgO
You multiply all of the elements in the compound by the coefficient in front.
Is it balanced yet???
NO! O Mg +  Mg O

67. Balancing Equations
Where else could we put a coefficient to balance it?
Mg + O2  2MgO
“reactants = product”
We need to add a coefficient in the front on the other side…
2Mg + O2  2MgO
There are 2Mg’s and 2 O’s on the left AND there are 2Mg’s and 2 O’s on the right…NOW it’s BALANCED!!! 

68. Balancing Equations I only added Coefficients!
2Mg + O2  2MgO
I only added Coefficients!
So let’s practice with some real problems to see how you do!
Reactants =
product

69. Balancing Equations Let’s practice…
1.) Al + Br AlBr3
2.) H2 + O H2O
3.) Na + Cl NaCl
3.) 2Na + Cl NaCl
4.) Fe + O Fe2O3
4.) 4Fe + 3O Fe2O3
5.) P4 + O P2O5
5.) P4 + 5O P2O5

70. Balancing Equations… 6.) N2 + H2 NH3 7.) Mg + O2 MgO 8.) H2 + Cl2 HCl
9.) Ag + S Ag2S
10.) S + O SO4

71. Balancing Equations… Lets see how you did! 6.) N2 + 3H2 2NH3
6a.) 2N2 + 6H NH3 Is this balanced?
7.) 2Mg + O MgO
8.) H2 + Cl HCl
9.) 2Ag + S Ag2S
10.) S + 2O SO4

72. Covalent Bonds Ionic Bonds
Try this without using your notes
Explain what are three differences between a Covalent bond and an Ionic Bond?
Covalent Bonds
Share valence electrons
Non-metal and Non-metal
Weak bonds
Low Boiling Pts. and Melting pts.
Ionic Bonds
1. Opposite charges attract
2. Metal and Non-metal
3. Strong bonds
4. High Boiling Pts. and Melting pts.

73. Metallic Bonds Form between 2 metal atoms. (metal and metal)
The atoms are unstable – they do not have full electron rings.
Bond by sharing very loosely held valence electrons with each other. (The electrons “flow” between the atoms.)
Metallic bonds are NOT the strongest bonds though…
Ionic Bonds are the strongest bonds!

74. Properties of Metallic Bonds
Metallic compounds are highly conductive. (They conduct heat & electricity very easily!!!)
They also have metallic luster (shine)
They are malleable (able to be hammered into thin sheets.)
They are ductile (can be rolled into wires.)
Examples: CuZn, AlSb, GaSb, LaMg

75. What makes it easier for some atoms to bond better than other atoms?
When you think about atoms bonding, what do atoms need to gain or lose?
VALENCE ELECTRONS!!!
N-3 Li+1
Which atom will bond the easiest?
Li+1 Why?
The LESS electrons an atom needs to gain or lose to have a full outer ring, the EASIER it is for that atom to bond!!!

76. Which groups (1-18) on the periodic table, will bond the easiest?

77. Which groups on the periodic table will share or transfer electrons the easiest? (i.e. be most likely to form bonds?)
ANSWER: Groups 1 and 17 b/c group 1 only needs to get rid of 1e- and group 17 only needs to gain 1e-.

78. Question…
Is an element in Group 13 more likely to bond than an element in Group 16? EXPLAIN…
ANSWER: No, b/c the element in Group 16 only needs to gain 2e-, but the element in Group 13 needs to lose 3e-.