1. Chemical Reactions

2. Quick Review mass volume
Matter is the “stuff” that makes up the universe.
mass
volume
All matter has ______ and ________.
All matter is composed of basic building
blocks known as _______.
atoms

3. Quick Review
We know that matter can undergo changes both _________ and __________.
physical
chemical

4. Quick Review
When matter undergoes a physical change the composition of the substance is unchanged.
When matter undergoes a chemical change or reaction the composition of the substance is changed and chemical bonds are formed.

5. What happens during a chemical reaction?
Atoms in the reactants are rearranged to form one or more different substances (products).
Old bonds are broken; new bonds form.
Reactants Products
MgO C CO Mg

6. How do you know a chemical reaction has occurred?
Evolution of heat and light
Formation of a gas
Formation of a precipitate (formation of a solid in a solution)
Color change
Temperature changes (endothermic/exothermic)
A new odor is produced

7. Learning Check 1 Classify each of the following as a
1) physical change or 2) chemical change
A. ____ a burning candle
B. ____ melting ice
C. ____ toasting a marshmallow
D. ____ cutting a pizza
E. ____ polishing silver

8. Solution 1 Classify each of the following as a
1) physical change or 2) chemical change
A. __2__ a burning candle
B. __1_ melting ice
C. __2__ toasting a marshmallow
D. __1__ cutting a pizza
E. __2__ polishing silver

9. A Chemical Reaction
Reactants Products

10. Learning Check 2 A. How does an equation indicate a change in
the identity of the reacting substances?
B. How did the black and white reactants
combine?
C. Did all the reactants form product? Why or
why not?

11. Solution 2
A. How does an equation indicate a change in the identity of
the reacting substances?
The formulas of the reactants are different than the formulas of the products.
B. How did the black and white reactants combine?
1 black combined with 1 white.
C. Did all the reactants form product? Why or why not?
No. There were more black reactants than white.

12. Mind Jogger
When an object burns, the quantity of ashes that remain is smaller than the original object that was burned. How do you account for the change in mass? Where is the matter that appears to be lost?

13. Law of Conservation of Mass
mass is neither created nor destroyed in a chemical reaction
total mass stays the same (mass of reactants = mass of products)
atoms can only rearrange
4 H
2 O
4 H
2 O
36 g
4 g
32 g

14. Law of Conservation of Mass

15. Analyze the Problem
The law of conservation of mass will allow us to determine the amount of a
missing reactant or product that was involved in a chemical reaction.
For example, if you were told that 4 grams of hydrogen reacted with some
oxygen to make 36 grams of water then you could figure out how much
oxygen was used.
Write a word equation
Hydrogen + Oxygen Water
Write the masses of each substance given in the question
4 g ?
36g
Use the law of conservation of mass (mass of reactants = mass of products)
4 + ? = 36
Solve to find the missing value
? = ? = 32 So 32 grams of oxygen were used

16. Learning Check 3
In the complete reaction of g of sodium with g of chlorine, what mass of sodium chloride is formed?
A 10.0 g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide. How many grams of oxygen reacted?

17. Solution 3
In the complete reaction of g of sodium with g of chlorine, what mass of sodium chloride is formed?
58.44 g of Sodium chloride
A 10.0 g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide. How many grams of oxygen reacted?
6.6 g of Oxygen

18. How do we represent these chemical reactions?
Chemists use statements called equations.
Chemical equations do not express numerical equalities as in math.
Chemical equations show the direction in which the reaction progresses. Instead of an equal sign (=), an arrow is used
(means yield)

19. Word Equations
A statement using words to describe a chemical reaction.
Sodium (s) + Chlorine (g) Sodium Chloride (s)
The statement reads sodium and chlorine react to produce or yield
sodium chloride.
Useful but lacks important information

20. Chemical Symbols

21. Skeletal Equation
Uses chemical formulas instead of words to identify reactants and products.
Important step in writing a complete equation
Na(s) + Cl(g) NaCl(s)
Na(s) + Cl2(g) NaCl(S)

22. Learning Check 4
Write skeleton equations for the following word equations.
hydrogen(g) + bromine(g) hydrogen bromide(g)
carbon(s) + sulfur(s) carbon disulfide(s)

23. Solution 4 Write skeleton equations for the following word equations.
hydrogen(g) + bromine(g) hydrogen bromide(g)
H2(g) + Br2(g) HBr(g)
carbon(s) + sulfur(s) carbon disulfide(s)
C(s) + S(s) CS2(s)

24. Writing a Chemical Equation
Chemical symbols give a “before-and-after” picture of a chemical reaction
Reactants Products
MgO C CO Mg
magnesium oxide to form carbon monoxide
reacts with carbon and magnesium

25. Balancing a Chemical Equation
Balanced means that “conservation of mass” is upheld. Same numbers of each type of atom on each side of the equation
Al S Al2S Not Balanced
2Al S Al2S Balanced

26. Matter Is Conserved H2 + Cl2 2 HCl + + Total atoms = Total atoms
Total atoms = Total atoms
2 H, 2 Cl 2H, 2 Cl
Total Mass = Total Mass
2(1.0) (35.5) 2(36.5)
73.0 g = g

27. Balance Equations with Coefficients
Use a number before the compound/element symbol
to indicate how many of them are needed called a
COEFFICIENT. Coefficients in front of formulas balance
each type of atom.
4NH O NO + 6H2O
4 N = 4 N
12 H = 12 H
10 O = 10 O

28. How to write and balance Chemical Equations
Write the skeleton equation: Al + O2 → Al2O3
2. Count Number of atoms for each element on both sides
This is not balanced because the numbers don’t match
3. Multiply coefficients until they match – multiply the entire units 2
Al + O2 → Al2O3
Go to 6 oxygens

29. Balancing Equations Balanced Al + O2 Al2O3 Al + Al2O3 O2 2
Multiply each atom by 2 4
Al + 2
Al2O3 O2 3
Balanced

30. Learning Check 5 Balance each equation. A. Mg + N2 Mg3N2
B. Al Cl AlCl3

31. Solution 5
A. 3 Mg N2 Mg3N2
B. 2 Al Cl AlCl3

32. What not to do when balancing Chemical Equations
Never change a subscript to balance an equation (You can only change coefficients)
If you change the subscript (formula) you are describing a different chemical.
H2O is a different compound than H2O2
Never put a coefficient in the middle of a formula; they must go only in the front.
2NaCl is okay, but Na2Cl is not.