1. S-133 Write the formula for Palladium (IV) Oxide Calcium Fluoride
Cadmium (II) Nitride
Write the name for
Al2S3
Rb3P
CrO3

2. Unit 7 Chemical Reaction
SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter.
Demonstrate the Law of Conservation of Matter in a chemical reaction.
Apply the Law of Conservation of Matter by balancing the following types of chemical equations;
Synthesis
Decomposition
Single Replacement
Double Replacement

3. 7.1 Describing Reactions What is the law of conservation of mass?
Why must chemical equations be balanced?
Why do chemists use the mole?
How can you calculate the mass of a reactant or product in a chemical reaction?

4. 7.1 Describing Reactions Chemical Equations
What is the law of conservation of mass?
Chemical Equations
Reactants – the substances that are present before a reaction
Products – the substances present after a reaction is complete
Always given in the form
Reactants  Products
Example:Carbon + Oxygen  Carbon Dioxide
Or C + O2  CO2

5. 7.1 Describing Reactions Writing Equations - Practice
What is the law of conservation of mass?
Writing Equations - Practice
Copper and Oxygen make Copper (II) Oxide
Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride
Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water.
Hydrogen and Chlorine combine to make Hydrogen Chloride

6. 7.1 Describing Reactions Conservation of Mass
What is the law of conservation of mass?
Conservation of Mass
Mass is not created or destroyed in a chemical reaction
For practical purposes
Same types of atoms before and after a reaction
Same number of each type of atom before and after
Equations must show this
They are called balanced equations

7. S-134 Write the formula for Dinitrogen Trioxide Copper (II) oxide
Dinitrogen Pentaoxide
Write the name for
CCl4
CrBr3
Mo2O5

8. S-135
Write the equation for a reaction of hydrogen sulfide with aluminum oxide to make aluminum sulfide and water.

9. 7.1 Describing Reactions Balancing Equations
Why must chemical equations be balanced?
Balancing Equations
If an equation does not have the same elements on both sides, it is a false equation
Can not actually occur
Coefficient – a number placed in front of a substance in a chemical equation
Used to balance equations

10. 7.1 Describing Reactions Balancing Equations - Steps
Why must chemical equations be balanced?
Balancing Equations - Steps
First write out the equation
Hydrogen and Oxygen make water becomes
H2 + O2  H2O
List the elements on each side
H-2  H-2
O-2 O-1
Add substances until both sides are equal

11. 7.1 Describing Reactions Balancing Equations - Practice
Why must chemical equations be balanced?
Balancing Equations - Practice
Copper and Oxygen make Copper (II) Oxide
Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride
Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water.

12. S-137 Balance the following equations
H2SO4 + Al(OH)3  Al2(SO4)3 + H2O

13. 7.1 Describing Reactions Counting With Moles A unit of measurement
Why do chemists use the mole? 18 Ar
Argon
Counting With Moles
A unit of measurement
Equals 6.02 x 1023 of anything
Used only to count atoms, molecules, formula unit
One mole of an element is equal to its atomic mass converted to grams (put a g beside the number)

14. 7.1 Describing Reactions Molar Mass
How can you calculate the mass of a reactant or product in a reaction?
Molar Mass
For an element equal to its atomic mass
For a compound
For each element – multiply the mass x the number of that element in the compound
Add the total

15. 7.1 Describing Reactions Molar Mass-Example C2H4
How can you calculate the mass of a reactant or product in a reaction?
Molar Mass-Example
C2H4
Carbon g x 2 = 24.02g
Hydrogen g x 4 = g
Total

16. 7.1 Describing Reactions Molar Mass-Example Pb(OH)4
How can you calculate the mass of a reactant or product in a reaction?
Molar Mass-Example
Pb(OH)4

17. S-137
What is the molar mass of
Al2(SO4)3

18. What are the general types of chemical reactions?
7.2 Types of Reactions
What are the general types of chemical reactions?

19. Types of Reactions Classifying Reactions
What are the general types of reactions?
Classifying Reactions
Describe how reactants interact to form products
Help to predict the products of reactions

20. Types of Reactions Synthesis
What are the general types of reactions?
Synthesis
Two or more substances react to form a single substance
Pattern A + B  AB
Always has one product
Examples
2Na + Cl2  2NaCl
2H2 + O2  2H2O

21. Types of Reactions Decomposition
What are the general types of reactions?
Decomposition
One substance breaks apart into two or more products
Pattern AB  A + B
Always has one reactant
Examples
CaCO3  CaO + CO2
2H2O  2H2 + O2

22. Types of Reactions Single Replacement (Displacement)
What are the general types of reactions?
Single Replacement (Displacement)
A compound switches parts with an element
Pattern A + BC  B + AC
Always has one element and one compound on each side
Examples
Cu + 2AgNO3  2Ag + Cu(NO3)2
2K + 2H2O  H2 + KOH

23. Types of Reactions Double Replacement (Displacement)
What are the general types of reactions?
Double Replacement (Displacement)
Two compounds switch parts
Often results in the formation of a precipitate
Pattern AB + CD  AD + CB
Always has two compounds on each side
Examples
Pb(NO3)2 + 2KI  PbI2 + 2KNO3
CaCO3 + 2HCl  CaCl2 + H2CO3

24. Types of Reactions Combustion Reacts rapidly with oxygen
What are the general types of reactions?
Combustion
Reacts rapidly with oxygen
Everything combines with oxygen
Pattern AB + O2  AO + BO
Always has oxygen as a reactant
Examples
CH4 + O2  CO2 + 2H2O
2Ca + O2  2CaO

25. S-138 Balance the following reactions and tell what type(s) they are.
Pb(NO3)2 + HCl  PbCl2 + HNO3
Ca + HCl  CaCl2 + H2

26. S-139
Write out the reaction, then balance it and tell what type it is.
Mercury reacts with oxygen to form Mercury (II) Oxide