1. Vocabulary To Go in Ch. 7 Notes: Grab a BOOK
Reactants
Products
Chemical Equation
Coefficients
Chemical Energy
Exothermic Reaction
Endothermic Reaction
Reaction Rate
Catalyst

2. Chemical Reactions
Chapter 7

3. Chemical Reactions Chemical Reaction Evidence of a Chemical Reaction
Rearranges atoms into different substances
Evidence of a Chemical Reaction
Temperature change
Production of light
Color change
Production of gas
Creation of a precipitate (solid)
end

4. Chemical Equations Chemical Equations 2 parts: Reactants Products
ON the LEFT
Products
ON the RIGHT
The State of Matter is with:
(s), (l), (g), (aq)
aq- aqueous (dissolved in water)
2 H2(g) + O2(g) 
2 H2O(l)
Yields/Forms/Produces
end

5. Chemical Equations Box the reactants and underline the products
2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
end

6. Chemical Equations The Law of Conservation of Matter
Matter CANNOT be created or destroyed!
Every atom at the start, must be at the end!
MUST BALANCE CHEMICAL EQUATIONS!!!
end

7. NEVER Change the Subscripts
Chemical Equations
Steps to balancing chemical equations:
Write Equation
List Elements
Multiply by Coefficients
Balance elements in 1 place first
NEVER Change the Subscripts
end

8. Chemical Equations Practice
___ N2 + ___ H2  ___ NH3
end

9. Practice
___ KClO3  ___ KCl + ___ O2

10. Practice
___ CH4 + ___ O2  ___ CO2 + ___ H2O

11. Practice ___ P + ___ O2  ___ P2O5
___ NaCl + ___ F2  ___ NaF + ___ Cl2

12. Practice

13. Balancing Polyatomic Ions
If there is a polyatomic ion in the chemical equation…COUNT IT AS A WHOLE
ONLY IF it has ( ) & is on both sides of the equation
FeCl3 + NaOH  Fe(OH) NaCl

14. Chemical Reactions There are 5 basic chemical reactions: Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
end

15. Chemical Reactions Synthesis A + B  AB ___ Mg + ___O2  ___ MgO
2 or more reactants combine to form 1 product
A + B  AB
___ Mg + ___O2  ___ MgO
end

16. Chemical Reactions Decomposition AB  A + B
1 reactant breaks down into 2 or more products
AB  A + B
___ H2O2  ___ O2 + ___ H2O
end

17. Chemical Reactions Single Replacement A + BC  AC + B
1 element replaces another element in a compound
A + BC  AC + B
__ Mg + __ HC2H3O2  __ Mg(C2H3O2)2 + __ H2
___Br2 + ___ MgI2  ___ MgBr2 + ___ I2
end

18. ___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
Chemical Reactions
Double Replacement
The reactants switch partners
AB + CD  AD + CB
Often produces water, a gas , or a solid
___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
end

19. Chemical Reactions Combustion ___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
Combine with oxygen give off heat and light
Forms CO2(g) and H2O(l)
___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
end

20. Chemical Reaction Classify the following: 2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
AgNO3 + NaCl  AgCl + NaNO3
2 C2H6 + 7 O2  4 CO2 + 6 H2O
end

21. Chemical Reaction
Complete #1-8 on “Classifying Chemical Reactions”

22. To Complete & Turn In Worksheet Balancing & Classifying Reactions
COMPLETE ALL!!!
#5 on Balancing Equations is a Challenge Problem)
Vocabulary & p. 198 #1-7 on Back of Worksheet

23. Bell Ringer What are the 5 types of chemical equations?
What does the law of conservation of matter state?
What type of Chemical Reaction are these:
Mg + 2HCl  MgCl2 + H2O -BALANCE
N2 + H2  2NH3 BALANCE

24. Quick Review from Yesterday

25. Chemical Reactions There are 5 basic chemical reactions: Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
end

26. Chemical Reactions Synthesis A + B  AB ___ Mg + ___O2  ___ MgO
2 or more reactants combine to form 1 product
A + B  AB
___ Mg + ___O2  ___ MgO
end

27. Chemical Reactions Decomposition AB  A + B
1 reactant breaks down into 2 or more products
AB  A + B
___ H2O2  ___ O2 + ___ H2O
end

28. Chemical Reactions Single Replacement A + BC  AC + B
1 element replaces another element in a compound
A + BC  AC + B
__ Mg + __ HC2H3O2  __ Mg(C2H3O2)2 + __ H2
___Br2 + ___ MgI2  ___ MgBr2 + ___ I2
end

29. ___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
Chemical Reactions
Double Replacement
The reactants switch partners
AB + CD  AD + CB
Often produces water, a gas , or a solid
___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
end

30. Chemical Reactions Combustion ___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
Combine with oxygen give off heat and light
Forms CO2(g) and H2O(l)
___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
end

31. Chemical Reaction Classify the following: 2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
AgNO3 + NaCl  AgCl + NaNO3
2 C2H6 + 7 O2  4 CO2 + 6 H2O
end

32. Write down the following formulas in your BR notebook
DEMO DAY
Write down the following formulas in your BR notebook

33. DEMO #1 A + B  AB ___ Mg + ___O2  ___ MgO
2 or more reactants combine to form 1 product
A + B  AB
___ Mg + ___O2  ___ MgO
end

34. DEMO #2 AB  A + B ___ H2O2  ___ O2 + ___ H2O
1 reactant breaks down into 2 or more products
AB  A + B
___ H2O2  ___ O2 + ___ H2O
end

35. DEMO # 3 A + BC  AC + B __ Mg + __ HC2H3O2  __ Mg(C2H3O2)2 + __ H2
1 element replaces another element in a compound
A + BC  AC + B
__ Mg + __ HC2H3O2  __ Mg(C2H3O2)2 + __ H2
___Br2 + ___ MgI2  ___ MgBr2 + ___ I2
end

36. ___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
DEMO #4
The reactants switch partners
AB + CD  AD + CB
Often produces water, a gas , or a solid
___ Pb(NO3)2 + ___ KI  ___ PbI2 + ___ KNO3
end

37. DEMO #5 Combustion ___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
Combine with oxygen give off heat and light
Forms CO2(g) and H2O(l)
___ C2H5OH + ___ O2  ___ CO2 + ___ H2O
end

38. CHEMICAL REACTION DEMONSTRATIONS & BALANCING THEIR EQUATIONS
You are to make your own observations per demonstration and write them down, you are also to make an educated guess as to what type of chemical reaction is taking place.

39. Bell Ringer : TURN IN BALANCING WORKSHEET
1) What can this symbol stand for in a chemical equation: 
Circle the reactants, and underline the products in the following chemical equations:
FeO3(s) + CO(g) --> Fe(l) + CO2(g)
H2SO4 + Pb(OH) --> Pb(SO4)2 + H2O
2) What do the letters (s), (g), (l) in the first chemical equation stand for?
3) What types of chemical reactions are above?
4) How many types of Reactions are there?

40. Identify Type of Chemical Reaction and Balance:
1) ___Na3PO4 + ___KOH --> ___NaOH + ___KPO4
Type: _____________________________
2) ___P4 + ___O2 --> ___P2O5
Type:________________________
3) ___C3H6O + ___O2 --> ___CO2 + ___H2O
4) ___ NO2 --> ___O2 + ___N2
Type: _______________________
5) ___AgNO3 + ___Cu --> ___Cu(NO3)2 + ___ Ag

42. Energy Changes Chemical Energy Exothermic Endothermic
Stored in chemical bonds
Changed during a chemical reaction
Exothermic
Give off energy
Produces heat/light
Endothermic
Takes in energy
Gets cold
end

43. Energy Changes Exothermic Reaction Gives OFF Energy
Produces heat and/or light
Instant heating pad, glow sticks
Energy written as a PRODUCT
AB + CD  AD + CB + energy
Na + Cl2  NaCl + 411kJ
Energy
end

44. Energy Changes In an exothermic reaction:
Reactants HIGHER than Products
More energy
end

45. Energy Changes Endothermic Reaction Takes IN Energy Gets colder
Instant icepacks
Energy written as a REACTANT
AB + CD + energy  AD + CB
15000 kJ + 6 CO2 + H2O  C6H12O6 + 6 O2
Energy
end

46. Energy Changes In an endothermic reaction:
Reactants LOWER than Products
Less energy
end

47. Reaction Rates Reaction Rate Speed that Reactants become Products
5 ways to make reactions go faster:
end

48. Reaction Rates Temperature Surface Area Adding Heat = Move Faster
Move Faster = Faster Reaction
Surface Area
Grind into a powder
More Surface Area = Faster Reaction
end

49. Reaction Rates Stirring Concentration Moves things around
More Movement = Faster Reaction
Concentration
More Reactants = Easier to Combine
Easier to Combine = Faster Reaction
end

50. Reaction Rates Catalyst Speeds up a reaction without being used
Lowers energy needed start the reaction
The size of the hill
Less Energy Needed = Faster Reaction
end