1. Reactions Physical Change Chemical Change
Change in appearance, but not composition. Examples are phase changes, tearing, ripping, color changes (sometimes)
Change of one substance into another. Examples include rusting, burning, color change (sometimes).

2. Reactions Indicators of a chemical change include:
- Change in temperature
- Gas/Odor given off
- Color change
- Heat/light given off
- Precipitate formed. A precipitate is a solid that comes out of solution

3. Chemical Equations
Another name for a chemical change is a chemical reaction where one or more substances are rearranged to form different substances.
Chemists use equations to represent chemical reactions.
Coefficient
Subscript
Parts of a chemical equation:
2H H2O
Reactants
Products
Yields

4. Law of Conservation of Mass and Conservation of Matter
The law of conservation of mass states that in a chemical reaction, mass is conserved. That means that the mass you start with must= the mass you end with.
Example:
CuCl2 + Al AlCl3 + Cu
The law of conservation of matter states that the same number and type of atom you start with must = the number and type you end with.
3CuCl2 + 2Al AlCl3 + 3Cu
10.2 g
10.2 g =

5. Balancing Chemical Equations
Solid Iron and gaseous chloride react to product a solid iron (III) chloride
1. Write the skeleton equation for the reaction
Symbol
Meaning +
Separates two or more reactants or products 
Separates reactants from products
(s)
Identifies a solid state
(l)
Identifies a liquid state
(g)
Identified a gaseous state
(aq)
Identifies water solution

6. Symbols for Equations Symbol Meaning +  (s) (l) (g) (aq)
Separates two or more reactants or products 
Separates reactants from products
(s)
Identifies a solid state
(l)
Identifies a liquid state
(g)
Identified a gaseous state
(aq)
Identifies water solution

7. Balancing Chemical Equations
Fe(s) + Cl2(g)  FeCl3
2. Count the atoms of the elements in the reactants

8. Balancing Chemical Equations
Fe(s) + Cl2(g)  FeCl3
3. Count the atoms of the elements in the products
Reactants
Products Fe 1 Cl 2

9. Balancing Chemical Equations
Fe(s) + Cl2(g)  FeCl3
4. Change the coefficients to make the number of atoms of each element equal on both sides of the equation
Reactants
Products Fe 1 Cl 2 3

10. Balancing Chemical Equations
2Fe(s) + 3Cl2(g)  2FeCl3
5. Write the coefficients in their lowest possible ratio

11. Balancing Chemical Equations
2Fe(s) + 3Cl2(g)  2FeCl3
6. Check your work

12. Al(OH)3(s) + HCl(aq)  AlCl3(aq) + H2O(l)

13. Types: Combination Combination/ Synthesis/ Composition
Def: 2 or more substances react to form 1 product. Usually releases energy, exothermic
A + X  AX
4 Fe (s) O2 (g)  2 Fe2O3 (s)
CaO (s) + H2O (l) Ca(OH)2 (s)

14. CaCO3 (s)  CaO (s) + CO2 (g)
Types: Decomposition
Def: A single compound breaks down into 2 or more elements or compounds
AX  A + X
2NaN3(s)  2Na(s) + 3N2 (g)
2KClO3 (s)  2KCl (s) + 3O2 (g)
CaCO3 (s)  CaO (s) + CO2 (g)
***Often Requires and energy source as an initiator. Energy sources can be heat, light, or electricity. Usually endothermic.

15. Types: Combustion
Def: Oxygen gas combines with a substance and releases energy in the form of light or heat. So combustion reactions are usually exothermic.
A + O2 
C(s) + O2(g)  CO2(g) + energy
4 Fe (s) + 3O2 (g)  2Fe2O3 (s) + energy
For hydrocarbons:
CxHy + [x + (y/4)] O2  xCO2 + (y/2)H2O
C3H8(g) O2(g)  CO2 (g) H2O (g) + light + heat

16. Types: Single Replacement/ Displacement
Def: A reaction in which the atoms of 1 element replace the atoms of another element in a compound.
A + BX  AX + B, where A = metal OR
BX + Y  BY + X, where Y = halogen
Li (s) H2O(l)  LiOH (aq) H2(g)
Cu (s) + 2AgNO3 (aq)  2Ag (s) + Cu(NO3)2 (aq)
F2 (g) + 2NaBr(aq)  2NaF(aq) + Br2(l)

17. Types: Double Replacement/ Displacement
Def: 2 compounds exchange ions to produce 2 new compounds.
AX + BY  AY + BX
K2CO3 (aq) + BaCl2 (aq)  2KCl (aq) + BaCO3 (s)
HCl (aq) + NaOH (aq)  H2O (l) + NaCl (aq)
2HI(aq) + Li2S(aq)  H2S(g) + 2LiI (aq)

18. Bonfire
Mass change of substance is evidence

19. 1. 2. Title: Indicators of a Chemical Reaction
Concept: Chemical Reactions
Descriptions: Each Image would be used to guide students into making a list that describes characteristics of chemical reactions. Characteristics of the reaction in each image are as follows: 1. Fire- smoke, heat energy, light energy, color change of products vs. reactants, and oder
2. Rust- a new substance forms (precipitate), color change of products
3. glowing solutions- fluorescence (color change for them)
4. Angel Cake- the rising dough from the formation of gas bubbles
Fire:
Copyright- January 2005
Credits- U.S. Department of the Interior, U.S. Geological Survey
Rust:
Copyright- none provided
Credits- Wikipedia
Fluorescence:
Angel Food Cake:
Copyright- 2007
Credits- Allrecipes.com, LatinaCook 2.

20. ???Do Now 03/16/07???
Write and balance the given equation. Indicate the type of chemical reaction represented.
a. Aluminum metal reacts with hydrochloric acid to produce hydrogen gas and aluminum chloride.
b. Iron (III) nitrate reacts with ammonium hydroxide to produce iron (III) hydroxide and ammonium nitrate.
c. Ammonium dichromate is heated to produce chromium (III) oxide, nitrogen, and water.

21. Predicting Products Synthesis/Combination
Solid aluminum reacts with solid iodine to produce?
Sodium and gaseous chlorine react to form?

22. Predicting Products Synthesis/Combination
Solid magnesium reacts with oxygen gas
to produce?
Solid iron and chlorine gas react to produce? Fe(III) product

23. Predicting Products Decomposition
Sodium Azide decomposes into?
Silver chloride decomposes to produce?

24. Predicting Products Decomposition
Magnesium bromide decomposes into?
Cobalt (II) oxide decomposes into?

25. Predicting Products Combustion
Aqueous ethanol (C2H6OH) reacts with oxygen to produce?
Solid barium reacts with oxygen to produce?

26. Predicting Products Combustion
Liquid acetone (C3H6O) reacts with oxygen to produce?
Solid boron reacts with oxygen to produce?

27. Replacement/ Displacement
Single: A reaction in which the atoms of 1 element replace the atoms of another element in a compound.
A + BX  AX + B, where A = metal OR
BX + Y  BY + X, where Y = halogen
Double: 2 compounds exchange ions to produce 2 new compounds.
AX + BY  AY + BX
In an aqueous solution and it results in either a gas, a precipitate, or liquid water as one of the products
Precipitate: a solid produced during a chemical reaction in a solution.

28. Single Replacement Activity Series
Metals
Halogen
Activity Series Li K Ca Na Mg Al Zn Fe Ni Sn H Cu Ag Au
Most Active F Cl Br I
Most Active
Least Active
F2 (g) + 2NaBr(aq)  2NaF(aq) + Br2(l)
Li (s) H2O(l)  LiOH (aq) H2(g)
Cu (s) + 2AgNO3 (aq)  2Ag (s) + Cu(NO3)2 (aq)
Least Active

29. Predicting Products Single Replacement
Iron metal reacts with copper (II) sulfate to yield?
Liquid Bromine reacts with magnesium chloride to yield?
Magnesium metal reacts with aluminum (III) chloride to yield?

30. Predicting Products Single Replacement
Zinc Metal reacts with sulfuric acid to produce?
Iron metal reacts with lead (II) nitrate to yield? Fe (II) product
Chlorine gas reacts with sodium iodide to yield?

31. Predicting Products Double Replacement
Calcium Iodide reacts with mercury (II) nitrate to yield?
Sulfuric acid reacts with Aluminum hydroxide to yield?
Ammonium chloride reacts with silver sulfate to yield?

32. Predicting Products Double Replacement
Barium nitrate reacts with phosphoric acid
Iron (II) sulfide reacts with hydrochloric acid
#1 on your HW sheet
Hydrochloric acid reacts with sodium hydroxide

33. C2H3OOH(aq) + NaHCO3 (aq)  H2CO3 (aq) + C2H3OONa (aq)
Double Displacement:
Form: AX + BY  BX + AY
Precipitate: K2CO3 (aq) + BaCl2 (aq)  2KCl (aq) + BaCO3 (s)
Produce Water: HCl (aq) + NaOH (aq)  H2O (l) + NaBr (aq)
Produce Gas: HI(aq) + Li2S(aq)  H2S(g) + 2LiI (aq)
Demo? Which type of product was formed?
1. baking soda and vinegar
C2H3OOH(aq) + NaHCO3 (aq)  H2CO3 (aq) + C2H3OONa (aq)
H2CO3 (aq)  H2O (l) + CO2 (g)
2. MgSO4 (aq) + NaOH (aq)  Mg(OH)2 (s) + Na2SO4 (aq)

34. ???Do Now 03/20/07???
Predict the products. Balance the equation. Write the net ionic equation.
Au (s) Al(NO3)3 (aq)
K(s) H2O (l) 
H2SO4 (aq) + BaCl2(aq) 
AgNO3 (aq) + HCl (aq) 