1. TURN IN OLD WARMUP SHEET!
What is a chemical reaction?
List the 5 types of chemical reactions.

2. Chemical Reactions

3. You need your green sheet for today

4. What is a Chemical Reaction?
Scientific Definition: A process in which physical and chemical properties of the original substance change as existing bonds are broken and new bonds are formed, producing new substances with different physical and chemical properties.
Simple Definition: A process that forms one or more new substances

5. Evidence of Chemical Reactions
Change in temperature
Unexpected change in color
Change in odor
Formation of a precipitate
Formation of a gas

6. Chemical Equation Vocab
Reactant – substance that is consumed
Product – substance that is formed
Catalyst – substance that speeds up a reaction, but is NOT consumed
Coefficient – number that shows how many molecules of a substance are consumed or produced
Physical State – symbol showing the state of matter of each substance in the reaction
(s) = solid
(l) = liquid
(g) = gas
(aq) = aqueous (dissolved in water)

7. Chemical Equations

8. Chemical Equations Word Equations: Formula Equations:
Calcium metal reacts with oxygen gas to form calcium oxide.
Water decomposes into hydrogen gas and oxygen gas.
Formula Equations:
2 Ca (s) + O2 (g)  2 CaO (s)
2 H2O (l)  2 H2 (g) + O2 (g)

9. Synthesis 2 or more reactants form one product
2 Na (s) + Cl2 (g)  2 NaCl (s)
CaO (s) + H2O (l)  Ca(OH)2 (aq)
CO2 (g) + H2O (l)  H2CO3 (aq)

10. Decomposition One reactant forms 2 or more products
2 KCl (s)  2 K (s) + Cl2 (g)
CaCO3 (s)  CaO (s) + CO2 (g)
2 NaHCO3 (s)  Na2CO3 (s) + H2O (l) + CO2 (g)
2 KOH (s)  K2O (s) + H2O (l)
2 NaClO3 (s)  2 NaCl (s) + 3 O2 (g)
H2CO3 (aq)  CO2 (g) + H2O (l)

11. Single Replacement
An element and a compound react to form a different element and compound
Zn (s) + CuSO4 (aq)  ZnSO4 (aq) + Cu (s)
2 Li (s) + 2 H2O (l)  2 LiOH (aq) + H2(g)
Zn (s) + 2 HCl (aq)  ZnCl2 (aq) + H2 (g)
2 NaBr (aq) + Cl2 (g)  2 NaCl (s) + Br2 (g)

12. Double Replacement 2 compounds react to form 2 different compounds
CaCl2 (aq) + 2 AgNO3(aq)  Ca(NO3)2 (aq) + 2 AgCl (s)
HCl (aq) + NaOH (aq)  NaCl (aq) + H2O (l)

13. Combustion
A hydrocarbon reacts with oxygen producing carbon dioxide, water vapor, and heat.
CH4 (g) + 2 O2 (g)  CO2 (g) + 2 H2O (g)
C2H5OH (g) + 3 O2 (g)  2 CO2 (g) + 3 H2O (g)

14. Writing equations practice

15. Warm-Up
What are the 7 diatomic elements?

16. Warm-Up
What are the 7 diatomic elements?

17. Balancing reactions
In the late 18th century Antoine Lavoisier prove the Law of Conservation of Mass, which states that matter cannot be created or destroyed
What does that mean for a chemical reaction?
The number of each reactant atom must equal the number of each product atom!

18. Balancing a reaction
Draw a vertical line under the arrow to separate the reactant side from the product side.
Identify the different elements on each side and list them below each side of the equation.
Count the number of each type of atom on each side of the reaction and list the amounts next to the symbols in your lists.

19. Balancing a reaction
Make the number of each type of atom on both sides equal. We use coefficients to do this. Notice that when a coefficient is put in front of a compound, it multiplies the number of atoms of ALL elements that make up that compound (i.e. multiplies the subscript of each atom).
Typically, you’ll have to add in more than one coefficient to completely balance the reaction. It helps if you do ONE element at a time in the following order (MeNOH):
Metals
Nonmetals (except Oxygen and Hydrogen)
Oxygen
Hydrogen

20. Balancing a reaction
Fe + O2  Fe2O3

21. Fe2(SO4)3 + KOH  K2SO4 + Fe(OH)3
Balancing a reaction
Fe2(SO4)3 + KOH  K2SO4 + Fe(OH)3

22. Balancing a reaction
C9H20 + O2  CO2 + H2O

23. Balancing a reaction
Nonmetals (except Oxygen & Hydrogen)
Oxygen
Hydrogen
Make the number of each type of atom on both sides equal. We use coefficients to do this. Notice that when a coefficient is put in front of a compound, it multiplies the number of atoms of ALL elements that make up that compound (i.e. multiplies the subscript of each atom).
Typically, you’ll have to add in more than one coefficient to completely balance the reaction. It helps if you do ONE element at a time in the following order (MeNOH):
Metals

24. Warm-Up
Write and balance the formula equation for the following reaction. Include all states of matter!
Solid aluminum oxide reacts with carbon monoxide gas, yielding aluminum metal and carbon dioxide gas.

25. Warm-Up
Write and balance the formula equation for the following reaction. Include all states of matter!
Solutions of phosphoric acid and magnesium hydroxide are mixed, yielding water and aqueous magnesium phosphate.

26. Warm-Up
Write and balance the formula equation for the following reaction. Include all states of matter!
Sulfur dioxide gas combines with oxygen gas to form sulfur trioxide gas.

27. Warm-Up Predict the products for each reaction below AND balance them.
Sr (s) + P4 (s) 
CaCO3 (s) 

28. Warm-Up Will the following reactions happen? Li + NaCl Co + AlCl3
Sb + AuCl3
Mn + ZnCl2
Na + BaCl2
Cr + KCl