1. Chemical Reactions
Chapter 10

2. 10.1 Reactions and Equations
The process by which the atoms of one substance are rearranged to form different substances is called a chemical reaction.
Subscript Yield
CH4 + 2 O2  CO2 + 2 H2O
Reactant Product

3. A chemical reaction has taken place when:
-Temperature change
-Color change
-A gas is produced
An odor is produced
Precipitation is formed
Matter cannot be created nor destroyed. Coefficients are added to have equal amounts of reactants as products.

4. Symbols + (a plus sign) separates two or more reactants or products
 (an arrow) separates reactants from products.
(s) = solid state
(l) = liquid state
(g) = gaseous state
(aq)= aqueous state or ( in water solution)

5. Word equations
Example: “ Solid iron and chlorine gas react to produce iron(III) chloride solid” Skeleton equations= changing the word equation into symbols Example: Fe(s) + Cl2  FeCl3 (s) Don’t forget about your diatomic molecules= H2 N2 O2 F2 Cl2 Br2 I2

6. Common mistakes Don’t forget to swap and drop
Don’t forget roman numerals= the charge
Fe (III) = Fe+3
If it ends with an –ide its bonded Ex: Hydrogen Chloride= HCl
If it end with an –ine its just the element Ex: Chlorine= Cl2

7. Examples
Solid carbon and solid sulfur decompose to make carbon disulfide.
Skeleton=

8. Examples
Hydrogen gas and bromine gas combine to produce hydrogen bromide gas.
Carbon monoxide gas and oxygen gas combine to produce carbon dioxide gas.

9. Example Potassium chlorate(s)  potassium chloride(s) + oxygen (g)
On your own do questions on pg 875 section questions 1-8