1. Chemical Equations
A _____________________represents, with symbols and formulas, the reactants and products in a chemical reaction
____________ are shown on the left hand side of the arrow
____________ are shown on the right hand side of the arrow
The arrow means “produces”, “yields”, or “reacts to form”
Chemical equations may also include abbreviations to denote the state of matter of the reactants and products:
(s) for _______________
(l) for ________________
(g) for ____________
(aq) for _________, which means dissolved in ____ (in solution)

2. HC2H3O2(__) + NaHCO3(__)  CO2(__) + H2O(__) + NaC2H3O2(___)
N2(g) + H2(g)  NH3(g)
HC2H3O2(__) + NaHCO3(__)  CO2(__) + H2O(__) + NaC2H3O2(___)
The equations above are called ________________________ because they represent the reactants and products of a reaction using their symbols and formulas
A word equation can be written using the names of the reactants and products

3. Why balance equations? 2H2O  2H2 + O2
In any chemical reaction, mass is conserved (meaning that the ____________________________________________ _____________________________)
A balanced chemical equation shows ___________________ _________________ of each element or compound react to exactly form the products
_______________________ are placed in front of formulas to show how many moles of that element/compound are needed in the equation
Coefficients must be whole numbers
Example:
2H2O  2H2 + O2

4. To balance a chemical equation
Steps to balance an equation:

5. Fe(OH)3 + BaCl2  FeCl3 + Ba(OH)2
Example #1
H2 + Cl2 HCl
Example #2
Fe(OH) BaCl2  FeCl Ba(OH)2

6. Example #3
Magnesium chloride reacts with silver nitrate to form solid silver chloride and magnesium nitrate

7. Types of Chemical Reactions
There are many different types of chemical reactions that will be studied throughout the year
In this unit, we will investigate 5 main types of reactions

8. __________________Reaction
In a synthesis reaction, two or more reactants come together to form _____________________
EXAMPLE:
Magnesium and oxygen react to form magnesium oxide:

9. _____________________ Reaction
In a decomposition reaction, a _________________breaks apart to form more than one product (the _____________ of a synthesis reaction)
EXAMPLE:
Silver oxide decomposes into solid metallic silver and oxygen gas

10. _________________________Reaction
In a single replacement reaction, one element ___________ another element in a compound, leaving the element by itself
EXAMPLE:
Aluminum reacts with copper(II) chloride to form copper metal and aluminum chloride

11. _________________________Reaction
In a double replacement reaction, _______________________ places, forming two new ionic compounds
EXAMPLE:
Silver nitrate solution reacts with sodium chloride solution to form solid silver chloride and aqueous sodium nitrate:

12. ___________________ Reaction
In a combustion reaction, a hydrocarbon (or compound containing carbon, hydrogen, and/or oxygen) reacts with _________________, forming carbon dioxide and water
Many different types of carbon compounds can provide the “fuel” for a combustion reaction…

13. Example __CH4 + __O2  __CO2 + __H2O
Methane reacts with oxygen gas, forming carbon dioxide and water
__CH4 + __O2  __CO2 + __H2O

14. Practice
Write and balance equations for the following combustion reactions:
Combustion of hexane (C6H14)
Combustion of methanol (CH3OH)