Download Chemical Reactions

Chapter 11
L. Bernard, 2015
L. Bernard, 2015
Do Now!
L. Bernard, 2015
• The process by which atoms of the same or different
element rearrange themselves to form a new substance
• Bonds are broken between atoms and re-formed to
form new molecules
reactants  products
L. Bernard, 2015
•
•
•
•
•
•
•
Production of heat
Absorption of heat (gets cold)
Production of gas (bubbles)
Production of a precipitate (solid)
Change in color
Change in odor
Change in state of matter
L. Bernard, 2015
1.
2.
3.
4.
5.
Synthesis
Decomposition
Single-Replacement
Double-Replacement
Combustion
L. Bernard, 2015
• Also known as combination
• When two or more substances react to form a SINGLE
substance
L. Bernard, 2015
L. Bernard, 2015
• When a single substance breaks down into two or
more products
• Opposite of synthesis
L. Bernard, 2015
L. Bernard, 2015
• Where one element replaces another element in a
compound
• Essentially one element switches compounds
L. Bernard, 2015
L. Bernard, 2015
• When there is an exchange of POSITIVE IONS
between two compounds
• The cations exchange places
L. Bernard, 2015
L. Bernard, 2015
• Where an element or compound reacts with oxygen to
produce carbon dioxide and water
• Produces heat and light
L. Bernard, 2015
L. Bernard, 2015
• P4 + 3O2  2P2O3
• Synthesis!
• 2MgI2 + Mn(SO3)2  2MgSO3 + MnI4
• Double Displacement!
• C6H12 + 9O2  6CO2 + 6H2O
• Combustion!
• 2AgNO3 + Cu  Cu(NO3)2 + 2Ag
• Single Displacement!
L. Bernard, 2015
•
•
•
•
•
•
•
•
Pb + FeSO4  PbSO4 + Fe
P4 + 3 O2  2 P2O3
C6H12 + 9 O2  6 CO2 + 6 H2O
O3  O. + O2
2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag
2 MgI2 + Mn(SO3)2  2 MgSO3 + MnI4
2 NO2  2 O2 + N2
SeCl6 + O2  SeO2 + 3Cl2
L. Bernard, 2015
L. Bernard, 2015
• Law of Conservation of Mass
• Matter cannot be created nor destroyed
• Just like with math, both sides of the YIELDS sign must
be equal!
• So the same number of atoms must be on both sides
of the equation
L. Bernard, 2015
L. Bernard, 2015
1. Inspection
2. “ABC” Method
3. Combustion Trick
L. Bernard, 2015
• Use when it is easy to see the solution
1. List all the elements within the chemical equation
2. Count the number of elements on each side
3. Balance the coefficients and charges
L. Bernard, 2015
L. Bernard, 2015
• Algebraically solve for the coefficients
1. Assign a letter for each coefficient in the reaction
2. Determine an algebraic equation to solve for the
value of each coefficient
L. Bernard, 2015
L. Bernard, 2015
L. Bernard, 2015
L. Bernard, 2015
• Use only with combustion reactions!
1. Balance the carbon and hydrogen first using the
inspection method
2. Balance the number of oxygens last
•
In the reactants, oxygen will always be alone as O2
L. Bernard, 2015
2
2
4
4
4
L. Bernard, 2015
•Li + H2O → LiOH + H2
•K + B2O3 → K2O + B
•C6H6 + O2 → CO2 + H2O
L. Bernard, 2015
• Matter can be changed from one form to another
• Cannot be created or destroyed!
• Why must we balance equations?
L. Bernard, 2015