1. Chemical Reactions

2. definition
Chemical reactions are processes in which one or more substances are converted into a new substance with different physical and chemical properties
In a chemical reaction, the atoms of the starting substance (reactants) are rearranged to produce a new substance (products).
The law of conservation of mass/matter is obeyed. This law states mass/matter can’t be created or destroyed, it simply changes form.

3. Signs a chemical reaction has occurred
Energy is absorbed (endothermic) or released (exothermic) so there will be a change in temperature)
Sometimes there is a change in color
Sometimes a precipitate (solid) forms
Sometimes a gas forms (bubbles)
Sometimes there is a change in odor

4. Representing Chemical Reactions
Words
Iron and chlorine react to produce iron (III) chloride
The reaction between carbon and sulfur yields carbon disulfide
Skeleton Equation
Fe + Cl2  FeCl3
C(s) + S(s)  CS2

5. Cont’d
Balanced Chemical Equation- shows the correct formulas for reactants and products and uses coefficients to reflect the law of conservation of mass (same # of atoms of each element on both sides of the equation arrow)
2Fe + 3Cl2  2FeCl3
C(s) + 2S(s)  CS2

6. Method for balancing Equation
Write skeleton equation
Count the atoms of each element on reactant side of the equation
Count the atoms of each element on product side of the equation
*** if a polyatomic ion appears on both sides, count it as a unit
Use coefficients to make the number of atoms (or ions) of each type equal on both sides of equation
Write coefficients in their lowest whole number ratio possible
If an element is in more than one compound on the same side of equation, wait until you have balanced all the other elements

7. Classifying Chemical reactions
There are five main types of chemical reactions:
Synthesis
Decomposition
Single replacement (or displacement)
Double replacement (or displacement)
Combustion

8. Synthesis
A reaction in which two or more substances react to form a single product
A + B  C
Ex: 2Na + Cl2  2NaCl

9. Decomposition
A reaction in which a single substance breaks down into two or more elements or new compounds
C  A + B
Ex: 2KClO3  2KCl + 3O2

10. Single replacement
A reaction in which the atoms of one element replace the atoms of another element in a compound
A + BC  AC + B
(where A and B are metals) or
X + BY  Y + BX
(where X and Y are halogens)
Ex: Zn + CuSO4  ZnSO4 + Cu
Br2 + 2KI  2KBr + I2

11. Double replacement
A reaction which involves an exchange of ions between two compounds
AB + CD  AD + CB
Ex: Ca(NO3)2 + H2SO4  CaSO4 + NaNO3

12. Combustion
(sometimes synthesis reactions are also combustion reactions)
A reaction in which oxygen combines with a substance to produce oxides of the elements in the substance (and releases energy in the form of heat and light)
CxHy + O2  CO2 + H2O
Ex: CH4 + O2  CO2 + H2O