1. Chemical Equations and Chemical Reactions

2. Chemical Equations
Representing a reaction in sentence form can be quite complex.
Chemical reactions can be written in the form of chemical equations.
Chemical equations are the “recipes” for the chemical reaction.

3. 5 Parts of a Chemical Equation
Reactants
Elements or compounds at the beginning of the reaction
Products
Elements or compounds that are formed as a Result of a chemical reaction
Yield
Arrow
Separates the reactants from the products
Coefficients
Numbers in front of the chemical formula
Shows the number of molecules
Subscripts
Small numbers behind the element or compound
Shows the number of atoms in each substance.

4. Label the Parts of a Chemical Equation
Yield
Reactants
Products
Subscripts
Coefficients

5. R C P
How Many Oxygen Atoms are on the Product Side?
How Many Elements are in this Chemical Formula?
How Many Water Molecules are on the Reactant Side? 6
= 18 12 C O H 6
18 = 12

6. Law of Conservation of Mass
“During a chemical reaction, atoms are neither created nor destroyed. The number of atoms remains constant throughout the reaction. Since the number of atoms doesn’t change, the mass must remain constant as well.”

7. Conservation of Mass
No atoms are destroyed and no new atoms are produced during a chemical reaction.
Instead, the atoms in the reactants are simply rearranged to form the products.
Chemical bonds between atoms are broken and new ones are formed and the atom simply reconnect in new ways.

10. Balancing Chemical Equations
A chemical equation that is complete except for coefficients is called an unbalanced equation or skeleton equation.
Example:
Skeleton Equation
H2 + O2  H2O
Balanced Equation
2H2O + O2  2H2O

11. How to Balance Equation
Begin by counting the number of atoms of each element.
Balance by placing COEFFICIENTS in front of the chemical formulas until the number of atoms in the reactants equals the products.
USE ONLY WHOLE NUMBERS
NEVER change a subscript.

14. Ask yourself “Has something new been created/destroyed?”
If so a chemical change/reactions has occurred.

15. Chemical Change
When a formation of new substances takes place with different chemical properties it is called chemical changes.
A chemical reaction is always accompanied by a chemical change.
Reaction is the term used for depicting a change or transformation.

16. Physical Change
A physical change in a substance doesn't change what the substance is.
whipping egg whites (air is forced into the fluid, but no new substance is produced)
H2O transforming from Solid to Liquid State. The Ice cube is melting but the chemical substance is still H2O
boiling water (water molecules are forced away from each other when the liquid changes to vapor, but the molecules are still H2O.)

17. Chemical Change
In a chemical change where there is a chemical reaction, a new substance is formed and energy is either given off or absorbed.
iron rusting (iron oxide forms)
gasoline burning (water vapor and carbon dioxide form)
eggs cooking (fluid protein molecules uncoil and crosslink to form a network)
bread rising (yeast converts carbohydrates into carbon dioxide gas)

18. Signs of a Chemical Reaction
Please
Precipitate
Excuse
Energy Change
Exothermic - Heat Given Off
Endothermic – Cold Given Off
Production of Light
Burps
Bubbles (Gas is Formed)
Coughs
Unexpected color change
Sneezes
Smell produced

19. Please P in Please stands for PRECIPITATE 2 liquid make a Solid
Precipitate is an insoluble solid that emerges from a liquid solution.

20. Excuse E in Excuse stands for Energy Change. Light is produced
Two types of energy change:
Endothermic (COLD)
Energy is absorbed, causing temperatures to DECREASE
Exothermic (HOT)
Energy is released, causing temperatures to INCREASE

21. Energy Change
Light Production

22. Burps B in Burps stands for Bubbles
If you see bubbles, a gas has been produced

23. Coughs C in Coughs stands for Color change
This change in color must be UNEXPECTED

24. Sneezes
S in Sneezes stands for production of smell