1. Indicators of a chemical reaction- Color change Producing a gas Heat/light energy released Formation of a precipitate

2. Chemical equation - Describes a chemical change. Parts of an equation: Zn + 2HClZnCl 2 + H 2 ReactantProduct Reaction symbol Coefficient

3. Reactant - The chemical(s) you start with before the reaction. Written on left side of equation. Product - The new chemical(s) formed by the reaction. Right side of equation.

4. Subscript - shows how many atoms of an element are in a molecule. EX: H 2 O 2 atoms of hydrogen (H) ‏ 1 atom of oxygen (O) ‏ Coefficient - shows how many molecules there are of a particular chemical. EX: 3 H 2 O 6 atoms of hydrogen (H) 3 atoms of oxygen (O)

5. 2H 2 + O 2  2H 2 O

6. Lavoisier: Matter is neither created nor destroyed in a chemical reaction. In other words, the number and type of atoms going INTO a reaction must be the same as the number and type of atoms coming OUT. If an equation obeys the Law of Conservation, it is balanced.

7. CH 4 + O 2  CO 2 + H 2 O Reactant SideProduct Side 1 carbon atom 4 hydrogen atoms 2 oxygen atoms 1 carbon atom 2 hydrogen atoms 3 oxygen atoms

8. A Balanced Equation CH 4 + 2O 2  CO 2 + 2H 2 O Reactant SideProduct Side 1 carbon atom 4 hydrogen atoms 4 oxygen atoms 1 carbon atom 4 hydrogen atoms 4 oxygen atoms

9. 1. Matter cannot be created or destroyed. 2. Subscripts cannot be added, removed, or changed. 3. You can only change coefficients. 4. Coefficients can only go in front of chem. formulas...NEVER in the middle of a formula. A few extra tips: Try balancing big formulas first; save free elements for last. If the same polyatomic ion appears on both sides of the equation, it’s usually okay to treat it as one unit. There is no one particular way to balance equations. Some equations are harder to balance than others and might require some creativity to solve.

10. Balance the following equation by adjusting coefficients. reactantsproducts N H N 2 + H 2  NH 3 2 2 1 3 2 2 6 3 6

11. Balance the following equation by adjusting coefficients. KClO 3  KCl + O 2 reactantsproducts K Cl O 1 1 1 1 3232 2 2 66 2 2 2

12. Balance the following equation: C 2 H 6 + O 2  CO 2 + H 2 O4672

13. Balance the following equation: Fe + O 2  Fe 2 O 3234

14. Chemical Reaction Types synthesis – reaction where 2 or more substances combine to form one A + B → AB Ex: 2H 2 + O 2 → 2H 2 O decomposition – reaction where a compound decomposes(breaks apart) into multiple substances AB → A + B Ex: 2KClO 3 → 2KCl + 3O 2 single replacement - single element replaces another element in a compound A + BC → AC + B Ex: 2Ag + FeCl 2 → Fe + 2AgCl My Mole-called Life AKA Mole-sterpiece Theatre

15. Chemical Reaction Types Continued… Double replacement - two elements in different compounds switch places AB + CD → AD + BC Ex: NaOH + HCl → NaCl + HOH(H 2 O) Combustion Reaction - Hydrocarbon combines with oxygen to form water and carbon dioxide hydrocarbon – any compound made from carbon and hydrogen hydrocarbon + O 2 → CO 2 + H 2 O Ex: C 2 H 4 + 3O 2 → 2CO 2 + 2H 2 O My Mole-called Life