1. Writing and Balancing Equations

2. Chemical Reactions A chemical reaction is the process by which one or more substances are changed into different substances.

3. Reactants are the beginning substances in a chemical reaction (left of arrow). Products are the substances produced in a chemical reaction (right of the arrow).

4. Chemical equations – represent chemical reactions using formulas and symbols for the substances, their states, and other conditions. (NH 4 ) 2 Cr 2 O 7 (s) → N 2 (g) + Cr 2 O 3 (s) + 4 H 2 O (reactant) (products)

5. Law of Conservation of Mass – states that matter can neither be created or destroyed in a chemical reaction. It can only change forms. Antoine-Laurent de Lavoisier

6. Therefore, the same number of each kind of atom must be found on the left and on the right sides of a chemical equation. 2H 2 +O2O2 2H 2 O

7. Example: assuming all reactants are used completely 2H 2 + O 2 → 2H 2 O 5 grams 40 grams __ grams

8. Writing Balanced Equations Step 1 – Determine the reactants and products. Important – The following elements exist as diatomic molecules in their free (uncombined) state: O 2, H 2, N 2, Cl 2, Br 2, F 2, and I 2

9. Step 2 – Write the chemical equation with the correct symbols for all reactants and products. Step 3 – Balance the equation by adding coefficients to the front of formulas Hint: Balance elements that appear more than once on a side last.

10. Step 4 – Add symbols, when appropriate. COMMON SYMBOLS  yields (separates reactants from products)  heat required (this symbol is placed over the arrow) (l) liquid (aq) aqueous (dissolved in water) (g) gas ( an  is sometimes used for a gas product)

11. ( s) solid (and  is sometimes used for a precipitate) ( cr) crystalline solid **Note: A formula over the yield arrow indicates a catalyst.

12. Example 1

13. Example 2 CH 3 OH (l) + O 2 (g) → CO 2 (g) + H 2 O (g) Example 3 Liquid water is formed from the combining of hydrogen and oxygen gases. (Write the Chemical Equation)