BALANCING EQUATIONS

1. BALANCING EQUATIONS

2. LEARNING OUTCOMES You Should Be Able To… 1. Define and explain the law of conservation of mass 2. Represent chemical reactions and the conservation of atoms, using molecular models 3. Write and balance (using the lowest whole number coefficients) chemical equations

3. VOCABULARY • Subscript - (of a letter, figure, or symbol) written or printed below the line • Coefficient - a coefficient is a constant by which a variable is multiplied. • Law of Conservation of Mass - in a chemical reaction, the mass of the products equals the mass of the reactants. • Molecule -a molecule refers to two or more atoms which have chemically combined to form a single species.

4. Compound - A compound is a chemical species that is formed when two or more atoms join together chemically, with covalent or ionic bonds. A type of molecule. All Compounds are molecules but Not all molecules are compounds. Molecule Examples H2O, O2, O3 Compound Examples NaCl, H2O

5. Balanced Equation - the mass and the charge are balanced on both sides of the reaction. • Reactant – Starting materials in a chemical reaction. • Product – substance formed as a result of a chemical reaction.

6. 4.3: Balancing Equations • Chemical reactions result in chemical changes. • Chemical changes occur when new substances are created. • The original substance(s), called reactants, change into new substance(s) called products. Products Reactants

7. 4.3: Balancing Equations Products Reactants

8. 4.3: Balancing Equations • Chemical reactions can be written in different ways. • A word equation: • Nitrogen monoxide + oxygen  nitrogen dioxide • A symbolic equation: • 2NO(g) + O2(g) 2NO2(g) • STATE OF MATTER • Letters indicate the state of each compound. • (aq) = aqueous/dissolved in water • (s) = solid • (l) = liquid • (g) = gas • COEFFICIENTS • Indicates how many of each molecule there is. • Ie: there are 2 molecules of NO.

9. Law of Conservation of Mass • When a chemical reaction occurs, new compounds are created, BUT… • No new matter is created or destroyed; atoms are just rearranged as the atoms change partners to form new compounds. • If there are 3 atoms of oxygen in the reactants, there MUST be 3 atoms of oxygen in the products. • Number of each atom in reactants = number of each atom in products. • The law of conservation of mass: • Mass of reactants = mass of products If you could collect and measure all of the exhaust from this car, you would find that mass of reactants (gas + O2) = mass of products (exhaust). (c) McGraw Hill Ryerson 2007

10. Writing & Balancing Equations • The simplest form of chemical equation is a word equation. • Potassium metal + oxygen gas  potassium oxide • A skeleton equation shows the formulas of the elements/compounds. • A skeleton equation shows which atoms are involved, but not how many molecules are involved. • K + O2 K2O

11. Writing & Balancing Equations • A balanced chemical equation shows all atoms and the coefficients tells us how many molecules (and atoms) there are. • Balancing ensures that the number of each atom is the same on both sides of the reaction arrow. • 4K + O2 2K2O K K O O K O K K O K K K

12. Counting Atoms to Balance Equations • Using the law of conservation of mass, we can count atoms to balance the number of atoms in chemical equations. • Word equation: methane + oxygen  water + carbon dioxide • Skeleton equation: CH4 + O2  H2O + CO2 • To balance the compounds, take note of how many atoms of each element occur on each side of the reaction arrow.

13. Counting Atoms to Balance Equations Skeleton equation: CH4 + O2  H2O + CO2 Carbon = 1 Carbon = 1 Hydrogen = 4 Hydrogen = 2 Oxygen = 2 Oxygen = 3 Balanced equation: CH4 + 2O2  2H2O + CO2Carbon = 1 Carbon = 1 Hydrogen = 4 Hydrogen = 4 Oxygen = 4 Oxygen = 4 The same number of atoms must be on each side. (c) McGraw Hill Ryerson 2007 See Page 207

14. Balancing Equations hydrogen + oxygen  water O2 H2 + H2O

15. Balancing Equations X hydrogen + oxygen  hydrogen peroxide H2 + O2 H2O2 YOU CANNOT CHANGE THE SUBSCRIPTS

16. 2 Balancing Equations hydrogen + oxygen  water H2 + O2 H2O

17. Balancing Equations hydrogen + oxygen  water H2 + O2 H2O 2

18. Balancing Equations hydrogen + oxygen  water 2 H2 + O2 H2O 2 (l) (g) (g)

19. Big Bag ‘O Balancing Tricks • Balance chemical equations by following these steps: • Trial and error will work but can be very inefficient. • USE A TABLE (write atoms underneath reactants and products) • If they look the same on both sides of the equation, treat polyatomic ions (such as SO42–) as a group & balance them as such. • If ‘OH’ and H2O are in the equation, write water as HOH. • Balance one compound at a time & rewrite the # of atoms in the chart as things change. • Only add coefficients; NEVER change subscripts!!! • If H and O appear in more than one place, attempt to balance them LAST. • Balance everything that isn’t ‘H’ or ‘O’ 1st. • Balance the ‘H’s 2nd to last. • Balance the ‘O’s last. • Always double-check after you think you are finished. • CHECK YOUR ANSWERS!!! See pages 209 - 211 (c) McGraw Hill Ryerson 2007

20. WATCH THIS LESSON ON BALANCING EQUATIONS Turn sound “on” http://www.youtube.com/watch?v=_B735turDoM A Beginner's Guide to Balancing Equations – Bozeman Science

21. Balance the following: • Fe + Br2 FeBr3 • Sn(NO2)4 + K3PO4  KNO2 + Sn3 (PO4)4 • C2H6 + O2  CO2 + H2O

22. ____Ba + ____H2O  ____Ba(OH)2 + ____H2 ____CO2 + ____H2O  ____H2CO3 ____Fe2O3 + ____C  ____Fe + ____CO ____Fe + ____H2O  ____H2 + ____Fe2O3