1. Balancing Chemical Equations Reactants: Zn + I 2 Product: Zn I 2

2. Introduction Chemical reactions occur when bonds between the outermost parts of atoms are formed or broken Chemical reactions involve changes in matter, the making of new materials with new properties, and energy changes. Symbols represent elements, formulas describe compounds, chemical equations describe a chemical reaction

3. Indications of a Chemical Reaction Certain easily observed changes usually indicate that a chemical reaction has occurred. 1.Evolution of energy as heat and light. 2.Production of a gas.

4. Indications of a Chemical Reaction 3. Formation of a precipitate.  A solid that is produced as a result of a chemical reaction in solution and that separates from the solution. 4. Color Change.

5. Characteristics of a Chemical Reaction The following requirements will aid you in writing and reading chemical equations correctly. 1.The equation must represent known facts. 2.The equation must contain the correct formulas for the reactants and products.

6. Characteristics of a Chemical Reaction 3. The law of conservation of mass must be satisfied. a relation stating that in a chemical reaction, the mass of the products equals the mass of the reactants.

7. Parts of a Reaction Equation reactants productsChemical equations show the conversion of reactants (the molecules shown on the left of the arrow) into products (the molecules shown on the right of the arrow). A + sign separates molecules on the same side The arrow is read as “yields” Example C + O 2  CO 2 This reads “carbon plus oxygen react to yield carbon dioxide”

8. The charcoal used in a grill is basically carbon. The carbon reacts with oxygen to yield carbon dioxide. The chemical equation for this reaction, C + O 2  CO 2, contains the same information as the English sentence but has quantitative meaning as well.

9. Chemical Equations Because of the principle of the conservation of matter, an equation must be balanced. It must have the same number of atoms of the same kind on both sides. Lavoisier, 1788

10. Symbols Used in Equations Solid (s) Liquid (l) Gas (g) Aqueous solution (aq) Catalyst Pd Escaping gas (  ) Change of temperature (  )

11. Balancing Equations notWhen balancing a chemical equation you may add coefficients in front of the compounds to balance the reaction, but you may not change the subscripts. Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or sharing for covalent)

12. Steps to Balancing Equations There are four basic steps to balancing a chemical equation. 1.Write the correct formula for the reactants and the products if not already done. DO NOT TRY TO BALANCE IT YET! You must write the correct formulas first. And most importantly, once you write them correctly DO NOT CHANGE THE FORMULAS! 2.Count the number of atoms for each element on each side. Compare the number of the atoms of the same element on the each side.

13. Steps to Balancing Equations 3.Place coefficients in front of formulas so that the left side has the same number of atoms as the right side for EACH element in order to balance the equation. 4.Check your answers to see if: The numbers of atoms on both sides of the equation are now balanced. The coefficients are in the lowest possible whole number ratios. (reduced)

14. Some Suggestions to Help You Helpful Hints for balancing equations: Take one element at a time, working left to right except for H and O. Save H for next to last, and O until last. IF everything balances except for O, and there is no way to balance O with a whole number, double all the coefficients and try again. (Because O is diatomic as an element) (Shortcut) Polyatomic ions that appear on both sides of the equation should be balanced as if they are a single unit.

16. ___ Al(s) + ___ Br 2 (l) ---> ___ Al 2 Br 6 (s) 2 3 Balancing Equations

17. ____C 3 H 8 (g) + _____ O 2 (g) ----> _____CO 2 (g) + _____ H 2 O(g) ____B 4 H 10 (g) + _____ O 2 (g) ----> ___ B 2 O 3 (g) + _____ H 2 O(g) Balancing Equations 5 3 4 2 11 410

18. Sodium phosphate + iron (III) oxide  sodium oxide + iron (III) phosphate ___Na 3 PO 4 +___Fe 2 O 3 ---->___Na 2 O +___FePO 4 Balancing Equations