1. Chemical Equations What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation?

2. Chemical Equations A chemical equation is written as an expression similar to a mathematic equation that can be compared to a recipe that a chemist follows in order to produce desired results.

3. Chemical Equations  All chemical equations have reactants and products.  We express a chemical equation as follows: Reactants  Products The arrow is equivalent to an “=“ math. When we describe the equation we use the word “yields” or “produces” instead of equals

4. Conservation of matter  The law of conservation of matter tells us that matter can neither be created nor destroyed. It is transformed from one form to another.  We follow the conservation of matter law when we balance equations.

5. Balancing a Chemical Equation A chemical equation is balanced when the ions or atoms found on the reactant side of the equation equals that found on the product side. The arrow can be considered the balance point.

6. Coefficients We use coefficients in front of elements or compounds on either side of the reaction to balance the equation. (The coefficients go in front of the chemical!) We cannot change subscripts because it would create new materials that are not part of reaction process.

7. Balance this equation! Na + Cl 2 NaCl Na-1Na-1 Cl-2Cl-1 **note that the number of sodiums balance but the chlorine does not. We will have to use coefficients in order to balance this equation.

8. Inserting subscripts Na + Cl 2 2 NaCl Na-1Na-1 2 Cl-2Cl-1 2 ** Now the chlorine balances but the sodium does not! So we go back and balance the sodium.

9. Finally balanced! 2Na + Cl 2 2 NaCl Na-1 2Na-1 2 Cl-2Cl-1 2 **Since the number of each element on the reactant side and the product side of the equation are equal, the equation is balanced.

10. Balancing Equation Practice 1. CuCl 3 + Li 2 S  Cu 2 S 3 + LiCl 2. NiNO 3 + KCl  NiCl+ KNO 3 3. FeCl 3 + Na 2 O  Fe 2 O 3 + NaCl

11. Answers:  1. 2CuCl 3 + 3Li 2 S  Cu 2 S 3 + 6LiCl  2. NiNO 3 + KCl  NiCl+ KNO 3 (already balanced)  3. 2FeCl 3 + 3Na 2 O  Fe 2 O 3 + 6NaCl

12. Identifying Reaction Types Reactions are classified by their products. There are several different types of chemical reactions. The 5 basic types of chemical reactions we will study are: synthesis or combination reactions, decomposition reactions, single replacement reactions, double replacement reactions, and combustion reactions.

13. Synthesis or Combination reactions Synthesis (meaning to make) or combination reactions are typified by their single product. If you have a reaction in which at least 2 elements or compounds are reacted and produce a single product, the reaction is a synthesis reaction.

14. Synthesis Reactions A + B  AB Note: Single Product! This is your clue that this is a synthesis or combination reaction.

15. Decomposition Reactions Decomposition reactions are really just the opposite of a synthesis reaction. Remember, if you can make a substance, you should be able to break it back apart into its components. A good way to remember decomposition reactions to to remember what happens when something decomposes. It falls apart!

16. Decomposition Reactions AB  A + B Note: Single Reactant! The single reactant is your clue that this is a decomposition reaction.

17. Single Replacement Reactions Single replacement reactions occur when one chemical takes the place of another in a reaction. In the typical single replacement reaction, an element trades places with one of the ions in a compound.

18. Single Replacement Reactions A + CD  AD + C Note: Element A replaces ion C in the reaction. The clue in this reaction is: Element+Compound  Element + Compound

19. Double Replacement Reactions Double replacement reactions are identified by two ions trading places and forming new compounds.

20. Double Replacement Reactions AB + CD  AD + CB Note: Notice that one ion from compound AB replaces one ion from compound CD. Clue: Compound+Compound  Compound+Compound

21. Combustion Reactions Combustion reactions are the ones that burn (or explode!). There are two types of combustion reactions— complete or incomplete reactions. These reactions are identified by their products. They either produce carbon monoxide and water or carbon dioxide and water.

22. Complete Combustion Reactions These reactions burn “efficiently” which means they produce carbon dioxide and water. These reactions typically burn cleanly and leave very little residue behind.

23. Complete Combustion Reactions CH 4 + O 2  CO 2 + H 2 O They may also be written: CH 4  CO 2 + H 2 O (O 2 is usually written above the arrow.) Clue: CO 2 (carbon dioxide) in the product along with water

24. Incomplete Combustion Reactions Incomplete combustion reactions occur when something does not burn efficiently. This can cause a lot of harm if the gases produced cannot escape. Carbon monoxide,an odorless and colorless gas, is dangerous. People poisoned by this gas usually become sleepy and can die due to exposure.

25. Incomplete Combustion Reactions CH 4 + O 2  CO + H 2 O These reactions may also be written by: CH 4  CO + H 2 O (the O 2 is usually written over the arrow.) Clue: CO (Carbon monoxide as a product.)

26. Completing Reactions Completing reactions requires knowledge of the different reaction types (sometimes called mechanisms). You must first identify the reaction type by the reactants. The only type of reaction that cannot be predicted this way is the combustion reaction since the products are very similar.

27. First Step:  Identify reaction type Example: Al + O 2  Clue: 2 elements – Synthesis or combination reaction

28. Second Step:  Write the net ionic equation for the reactants Al + O 2  Al 3+ + O 2- 

29. Step 3  Using clues, complete reaction taking care to write each formula correctly by checking charges and “criss-crossing” if necessary. Al + O 2  Al 3+ O 2- Al + O 2  Al 2 O 3

30. Completion Practice 1. Na + K 2 SO 4  2. PbSO 4 + LiCl  3. Ca + H 2 O 