1. Chemical Reactions Quantitative Chem

2. Indicators of a Chemical Reaction

3. 1.Formation of a solid (called a precipitate)

4. Indicators of a Chemical Reaction 1.Formation of a solid (called a precipitate) 2.Production of gas

5. Indicators of a Chemical Reaction 1.Formation of a solid (called a precipitate) 2.Production of gas 3.Production (or absorption) of heat and light

6. Parts of a Chemical Equation 2Na (s) + Cl 2 (g)  2 NaCl (s)

7. Parts of a Chemical Equation 2Na (s) + Cl 2 (g)  2 NaCl (s) Reactants  Products

8. Parts of a Chemical Equation 2Na (s) + Cl 2 (g)  2 NaCl (s) Reactants  Products  Coefficients 

9. Parts of a Chemical Equation 2Na (s) + Cl 2 (g)  2 NaCl (s) Reactants  Products  Subscripts

10. Parts of a Chemical Equation 2Na (s) + Cl 2 (g)  2 NaCl (s)  ……...  …..…  …….....…  States of Matter

11. Parts of a Chemical Equation States of Matter: (s) = solid(l) = liquid (g) = gas(aq) = solution Arrows:  means “to yield” or “produce”

12. Why do we need to balance a chemical equation? Because matter is not created or destroyed in a chemical reaction! (The law of conservation of matter) The amount of each element remains the same.

13. Determine the number of atoms in each of the following compounds. NaCl:_____ Na _____ Cl K 3 N:_____ K_____ N Al 2 O 3 :_____ Al_____O

14. Coefficients! 3NaCl:_____ Na _____ Cl 4Al 2 O 3 :_____ Al_____O

15. Rules for Balancing (Coeff) 1.Start with the most complex element or compound. 2.Balance oxygen last 3.Balance hydrogen second to last 4.If stuck on oxygen, double everything except O 2, then balance. 5.Double-check your work.

16. 3. Classifying Reactions and Predicting Products

17. Examples of Chemical Reactions C 3 H 8 + O 2 → CO 2 + H 2 O NaOH → Na 2 O + H 2 O H 2 + O 2 → H 2 O Zn + 2 HCl → H 2 + ZnCl 2 K 2 CrO 4 + Pb(NO 3 ) 2 → 2 KNO 3 + PbCrO 4 H 2 CrO 4 + Pb(OH) 2 → 2 H 2 O + PbCrO 4

18. COMBUSTION What are some examples? What is it? (write the definition) Reaction 1: Candle Experiment 2C 24 H 50 + 73O 2  48CO 2 + 50H 2 O Reaction 2: CH 4 + 2O 2  CO 2 + 2H 2 O Reaction 3: C 3 H 8 + O 2 . What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) An exothermic reaction that takes place between a substance and oxygen. C X H Y + O 2  CO 2 + 2H 2 O (X and Y are integers) A carbon-based substance that reacts with oxygen. Produces carbon dioxide and water. C 3 H 8 + O 2  CO 2 + H 2 OEQ? C 3 H 8 + 5O 2  3CO 2 + 4H 2 O

19. SYNTHESIS What are some examples? What is it? (write the definition) Reaction 1: Magnesium + Oxygen Δ 2Mg + O 2  2MgO Reaction 2: Formation of Iron (II) Sulfide Δ 8Fe + S 8  8FeS Reaction 3: Formation of Water Δ H 2 + O 2 . What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) Two or more reactants combine to form a single product. A + B  AB Picture Energy (“Δ”) needs to be supplied. Only 1 compound is formed H 2 + O 2  H 2 OEQ? 2H 2 + O 2  2H 2 O

20. DECOMPOSITION What are some examples? What is it? (write the definition) Reaction 1: Carbonation in Soda H 2 CO 3  H 2 O + CO 2 Reaction 2: Decomposition of Water 2H 2 O  2H 2 + O 2 Reaction 3: Decomposition of Table Salt NaClO 3 . What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) A compound is broken down into two or more simpler substances. AB  A + B Picture 1. Metallic Hydroxide  2. Metallic Carbonate  3. Metallic Chlorate  4. Oxyacid  5. Binary Compound  Metallic Oxide + H 2 O Metallic Oxide + CO 2 Metallic Chloride + O 2 Nonmetallic Oxide + H 2 O 2 Elements NaClO 3  NaCl + O 2EQ? 2NaClO 3  2NaCl + 3O 2

21. SINGLE DISPLACEMENT What are some examples? What is it? (write the definition) Reaction 1: Copper & Silver Nitrate Cu + AgNO 3  2Ag + Cu(NO 3 ) 2 Reaction 2: 2NaBr + Cl 2  NaCl 2 + Br 2 Reaction 3: Zn + HCl  H 2 + ZnCl 2 What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) One element displaces another element from a compound. AX + Z  AZ + X A + BX  B + AX A cation replaces a cation An anion replaces an anion An element and compound Zn + HCl  H 2 + ZnCl 2EQ? Zn + 2HCl  H 2 + ZnCl 2

22. DOUBLE DISPLACEMENT What are some examples? What is it? (write the definition) Reaction 1: Potassium Iodide + Plumbous Chromate KI + PbCrO 4  K 2 CrO 4 + PbI 2 Reaction 2: AgNO 3 + CuCl 2  AgCl 2 + Cu(NO 3 ) Reaction 3: Fe 2 (SO 4 ) 3 + HCl  What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) Two aqueous compounds switch their cations (or anions). AC + BD  BC + AD Two soluble compounds react Forms two compounds where the cations (or anions) switch places. H 2 SO 4 + FeCl 3EQ?

23. NEUTRALIZATION What are some examples? What is it? (write the definition) Reaction 1: Hydrochloric Acid & Sodium Hydroxide HCl + NaOH  NaCl + H 2 O Reaction 2: H 2 SO 4 + NaOH  Na 2 SO 4 + H 2 O Reaction 3: H 2 CO 3 + Ca(OH) 2  What are the characteristics of the reactants that undergo this type of reaction? What are the products of this type of reaction? (on pg 12) An acid reacts with a base to form salt and water. HA + BOH  BA + H 2 O An acid reacts with a hydroxide compound An ionic compound (“salt”) and water CaCO 3 + H 2 OEQ?