1. 1.To learn about some of the factors that cause reactions to occur 2.To learn to identify the solid that forms in a precipitation reaction 3.To learn to write molecular, complete ionic, and net ionic equations 8.1 Objectives Chapter 8

2. A. Predicting Whether a Reaction Will Occur Four driving forces favor chemical change. Formation of a solid Formation of a solid Formation of water Formation of water Transfer of electrons Transfer of electrons Formation of a gas Formation of a gas

3. B. Reactions in Which a Solid Forms A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate Solid = precipitate http://www.youtube.com/watch?v=pFovlKpPCbI

4. The ions separate and move around independently. B. Reactions in Which a Solid Forms What Happens When an Ionic Compound Dissolves in Water?

5. B. Reactions in Which a Solid Forms What Happens When an Ionic Compound Dissolves in Water? K 2 CrO 4 (aq) + Ba(NO 3 ) 2 (aq)  Products NaCl(s) + H 2 O(l)  Na + + Cl - + H 2 O http://www.youtube.com/watch?v=EBfGcTAJF4o

6. Determine the possible products from the ions in the reactants. In our example K 2 CrO 4 (aq) + Ba(NO 3 ) 2 (aq)  Products The possible ion combinations are: B. Reactions in Which a Solid Forms How to Decide What Products Form

7. B. Reactions in Which a Solid Forms How to Decide What Products Form Decide which is most likely to be the yellow solid formed in the reaction. K 2 CrO 4 (aq) reactant Ba(NO 3 ) 2 (aq) reactant The possible combinations are KNO 3 and BaCrO 4. –KNO 3 white solid –BaCrO 4 yellow solid

8. Reading! Read in 8.1, the section title Using Solubility Rules (pg 244-245) Study the solubility rules, Table 8.1 and Figure 8.3 (pg 245) Study the solubility rules, Table 8.1 and Figure 8.3 (pg 245) Also, read and examine Example 8.1 (pg 246-247)

9. B. Reactions in Which a Solid Forms Using Solubility Rules: Table

10. B. Reactions in Which a Solid Forms Predicting Precipitates Using Solubility Rules –Soluble solid –Insoluble solid –Slightly soluble solid

11. B. Reactions in Which a Solid Forms Review! How to predict precipitates when solutions of 2 Ionic Compounds are mixed: Step 1: Write the reactants as they actually exist before any reaction occurs. Remember that when a salt dissolves, its ions separate. Step 2: Consider the various solids that could form. To do this, simply exchange the anions of the added salts. Step 3: Use the solubility rules (Table 8.1 and your chart) to decide whether a solid forms and, if so, to predict the identity of the solid.

12. C. Describing Reactions in Aqueous Solutions Three types of equations: Molecular (formula) equation  Molecular (formula) equation  complete formulas of all reactants and products complete formulas of all reactants and products Complete ionic equation  Complete ionic equation  all strong electrolytes are shown as ions all strong electrolytes are shown as ions Net ionic equation  Net ionic equation  only those components of the solution that undergo a change only those components of the solution that undergo a change Spectator ion (those that remain unchanged)  not shown in the net ionic equation not shown in the net ionic equation

13. Example NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq) Molecular equation: NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq) NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq) Complete Ionic Equation: Na + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq) → AgCl(s) + Na + (aq) + NO 3 - (aq) Na + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq) → AgCl(s) + Na + (aq) + NO 3 - (aq) Net Ionic Equation: Cl - (aq) + Ag + (aq) → AgCl(s) Cl - (aq) + Ag + (aq) → AgCl(s)

14. 1.To learn about reactions between strong acids and strong bases 2.To learn about the reaction between a metal and a nonmetal 3.To understand how electron transfer produces a chemical reaction 8.2 Objectives

15. A. Reactions That Form Water: Acids and Bases Arrhenius Acids and Bases A strong acid is one in which virtually every molecule dissociates (ionizes) in water to an H + ion and an anion.

16. A strong base is a metal hydroxide that is completely soluble in water, giving separate OH  ions and cations. A. Reactions That Form Water: Acids and Bases Arrhenius Acids and Bases –Most common  NaOH, KOH

17. A. Reactions That Form Water: Acids and Bases Arrhenius Acids and Bases The products of the reaction of a strong acid and a strong base are water and a salt. –Salt  Ionic compound Net ionic equation –H + (aq) + OH − (aq)  H 2 O(l) Reaction of H + and OH − is called an acid-base reaction. –H +  acidic ion –OH −  basic ion

18. B. Reactions of Metals with Nonmetals (Oxidation-Reduction) Reactions between metals and nonmetals involve a transfer of electrons from the metal to the nonmetal. –oxidation – reduction reaction

19. 1.To learn various classification schemes for reactions 8.3 Objectives

20. A. Ways to Classify Reactions Driving forces for a reaction: Formation of a solid Formation of a solid AB + CD  AD + CB Precipitation reaction Double displacement reaction Formation of water Formation of water H + (aq) + OH − (aq)  H 2 O(l) Acid-base reaction

21. A. Ways to Classify Reactions Driving forces for a reaction: –Transfer of electrons

22. A. Ways to Classify Reactions Driving forces for a reaction: –Transfer of electrons –Formation of a Gas A + BC  B + AC Single replacement reaction

23. Involve oxygen and produce energy so rapidly that a flame results CH 4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O(g) CH 4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O(g) Special class of oxidation-reduction reactions Special class of oxidation-reduction reactions B. Other Ways to Classify Reactions Combustion Reactions

24. A synthesis reaction is one in which a compound forms from simpler materials. C(s) + O 2 (g)  CO 2 (g) C(s) + O 2 (g)  CO 2 (g) Special class of oxidation-reduction reactions Special class of oxidation-reduction reactions B. Other Ways to Classify Reactions Synthesis (Combination) Reactions +

25. A decomposition reaction occurs when a compound is broken down into simpler substances. 2H 2 O(l)  2H 2 (g) + O 2 (g) 2H 2 O(l)  2H 2 (g) + O 2 (g) B. Other Ways to Classify Reactions Decomposition Reactions +

26. B. Other Ways to Classify Reactions Summary http://www.youtube.com/watch?v=tE4668aarck&safety_mode=true&persist_safety_mode=1