1. L AUNCHING A CTIVITY What will happen? Place 20 ml of Na 2 Si 3 O 7 into a dixie cup. Place 10 ml of C 2 H 5 OH into a test tube. Examine and predict what may happen! Add Na 2 Si 3 O 7 + C 2 H 5 OH and 2 drops of red food coloring in the cup. Stir. Did you get what you thought?

2. UEQ How can a good balanced equation help you understand the interaction of compound in a chemical reaction?

3. C HEMICAL R EACTIONS An expression of the behavior of chemical compounds 1. Expressed in a chemical equation: Reactant(s)  Product(s) (compounds reacting) To Yield(reconstituted compounds)

4. P ARTS OF A C HEMICAL E QUATION 2 Na (s) + 2H 2 O (l)  2NaOH (aq) + H 2(g) To Yield Subscripts : # of atoms in compound Physical State: (s), (l), (g), (aq) Coefficient: the # of cpd (moles) present. Can be factions, ONLY # that is changed Reversible reaction:  Catalyst: speeds up a reaction without being a part of the product such as heat, Δ, or compound (FeO 2 )

5. R EVIEW Q UESTIONS 1. What does the subscript tell you? 2. A species in a reaction that speeds up the reaction but does not appear in the final product is called a(n) ________? 3. The stuff that you get as a result of chemical interaction is called the ____? 4. What does (aq) mean? 5. What is used to indicate that a precipitate has formed?

6. LEQ What defines a good balanced equation?

7. B ALANCING C HEMICAL E QUATIONS ONLY the coefficient can be changed. 1. Write the compounds (criss-cross) or prefix for molecules. 2. Define the type of reaction (activity series and solubility rules) 3. Take count of the type and number of elements in the compounds. 4. Change of the coefficient ONLY to ensure that the same # and type of each are present on both sides of the arrow.

8. W ORD P ROBLEM An aqueous solution of sodium chloride and hydrogen sulfide gas is produced when aqueous sodium sulfide reacts with an excess of hydrochloric acid. Na 2 S (aq) + HCl (aq)  NaCl (aq) + H 2 S (g) Na 2 S (aq) + 2HCl (aq)  2NaCl (aq) + H 2 S (g)

9. TPS: W ORD P ROBLEM S AMPLER Solid lead is dissolved in aqueous sulfuric acid to precipitate lead (III) sulfate and hydrogen gas is evolved. Pb (s) + H 2 SO 4(aq)  Pb 2 (SO 4 ) 3(s) + H 2(g) 2Pb (s) + 3H 2 SO 4(aq)  Pb 2 (SO 4 ) 3 (s) + 3H 2(g) TLS: ‘Balance Act’ and ‘Balancing Equations’.

10. 1. When lithium hydroxide pellets are added to a solution of sulfuric acid, lithium sulfate and water are produced. 2. If a copper coil is placed into a solution of silver nitrate, silver crystals form on the surface of the copper and a highly soluble copper (I) nitrate is generated. 3. When crystilline C 6 H 12 O 6 is burned in oxygen, carbon dioxide and water are produced.

11. LEQ How do you identify the different types of reactions?

12. T YPE OF R EACTIONS 1. Synthesis Reaction 2. Decomposition Reaction 3. Single Replacement 4. Double Replacement 5. Combustion Reaction.

13. S YNTHESIS R EACTION The reaction of two or more reactants to produce a single product. a. Form: A 2 + 2CB  2ACB Sulfur dioxide and water react to produce sulfurous acid SO 2 + H 2 O  H 2 SO 3

14. S YNTHESIS R EACTION 1. Metal react w/ O 2 to form metal oxide 2Fe + O 2  2FeO (s) (rust) 2. Metal oxides react w/ O 2 to form metal oxides? 4 FeO + O 2  2 Fe 2 O 3 3. Metal oxides react with H 2 O to form bases. CaO + H 2 O  Ca(OH) 2

15. S YNTHESIS R EACTIONS 4. Non-metals react with O 2 to form non-metal oxides. S 8 + 8 O 2  8 SO 2 5. Non-metal oxides react with H 2 O to form acids. SO 2 + H 2 O  H 2 SO 3 NOTE: Oxidation number does NOT change, this defines the product!

16. S YNTHESIS R EACTION 6. Metal oxide + non-metal oxide will produce a salt. CaO + SO 3  CaSO 4 NOTE: the oxidation number will define the product! 7. Metal and non-metal react w/ H 2 to form metal and non-metal hydrides. 2Li + H 2  2LiH metal hydride H 2 + Cl 2  2HCl non-metal hydrides (most acids)

17. S YNTHESIS S AMPLERS 1. BaO + H 2 O  2. MgO + SO 2  3. Cr + O 2  4. _____ + H 2 O  HNO 2 5. K + H 2  6. CrO + O 2  7. H 2 + Br 2 

18. D ECOMPOSITION R EACTION A reaction where one or more reactants breakdown into several simpler forms. a. Form: AB 2  A + 2B b. Requires energy to breakdown! Ammonia breaks down to nitrogen gas and hydrogen gas 2NH 3  N 2 + 3H 2 NOTE: NH 3 is a nonmetal hydride

19. S INGLE R EPLACEMENT A reaction where the metals (or non-metal) trade places. a. Form: AB + C  CB + A b. Only like charged species trade places!!!!! c. Depends directly of the activity series for metals and non-metals.

20. LEQ What determines an elements placement on the activity series?

21. A CTIVITY S ERIES Back of periodic table: **The more active the metal (or non-metal), the more likely it is to replace the less active metal (or non-metal). **All metals will replace Gold according to the list. **Lithium will replace all metals. **Fluorine is the most active non-metal. NOTE: non-metal series are Group 7A

22. TPS: S AMPLE : S INGLE R EPLACEMENT Sodium plus copper (II) chloride yields sodium chloride and copper metal. 2Na + CuCl 2  Magnesium metal reacts with potassium hydroxide to yield Mg + KOH 

23. S INGLE R EPLACEMENT S AMPLER 1. Fe + H 2 O  2. Cd + HNO 3  3. Cu + MgO  4. ____ + ____  KClO 3 + Pb 5. Na 2 SO 4 + Hg  6. Na 2 CrO 4 + Ba  7. ____ + ____  Sb + ZnCl 2

24. LEQ How are solubility rules use to describe how a double replacement reaction may occur?

25. D OUBLE R EPLACEMENT a reaction where the metals or non-metals trade positions. (like replaces like). Form: AB + CD  AD + CB A precipitate can be formed as one of the produces often. (Metathesis Reaction) Neutralization reaction: Acid/Base NOTE: Always refer to the solubility rules.

26. TPS: S AMPLE : D OUBLE R EPLACEMENT Silver (I) nitrate plus sodium chloride to yield ? **Are the reactants soluble? **Like ions trade places to form a new product. **Balance the charge then balance the equation** AgNO 3 + NaCl  AgNO 3 + NaCl  NaNO 3 + AgCl

27. TPS: S OLUBILITY Ionic compounds ability to dissolve in water. Solubility Rule: Note the Periodic Reference Page Ba(NO 3 ) 2 Pb 2 (SO 4 ) 3 C2H4C2H4 AgCl 2 CaCO 3

28. D OUBLE R EPLACEMENT S AMPLERS 1. Fe(NO 3 ) 2 + Na 2 CrO 4  2. (NH 4 ) 2 S + Na 2 SO 4  3. HNO 3 + KOH  4. Hg 2 Cl 2 + NaOH  5. Na 3 PO 4 + BaSO 4 

29. C OMBUSTION R EACTION The burning of hydrocarbons in the presence of oxygen and energy. Form: Hydrocarbon gas + oxygen  carbon dioxide and water. (a complete burn). CH 4 + O 2  CO 2 + H 2 O (a complete burn) Or CH 4 + O 2  CO + H 2 O (a dirty burn)

30. LEQ How do you write the net ionic equation?

31. N ET I ONIC E QUATIONS Spectator Ions: Occurs when reactant compounds dissolve into solution and ions remain in solution. Pay attention to the physical state. (s) (l) and (g) indicates that it has NOT ionized (broken down) Pay attention to the solubility rules on the periodic table. The ions that are on both sides of the equation are called spectator ions and cancel. The ions that remain form a net ionic equation.

32. N ET I ONIC E QUATIONS -gas production is a non-soluble product -water is a non-soluble product -solids indicate a non-soluble product.

33. S AMPLE : N ET I ONIC E QUATION Pb(ClO 4 ) 2 (aq) + NaI (aq)  PbI 2(s) + NaClO 4(aq) TPS: 1. Aqueous solutions of lead (II) nitrate and ammonium chloride are mixed  2. Aqueous solution of aluminum chloride and sodium carbonate combine  3. Sulfuric acid reacts with sodium hydroxide  4. Sodium sulfide reacts with hydrochloric acid 

34. T HINKING Q UESTIONS 1. If water is the product in the net ionic equation in an acid/base reaction, what does this tell you about the reaction? 2. What type of solution would you have if all the reactants and products were soluble? 3. Where would a net ionic reaction be useful? Hint spectator ions.

35. D OUBLE R EPALACEMENT P RE -L AB Cu(NO 3 ) 2 BaCl 2 Na 2 CrO 4 Pb(NO 3 ) 2 Al 2 (SO 4 ) 3

36. C HEMICAL E QUATION 2Na (s) + 2H 2 O (l)  2NaOH (aq) + H 2(g) reactants To Yield Products (s) : solids (l) : liquid (aq): aqueous (g): gas Coefficient: Big number in front. # of compounds present (# of moles). ONLY number that can change. Subscript: # of atoms present in the compound Reversible; Catalyst

37. C HEMICAL R EACTION An expression of the behavior of chemical compounds Expressed in a chemical equation: To yield Reactant(s)  Product(s) (stuff reacting)(reforming of stuff) ****Energy is required to break or form****

38. B ALANCING C HEMICAL E QUATIONS Same number and type of each element on both sides of the . *Same by changing the coefficient ONLY. *Coefficient in front of cpd ONLY. *Once the charges of a cpd are balanced, NEVER change a subscript! Review: Writing formula units and molecular formula Criss-cross to balance charge