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Section 4 Chemical Reactions

Section 4 Chemical Reactions. Ions in Aqueous Solution Ionic Theory of Solutions. Many ionic compounds dissociate into independent ions when dissolved in water. These compounds that “freely” dissociate into independent ions in aqueous solution are called electrolytes.

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Section 4 Chemical Reactions

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  1. Section 4 Chemical Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  2. Ions in Aqueous SolutionIonic Theory of Solutions • Many ionic compounds dissociate into independent ions when dissolved in water • These compounds that “freely” dissociate into independent ions in aqueous solution are called electrolytes. • Their aqueous solutions are capable of conducting an electric current. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  3. Ions in Aqueous SolutionIonic Theory of Solutions • Not all electrolytes are ionic compounds. Some molecular compounds dissociate into ions. • The resulting solution is electrically conducting, and so we say that the molecular substance is an electrolyte. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  4. Ions in Aqueous SolutionIonic Theory of Solutions • Most molecular compounds (except acids) dissolve but do not dissociate into ions. • These compounds are referred to as nonelectrolytes. They dissolve in water to give a nonconducting solution. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  5. Ions in Aqueous SolutionIonic Theory of Solutions • Strong and weak electrolytes. • A strong electrolyte is an electrolyte that exists in solution almost entirely as ions. • Most ionic solids that dissolve in water do so almost completely as ions, so they are strong electrolytes. • strong electrolytes – strong acids, strong bases, soluble salts Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  6. Ions in Aqueous SolutionIonic Theory of Solutions • A weak electrolyteis an electrolyte that dissolves in water to give a relatively small percentage of ions. • Most soluble molecular compounds are either nonelectrolytes or weak electrolytes. • Weak electrolytes - weak acids, weak bases, insoluble salts • Solutions of weak electrolytes contain only a small percentage of ions. We denote this situation by writing the equation with a double arrow. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  7. Solubility Rules for Ionic Compounds (Dissociates 100%) 1.) All compounds containing alkali metal cations and the ammonium ion are soluble. 2.) All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble. 3.) All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg22+. 4.) All sulfates are soluble except those containing Hg22+, Pb2+, Ba2+, Sr2+, or Ca2+. Ag2SO4 is slightly soluble. 5.) All hydroxides are insoluble except compounds of the alkali metals and Ca2+, Sr2+, and Ba2+ are slightly soluble. 6.) All other compounds containing PO43-, S2-, CO32-, CrO42-, SO32- and most other anions are insoluble except those that also contain alkali metals or NH4+. Generally, compound dissolves > 0.10 M - soluble (aq) < 0.01 M - insoluble (s) in between - slightly soluble (this class we will assume slightly soluble as soluble) HW 26 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  8. Strong Acids (Ionizes 100%) HCl, HBr, HI, HClO4, HNO3, H2SO4 Strong Bases (Dissociates 100%) NaOH, KOH, LiOH, Ba(OH)2, Ca(OH)2, Sr(OH)2 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  9. Ions in Aqueous SolutionMolecular and Ionic Equations • A molecular/formula unit equation is one in which the reactants and products are written as if they were molecules/formula units, even though they may actually exist in solution as ions. Calcium hydroxide + sodium carbonate F.U. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  10. Ions in Aqueous SolutionMolecular and Ionic Equations • An total ionic equation, however, represents strong electrolytes as separate independent ions. This is a more accurate representation of the way electrolytes behave in solution. • A complete ionic equation is a chemical equation in which strong electrolytes (such as soluble ionic compounds, strong acids/bases) are written as separate ions in solution . (note: g, l, insoluble salts (s), weak acid/bases do not break up into ions) F.U. Ca(OH)2 (aq) + Na2CO3 (aq)  CaCO3 (s) + 2 NaOH (aq) Total ionic Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  11. A net ionic equation is a chemical equation from which the spectator ions have been removed. • A spectator ion is an ion in an ionicequationthat does not take part in the reaction. • Net ionic equations. F.U. Ca(OH)2 (aq) + Na2CO3 (aq)  CaCO3 (s) + 2 NaOH (aq) Total Ionic Ca2+(aq) + 2OH-(aq) + 2Na+(aq) + CO32- (aq)  CaCO3(s) + 2Na+(aq) + 2OH-(aq) Net Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  12. Ions in Aqueous SolutionMolecular and Ionic Equations • Complete and net ionic equations • Let’s try an example. First, we start with a molecular equation. F.U. HNO3(aq) + Mg(OH)2(s) Total ionic Net Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  13. Ions in Aqueous SolutionMolecular and Ionic Equations F.U. HCN (aq) + NaOH (aq) Total ionic Net Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  14. Types of Chemical Reactions • Most of the reactions we will study fall into one of the following categories • Precipitation Reactions • Acid-Base Reactions • Oxidation-Reduction Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  15. Types of Chemical ReactionsPrecipitation Reactions • A precipitation reaction occurs in aqueous solution because one product is insoluble. • A precipitate is an insoluble solid compound formed during a chemical reaction in solution. • For example, the reaction of sodium chloride with silver nitrate forms AgCl(s), an insoluble precipitate. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  16. Types of Chemical ReactionsPrecipitation Reactions • Suppose you mix together solutions of nickel(II) chloride, NiCl2, and sodium phosphate, Na3PO4. • Precipitation Reactions. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  17. F.U. NaCl (aq) + Fe(NO3)2(aq) HW 27 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  18. Types of Chemical Reactions • Acid-Base Reactions • Acids and bases are some of the most important electrolytes. • They can cause color changes in certain dyes called acid-base indicators. • Household acids and bases. • Red cabbage juice asan acid-base indicator. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  19. Types of Chemical ReactionsAcid-Base Reactions • The Arrhenius Concept • The Arrhenius concept defines acids as substances that produce hydrogen ions, H+, when dissolved in water. • An example is nitric acid, HNO3, a molecular substance that dissolves in water to give H+ and NO3-. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  20. Types of Chemical ReactionsAcid-Base Reactions • The Arrhenius Concept • The Arrhenius concept defines bases as substances that produce hydroxide ions, OH-, when dissolved in water. • An example is sodium hydroxide, NaOH, an ionic substance that dissolves in water to give sodium ions and hydroxide ions. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  21. Types of Chemical ReactionsAcid-Base Reactions • By Arrhenius concept is ammonia an acid or base? Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  22. Types of Chemical ReactionsAcid-Base Reactions • The Brønsted-Lowry Concept • The Brønsted-Lowry concept of acids and bases involves the transfer of a proton (H+) from the acid to the base. • In this view, acid-base reactions are proton-transfer reactions. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  23. Types of Chemical ReactionsAcid-Base Reactions • The Brønsted-Lowry Concept • The Brønsted-Lowry concept defines an acid as the species (molecule or ion) that donates a proton (H+) to another species in a proton-transfer reaction. • Abase is defined as the species (molecule or ion) that accepts the proton (H+) in a proton-transfer reaction. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  24. H+ Types of Chemical ReactionsAcid-Base Reactions • The Brønsted-Lowry Concept the H2O molecule is the acid because it donates a proton. The NH3 molecule is a base, because it accepts a proton. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  25. H+ where HNO3 is an acid (proton donor) and H2O is a base (proton acceptor). Conjugate acid/base pairs – differ by a proton Types of Chemical ReactionsAcid-Base Reactions • The Brønsted-Lowry Concept Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  26. Types of Chemical ReactionsAcid-Base Reactions • In summary, • The Arrhenius concept • acid: proton (H+) producer • base: hydroxide ion (OH-) producer • The Brønsted-Lowry concept • acid: proton (H+) donor • base: proton (H+) acceptor HW 28 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  27. Types of Chemical ReactionsAcid-Base Reactions • Strong and Weak Acids and Bases • A strong acid is an acid that ionizes completely in water; it is a strong electrolyte. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  28. Types of Chemical ReactionsAcid-Base Reactions • Strong and Weak Acids and Bases • A weak acid is an acid that only partially ionizes in water; it is a weak electrolyte. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  29. Types of Chemical ReactionsAcid-Base Reactions • Strong and Weak Acids and Bases • A strong base is a base that is present entirely as ions, one of which is OH-; it is a strong electrolyte. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  30. Types of Chemical ReactionsAcid-Base Reactions • Strong and Weak Acids and Bases • A weak base is a base that is only partially ionized in water; it is a weak electrolyte. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  31. What are weak bases? NH3, NH2-, NH-, some anions. • Which anions? Salts may be acidic/basic/neutral and are composed of cations (positive ions) and anions (negative ions) cation anion Acidic or neutral basic or neutral Cations of strong bases Anions of monoprotic strong are neutral; otherwise acids are neutral; otherwise cation contributes acidity anion contributes basicity i.e. NaCN NaCl AlCl3 K2CO3 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  32. acid base salt Types of Chemical ReactionsAcid-Base Reactions • One of the chemical properties of acids and bases is that they neutralize one another. • A neutralization reaction is a reaction of an acid and a base that results in an ionic compound (salt) and water. A + B  salt + H2O • The ionic compound that is the product of a neutralization reaction is called a salt (acidic, basic, or neutral). • SA + WB  • SA + SB  • WA + SB  • Neutralization Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  33. See better in net eq. H+ • The net ionic equation for each acid-base neutralization reaction involves a transfer of a proton. • Neutralization Reactions Total: Net: Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  34. Types of Chemical ReactionsAcid-Base Reactions • Consider the reaction of the strong acid , HCl(aq) and a strong base, KOH(aq). • Neutralization Reactions Total: Net: HW 29 &30 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  35. Types of Chemical ReactionsAcid-Base Reactions • Carbonates react with acids to form CO2, carbon dioxide gas. • Acid-Base Reactions with Gas Formation • Sulfites react with acids to form SO2, sulfur dioxide gas. • Sulfides react with acids to form H2S, hydrogen sulfide gas. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  36. Types of Chemical ReactionsAcid-Base Reactions • Other Acid-Base reactions Nonmetal oxides (or acid oxides or acid anhydrides) react with water to form acids SO2 + H2O  H2SO3 Metal oxides (or basic oxides or basic anhydrides) react with water to form bases Na2O + H2O  2NaOH Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  37. Types of Chemical Reactions • Oxidation-reduction reactions involve the transfer of electrons from one species to another. • Oxidation is defined as the loss of electrons. • Reduction is defined as the gain of electrons. • Oxidation and reduction always occur simultaneously. • Oxidation-Reduction Reactions (Redox rxn) Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  38. Redox reactions – transfer of e- • reduction – oxidation reactions • Reduction – gain of e- / gain of H / lost of O • Fe3++ 1e- Fe2+ (lower ox state) • note: must balance atoms and charges Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  39. Oxidation - loss of e- / loss of H / gain of O Fe2+ Fe3++ 1e- (higher ox state) H2O + BrO3-  BrO4- + 2H++ 2e- (Br oxidized: charge 5+  7+) 2H++ 2e-  H2 (H reduced: charge 1+  0) Oxidizing agent is species that undergoes reduction. Reducing agent is species that undergoes oxidation. Note: need both for reaction to happen; can’t have something being reduced unless something else is being oxidized. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  40. Types of Chemical Reactions • Oxidation-Reduction Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  41. Types of Chemical Reactions • Oxidation-Reduction Reactions Loss of 2 e-1oxidation Gain of 2 e-1reduction Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  42. Types of Chemical ReactionsOxidation-Reduction Reactions • Oxidation Numbers • The concept of oxidation numbers is a simple way of keeping track of electrons in a reaction. • The oxidation number (or oxidation state) of an atom in a substance is the actual charge of the atom if it exists as a monatomic ion. • Alternatively, it is hypothetical charge assigned to the atom in the substance by simple rules. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  43. Types of Chemical ReactionsOxidation-Reduction Reactions • Oxidation Number Rules Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  44. Oxidation-Reduction Reactions • Oxidation Number Rules HW 31 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  45. Types of Chemical ReactionsOxidation-Reduction Reactions • Some Common Oxidation-Reduction Reactions • Most of the oxidation-reduction reactions fall into one of the following simple categories: • Combination Reaction • Decomposition Reactions • Displacement Reactions • Combustion Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  46. Types of Chemical ReactionsOxidation-Reduction Reactions • Combination Reactions • A combination reaction is a reaction in which two substances combine to form a third substance. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  47. Types of Chemical ReactionsOxidation-Reduction Reactions • Decomposition Reactions • A decomposition reaction is a reaction in which a single compound reacts to give two or more substances. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  48. A displacement reaction (also called a single- replacement reaction) is a reaction in which an element reacts with a compound, displacing an element from it. Types of Chemical ReactionsOxidation-Reduction Reactions • Displacement Reactions Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  49. Types of Chemical ReactionsOxidation-Reduction Reactions • Combustion Reactions • A combustion reaction is a reaction in which a substance reacts with oxygen, usually with the rapid release of heat to produce a flame. • Common combustion reactions involve hydrocarbons • Hydrocarbon + O2 CO2 + H2O HW 32 Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

  50. Types of Chemical ReactionsOxidation-Reduction Reactions • How do we balance Oxidation-Reduction Reactions • Look again at the net reaction of iron with copper(II) sulfate. • We can write this reaction in terms of two half-reactions. Material was developed by combining Janusa’s material with the lecture outline provided with Ebbing, D. D.; Gammon, S. D. General Chemistry, 8th ed., Houghton Mifflin, New York, NY, 2005. Majority of figures/tables are from the Ebbing lecture outline.

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