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Chapter 7 Chemical Reactions

Chapter 7 Chemical Reactions. Chemical Reactions. Chemical reactions are processes in which one set of chemicals are converted to a new set of chemicals Chemical reactions are described by chemical equations. Evidence for Chemical Reactions. A gas is produced. A precipitate is formed.

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Chapter 7 Chemical Reactions

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  1. Chapter 7Chemical Reactions

  2. Chemical Reactions • Chemical reactions are processes in which one set of chemicals are converted to a new set of chemicals • Chemical reactions are described by chemical equations.

  3. Evidence for Chemical Reactions • A gas is produced. • A precipitate is formed. • A permanent color change is observed. • An energy change occurs.

  4. Chemical Equations • N2 (g) + 3 H2 (g)  2 NH3 (g) • must be balanced to satisfy Law of conservation of mass • State Designations • (g) gas • (l) liquid • (s) solid • (aq) aqueous

  5. Copper(II) oxide reacts with ammonia (NH3) to yield copper, nitrogen gas, and water. • Write a balanced equation for this reaction.

  6. Ammonia reacts with oxygen gas to form nitrogen monoxide and water.

  7. Zinc metal reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. • Potassium chlorate when heated, decomposes to form potassium chloride and oxygen gas.

  8. Hexane(C6H14) burns in oxygen gas to form carbon dioxide and water. • Lead(II) nitrate reacts with potassium chromate to form lead(II) chromate (yellow ppt.) and potassium nitrate.

  9. Some more examples • N2 + H2 NH3 • Be2C + H2O  Be(OH)2 + CH4 • HCl + CaCO3 CaCl2 + H2O + CO2 • C2H6 + O2 CO2 + H2O

  10. Electrolyte • Substances such as NaCl of KBr, which conduct electricity when dissolved in water. Dissociates to produce ions in solution. Non electrolyte • Substances such as sucrose, which do not conduct electricity when dissolved in water. Do not produce ions in solution.

  11. Dissociation • The breaking apart of a molecular substance into ions in solution.

  12. NaCl(aq) + AgNO3(aq)  AgCl(s) + NaNO3(aq)

  13. Writing ionic equations • Soluble ionic substances are written as ions. • Strong acids and bases are written as ions. • HClO4 NaOH • H2SO4 KOH • HBr Ba(OH)2 • HCl Ca(OH)2 • HNO3 all soluble hydroxides • Weak acids and bases are written in the undissociated form. • Weak electrolytes or insoluble salts written as molecular formula.

  14. Solubility Rules • Alkali metals and NH4+ compounds are soluble. • Nitrates(NO3), acetates (CH3CO2), chlorates (ClO3), and perchlorates(ClO4) are soluble. • Chlorides(Cl), bromides(Br), iodides(I), are soluble except for Silver(Ag+),mercury(I)(Hg2+2), and lead(II)( Pb+2) halides. • Sulfates(SO42) are soluble except for Sr+2, Ba+2, Pb+2, and Hg2+2. • Hydroxides(OH) are insoluble except for alkali metals and NH4+ (see#1). • Sulfides(S2), carbonates(CO32), phosphates(PO43), and chromates(CrO42) are insoluble except for alkali metals and NH4+ (see#1).

  15. Vinegar(acetic acid) reacts with baking soda (sodium bicarbonate) to produce carbon dioxide gas, sodium acetate, and water.

  16. Iron(III) chloride reacts with ammonium hydroxide to form iron(III) hydroxide (brown ppt.) and ammonium chloride. • Barium hydroxide and ammonium chloride react to form ammonia (NH3), water, and barium chloride.

  17. Classifying Reactions by Type of Chemistry

  18. Classifying Reactions by Type of Chemistry • Precipitation AX + BZ  AZ + BX • Acid Base HX +BOH  BX +H2O • Gas Evolution • H2X + BCO3 H2O + CO2(g) + BX • H2X + BSO3 H2O + SO2(g) + BX • NH4X + BOH  H2O + NH3(g) + BX • Oxidation Reduction A+2 + B  A + B+2 • Combustion CxHxOx+O2CO2 + H2O

  19. Classifying Reactions by what Atoms Do

  20. Classifying Reactions by what Atoms Do • Combination/Synthesis A + Z  AZ • Decomposition AZ  A + Z • Single Displacement A + BZ  AZ + B • Double displacement AX + BZ  AZ + BX • Neutralization HX +BOH  BX +H2O

  21. Predicting ReactionsDouble Displacement

  22. BaCl2 + ZnSO4 • Conventional equation • BaCl2(aq) + ZnSO4(aq) BaSO4(s) + ZnCl2(aq) • Total ionic equation • Ba+2(aq) + 2Cl-1(aq) + Zn+2(aq) + SO4-2(aq)  BaSO4(s) + Zn+2 (aq) + 2Cl-1(aq) • Net ionic equation • Ba+2(aq) + SO4-2(aq)  BaSO4(s)

  23. AgNO3 + Na2SO4 • AgNO3 + Na2SO4 NR

  24. (NH4)2CO3 + CaCl2 (NH4)2CO3 + CaCl2 2 NH4Cl + CaCO3(s)

  25. Na2S + ZnCl2 Na2S + ZnCl22 NaCl + ZnS(s)

  26. K3PO4 + Sr(NO3)2 2 K3PO4 + 3 Sr(NO3)2 6 KNO3 + Sr3(PO4)2 (s)

  27. Mg(NO3)2 + NaOH  Mg(NO3)2 + 2 NaOH  Mg(OH)2(s)+ 2 NaNO3

  28. Ba(OH)2 + H3PO4 3 Ba(OH)2 +2 H3PO4 Ba3(PO4)2(s) + 6 H2O

  29. HClO4 + NaOH  HClO4 + NaOH  H2O(l) + NaClO4

  30. H3PO3 + NH3 H3PO3 + 3 NH3 (NH4)3PO3

  31. CH3COOH + KOH  CH3COOH + KOH  CH3COO-K+ + H2O

  32. NH4Cl + KOH  NH4Cl + KOH  (NH4OH + KCl)  NH3 +HOH+ KCl

  33. K2CO3 + HCl  K2CO3 + 2 HCl  (H2CO3 + 2 KCl) H2O + CO2 + 2 KCl

  34. K2SO3 + HCl  K2SO3 + 2 HCl  (H2SO3 + 2 KCl) H2O + SO2 + 2 KCl

  35. H2CO3 + Ca(NO3)2  H2CO3 + Ca(NO3)2  CaCO3(s) + 2 HNO3

  36. Fe(NO3)3 + NH3 Fe(NO3)3 + 3NH3 + 3H2O Fe(OH)3(s) + 3NH4NO3

  37. More • K2S + CuSO4 • Na2CrO4 + Pb(C2H3O2)2 • ZnBr2 + K3PO4 • KOH + NH4Cl  • NH3 + HCN 

  38. Predicting Reactions Single Displacement (AKA Single Replacement)

  39. Pb + Zn(NO3)2

  40. Fe + HCl 

  41. Cu + AgNO3

  42. Cr + Zn(NO3)2

  43. Pb + Sn(NO3)2

  44. H2 + NiCl2

  45. Cr + NiCl2

  46. H2 + Au(NO3)2

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