1. Chemical Equations

2. Like a recipe: ReactantsProducts 2H 2 (g) + O 2 (g)  2H 2 O(l) Introduction

3. Symbols  Yields or Produces (s)solid (l)liquid (aq)aqueous (g) gas Introduction

4. The Difference between (l) and (aq) Liquid – Pure liquid.Nothing is in it. H 2 O(l) Aqueous – Dissolved in water. NaCl(aq) = Salt water (l) or (aq)?

5. Distilled water Tap Water Iced Tea Mouthwash Gasoline Paint (l) or (aq)?

6. Easy Examples: Hd 10 + Bu 8  HdBu Balancing

12. 1. Must balance because of the Law of Cons. of Matter 2.Rules: Can only change the coefficient, never the subscript Coefficient multiplies every atom in a formula Balancing

13. S + O 2  SO P 2 (g) + H 2 (g)  PH 3 (g) Balancing

14. Al + Cl 2  AlCl 3 H 2 O + C  H 2 + CO C 3 H 8 + O 2  CO 2 + H 2 O Balancing

15. C 2 H 6 + O 2  CO 2 + H 2 O C 4 H 10 + O 2  CO 2 + H 2 O Na 2 SO 4 + Fe(NO 3 ) 3  NaNO 3 + Fe 2 (SO 4 ) 3 Balancing

16. Fe(OH) 3 + H 2 SO 4  Fe 2 (SO 4 ) 3 + H 2 O Sodium reacts with water to form sodium hydroxide and hydrogen gas Balancing

17. Magnesium hydroxide reacts with hydrochloric acid (HCl) to form magnesium chloride and water.

18. Calcium reacts with water to form hydrogen and calcium hydroxide Aluminum nitrate reacts with sodium hydroxide to form aluminum hydroxide and sodium nitrate

19. Copper(II) chloride reacts with iron(III) sulfate to form copper(II)sulfate and iron(III) chloride Phosphoric acid (H 3 PO 4 ) reacts with calcium hydroxide to form water and calcium phosphate Balancing

20. Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  MgSO 4 + AlPO 4 Fe 2 S 3 + O 2  Fe 2 O 3 + SO 2 Ru 2 O 3 + CO  Ru + CO 2 NaBr + Al(NO 3 ) 3  NaNO 3 + AlBr 3 Ba + AlCl 3  BaCl 2 + Al Propane (C 3 H 8 ) is burned in oxygen to produce carbon dioxide and water Iron(III)nitrate reacts with lithium carbonate to form iron(III)carbonate and lithium nitrate. Sodium Chlorate decomposes to form sodium chloride and oxygen gas

21. Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  3MgSO 4 + 2AlPO 4 2Fe 2 S 3 + 9O 2  2Fe 2 O 3 + 6SO 2 Ru 2 O 3 + 3CO  2Ru + 3CO 2 3NaBr + Al(NO 3 ) 3  3NaNO 3 + AlBr 3 3Ba + 2AlCl 3  3BaCl 2 + 2Al C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 2Fe(NO 3 ) 3 + 3Li 2 CO 3  Fe 2 (CO 3 ) 3 + 6LiNO 3 2NaClO 3  2NaCl + 3O 2

22. Sulfur trioxide reacts with water to form sulfuric acid (H 2 SO 4 ) Boron sulfide, B 2 S 3, reacts with water to form boric acid, H 3 BO 3 and hydrogen sulfide, H 2 S. Mercury(II)nitrate decomposes to form mercury(II) oxide, nitrogen dioxide, and oxygen Hydrogen sulfide reacts with iron(III)hydroxide to form iron(III)sulfide and water.

23. Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  MgSO 4 + AlPO 4 Fe 2 S 3 + O 2  Fe 2 O 3 + SO 2 Ru 2 O 3 + CO  Ru + CO 2 a.Propane (C 3 H 8 ) is burned in oxygen to produce carbon dioxide and water b.Iron(III)nitrate reacts with lithium carbonate to form iron(III)carbonate and lithium nitrate. c.Sodium Chlorate decomposes to form sodium chloride and oxygen gas

24. Chemical Equations

27. Synthesis (Combination) Decomposition Combustion Single Replacement Double Replacement Dissolving Types of Reactions

28. 1. Synthesis Two or more elements or compounds combine to form a new compound Examples Na(s) + Cl 2 (g)  NaCl(s) C(s) + O 2 (g)  CO 2 (g) CaO(s) + CO 2 (g)  CaCO 3 (s) Types of Reactions

29. 2. Decomposition Opposite of synthesis One compound breaks down, usually requires heat energy Types of Reactions

30. Dima, a 40,000 year old frozen mammoth (Alaska)

32. Examples: HgO(s)  Hg(l) + O 2 (g) CaCO 3 (s)  CaO(s) + CO 2 (g) KClO 3 (s)  KCl(s) + O 2 (g) Types of Reactions

33. Duke: In loving memory.

34. 3. Combustion Fast reaction with O 2 (Burning) Hydrocarbons burn to form CO 2 and H 2 O Types of Reactions

35. Examples: Mg(s) + O 2 (g)  MgO(s) C 8 H 18 + O 2  CO 2 + H 2 O C 6 H 12 O 6 + O 2  CO 2 + H 2 O Types of Reactions

36. 4. Single replacement One element replaces another Not every element can replace every other element Types of Reactions

37. Zn + CuCl 2  Cu + ZnCl 2 Cr + Pb(NO 3 ) 2  Pb + Cr(NO 3 ) 3 Mg + HCl  MgCl 2 + H 2

38. 5. Double replacement Two elements switch places ZnBr 2 + AgNO 3  Zn(NO 3 ) 2 + AgBr BaCl 2 + H 2 SO 4  BaSO 4 + HCl Na 2 CO 3 + CaCl 2  CaCO 3 + NaCl Types of Reactions

39. Acid/Base Reactions A special type of double replacement Acids a. produce H + b. Often start with H (HCl, H 2 SO 4, H 3 PO 4 ) Types of Reactions

40. Bases a. produce OH - b. Hydroxides (Drano, NaOH) NaOH + HCl  KOH + HCl  Types of Reactions

41. 6. Dissolving A. Molecular Compounds 1) Contain all non-metals 2) Do not break up into ions in water 3) Some are still soluble: C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) Types of Reactions

43. B. Ionic Compounds (and acids) 1) Contain a metal 2) Break up into ions in water. 3) Examples: NaCl(s)  Na + (aq) + Cl - (aq) CaCl 2 (s)  Ca 2+ (aq) + 2Cl - (aq) KNO 3 (s)  K + (aq) + NO 3 - (aq) 4) Different than decomp. because ions are produced. Types of Reactions

48. What Ions are produced when these dissolve: AlCl 3 (s)  Na 2 CO 3 (s)  NH 4 Cl(s)  FeBr 2 (s)  (NH 4 ) 2 Cr 2 O 7 (s)  Types of Reactions

49. BaCO 3 (s)  BaO(s) + CO 2 (g) Ca(NO 3 ) 2 (s)  Ca 2+ (aq) + 2NO 3 - (aq) KOH + HBr  KBr + H 2 O N 2 + H 2  NH 3 BaCl 2 + MgSO 4  BaSO 4 + MgCl 2 Cr + Pb(NO 3 ) 2  Pb + Cr(NO 3 ) 3 C 5 H 12 + O 2  CO 2 + H 2 O Types of Reactions

50. Steps: 1.Identify the type of reaction 2.Break all elements into ions (generally keep polyatomic together) 3.Write the products 4.Balance the equation Predicting Reactions

51. K + O 2  Mg + O 2  Al + Cl 2  Na + N 2  K + F 2  Predicting Reactions

52. CH 4 + O 2  C 2 H 6 + O 2  C 3 H 8 + O 2  C 6 H 6 + O 2  Predicting Reactions

53. CuSO 4 + NaOH  BaCl 2 + AgNO 3  HNO 3 + LiOH  H 2 SO 4 + KOH  AgNO 3 + HCl  Predicting Reactions

54. K + Fe(OH) 2  Al 2 O 3 + Mg  Fe + CuCl 2  HCl + Al  Na + Ca(NO 3 ) 2 

55. CuCl 2 (s) (placed in water)  KNO 3 (s) (placed in water)  Mg(NO 3 ) 2 (s) (placed in water)  Na 3 PO 4 (s) (placed in water) 

56. K 2 CO 3 (s)  (Placed in water) HNO 3 + KOH  Pb(NO 3 ) 2 + K 2 SO 4  Al + O 2  FeCl 3  (Placed in water) H 2 SO 4 + NaOH  C 2 H 4 + O 2  Mg + CaCl 2  Types of Reactions

57. C 4 H 10 + O 2  Ga + Cl 2  Na + HNO 3  H 3 PO 4 + NaOH  Ba(NO 3 ) 2 (s)  (Placed in water) AgNO 3 + KCl  Li + O 2  C 6 H 12 O 6 (s)  (placed in water) Types of Reactions

58. Barium nitrate reacts with copper(II) sulfate Sulfuric acid (H 2 SO 4 ) plus lithium hydroxide Zinc metal reacts with lead(II)nitrate Propane (C 3 H 8 ) is burned in oxygen Aluminum metal reacts with bromine Magnesium phosphate dissolves in water

59. HCl + Ba(OH) 2  HClO 4 + LiOH  Pb(NO 3 ) 2 + KI  H 3 PO 4 + NaOH  H 3 PO 4 + Ca(OH) 2  Types of Reactions

60. 2H 2 +O 2  2H 2 O 2 molecules 4molecules 7molecules 24 molecules

61. CH 4 +2O 2  CO 2 +2H 2 O 5 molecules 18 molecules 16 molecules Molecule to Molecule

62. 2KBrO 3  2KBr+3O 2 2 molecules 4 molecules 6molecules 12 molecules 12 molecules 24 molecules Molecule to Molecule

63. H 3 PO 4 +3NaOH  Na 3 PO 4 +3H 2 O 12 molecules 75 molecules 18 molecs Molecule to Molecule

64. 4Al +3O 2  2Al 2 O 3 100 atoms 12 molecules 32 molecules Molecule to Molecule

66. a)P 2 + H 2  PH 3 b)B 2 H 6 + H 2 O  H 3 BO 3 + H 2 c)C 2 H 4 + O 2  CO 2 + H 2 O d)KBrO 3  KBr + O 2

67. Fe + CuSO 4  KI + Pb(NO 3 ) 2  NaCl (s)  C12H22O11(s)  HCl + NaOH C 3 H 7 OH + O 2  Mg + O 2  (NH 4 ) 2 CO 3 

68. 19.2Al + 3H 2  2Al H 3 4Al + 3O 2  2Al 2 O 3 2Al + 3I 2  2AlI 3 2Al + N 2  2AlN 21.2SbF 5  2Sb + 5F 2 PtO 2  Pt + O 2 3BrF  Br 2 + BrF 3

69. 23.2C 4 H 10 + 13O 2  8CO 2 + 10H 2 O H 2 SO 3  SO 2 + H 2 O 2Na + O 2  Na 2 O 2 2Cu 2 O  4Cu + O 2

70. 25. Ca 2+ (aq) + 2ClO 3 - (aq) Cs + (aq) + Br - (aq) Al 3+ (aq) + 3Cl - (aq) 2Cs + (aq) + SO 3 2- (aq) 27.LiOH  Li + (aq) + OH - (aq) HI  H + (aq) + I - (aq) 56.Ca(OH) 2 + 2HI  CaI 2 + 2H 2 O H 2 SO 4 + 2LiOH  2H 2 O + Li 2 SO 4 2HClO 4 + Ba(OH) 2  2H 2 O + Ba(ClO 4 ) 2

71. Fe + CuSO 4  Pb(NO 3 ) 2 + KI  NaCl(s)  C 12 H 22 O 11 (s)  HCl + NaOH  C 3 H 7 OH + O 2  Mg + O 2  (NH 4 ) 2 CO 3 (heated) 

72. Al + F 2  C 2 H 6 + O 2  KCl(s) (in water)  H 2 SO 4 + KOH  Ba + N 2  KCl + AgNO 3  (NH 4 ) 2 CO 3 (s) (in water) 

73. C 6 H 12 O 6 + O 2  Na 2 CO 3 + FeBr 3  Fe(NO 2 ) 2 (s) (in water)  Li + S 8  K 2 S + FeC 2 O 4  Mg + I 2  HNO 2 + Mg(OH) 2  C 4 H 6 + O 2  HCl + Al 

74. 3. a) 2121 b)2112 c)121 d)2313 5a)1212 b)1333 c)838 d)2343

75. 7a) 1212 b)1211 c)1316 d)1415 9a)1212 b)1331 c)4143 d)1434

76. 11 a) C 6 H 6 O + 7O 2  6CO 2 + 3H 2 O b) Ca(OH) 2 + SO 3  CaSO 4 + H 2 O c) 6Li + N 2  2Li 3 N d) 3Mg + 2Cr(NO 3 ) 3  2Cr + 3Mg(NO 3 ) 2 13Fe 3 O 4 + CO  3FeO + CO 2 17a) 2C 2 H 6 O 2 + 5O 2  4CO 2 + 6H 2 O b) 2B 6 H 12 + 15O 2  6B 2 O 3 + 12H 2 O c) C 6 H 12 + 9O 2  6CO 2 + 6H 2 O d) Pb(C 2 H 5 ) 4 +14O 2  PbO 2 +8CO 2 +10H 2 O

77. 19.2Al + 3H 2  2AlH 3 4Al + 3O 2  2Al 2 O 3 2Al + 3I 2  2AlI 3 2Al + N 2  2AlN 21. SbF 5  F 2 + SbF 3 PtO 2  Pt + O 2 3BrF  Br 2 + BrF 3 25. Ca(ClO 3 ) 2 (s)  Ca 2+ (aq) + 2ClO 3 - (aq) CsBr(s)  Cs + (aq) + Br - (aq) AlCl 3 (s)  Al 3+ (aq) + 3Cl - (aq) Cs 2 SO 3 (s)  2Cs + (aq) + SO 3 2- (aq)

78. Ca 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  3CaSO 4 + 2AlPO 4 2C 4 H 10 + 13O 2  8CO 2 + 10H 2 O 2Fe 2 S 3 + 9O 2  2Fe 2 O 3 + 6SO 2 Fe 2 O 3 + 3CO  2Fe + 3CO 2 3KBr + Al(NO 3 ) 3  3KNO 3 + AlBr 3 2HgNO 3 + Na 2 CO 3  2NaNO 3 + Hg 2 CO 3 3Ca + 2AlCl 3  3CaCl 2 + 2Al 2HgO  2Hg + O 2

79. 2K + Br 2  2KBr 2Au 2 O 3  4Au + 3O 2 2C 6 H 6 + 15O 2  12CO 2 + 6H 2 O P 4 + 10F 2  4PF 5 H 2 SO 4  H 2 O + SO 3

80. Types of Reactions a)Doublej) Single b)Singlek) Combustion c)Combustionl) Synthesis d)Decompositionm) Decomposition e)Synthesisn) Double f)Combustion g)Decompostion h)Single i)Synthesis

81. Na 2 S(s)  2Na + (aq) + S 2- (aq) Li 2 SO 4 (s)  2Li + (aq) + SO 4 2- (aq) FeCl 3 (s)  Fe 3+ (aq) + 3Cl - (aq) NaNO 3 (s)  Na + (aq) + NO 3 - (aq) Ca(NO 3 ) 2 (s)  Ca 2+ (aq) + 2NO 3 - (aq) NH 4 Cl(s)  NH 4 + (aq) + Cl - (aq)

82. SET A 2Al + 3F 2  2AlF 3 3Na 2 CO 3 + 2FeCl 3  Fe 2 (CO 3 ) 3 + 6NaCl AlCl 3 + 3Na  3NaCl + Al 2C 4 H 6 + 11O 2  8CO 2 + 6H 2 O KCl(s)  K + (aq) + Cl - (aq) 2C 2 H 6 + 7O 2  4CO 2 + 6H 2 O Fe(NO 3 ) 2 (s)  Fe 2+ (aq) + 2NO 3 - (aq) 4Na + O 2  2Na 2 O H 2 SO 4 + 2KOH  K 2 SO 4 + 2H 2 O

83. Na 2 S + CuSO 4  Na 2 SO 4 + CuS 3Ba + N 2  Ba 3 N 2 Mg + CuCl 2  Cu + MgCl 2 KCl + AgNO 3  AgCl + KNO 3 2HNO 3 + Ca(OH) 2  2H 2 O + Ca(NO 3 ) 2 (NH 4 ) 2 CO 3  2NH 4 + + CO 3 2- C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O

84. SET B 3K + AlCl 3  Al + 3KCl AgNO 3 + HCl  AgCl + HNO 3 C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 2Al + 3Cl 2  2AlCl 3 NaNO 3 (s) (in water)  Na + (aq) + NO 3 - (aq) HCl + KOH  H 2 O + KCl Mg(NO 3 ) 2 + 2Na  Mg + 2NaNO 3 BaCl 2 + Na 2 SO 4  2NaCl + BaSO 4 CuSO 4 (s) (in water)  Cu 2+ (aq) + SO 4 2- (aq)

85. 2Na + I 2  2NaI Ca(OH) 2 + 2HBr  2H 2 O + CaBr 2 2C 4 H 10 + 13O 2  8CO 2 + 10H 2 O Mg + CuCl 2  MgCl 2 + Cu 3K 2 CO 3 + 2Fe(NO 3 ) 3  6KNO 3 + Fe 2 (CO 3 ) 3

86. Set C 4Li + O 2  2Li 2 O Al(NO 3 ) 3 (s) (in water)  Al 3+ (aq) + 3NO 3 - (aq) 16Ga + 3S 8  8Ga 2 S 3 H 2 SO 4 + 2NaOH  2H 2 O + Na 2 SO 4 3Zn(C 2 H 3 O 2 ) 2 + 2Al  3Zn + 2Al(C 2 H 3 O 2 ) 3 2NaOH + CuCl 2  Cu(OH) 2 + 2NaCl Fe 2 (SO 4 ) 3 (s) (in water)  2Fe 3+ (aq) + 3SO 4 2- (aq) C 2 H 5 OH + 3O 2  2CO 2 + 3H 2 O

87. 3Mg(OH) 2 + 2H 3 PO 4  Mg 3 (PO 4 ) 2 + 6H 2 O Sn + 2HCl  SnCl 2 + H 2 4Al + 3O 2  2Al 2 O 3 2AlBr 3 + 3Na 2 S  6NaBr + Al 2 S 3 2CH 4 O + 3O 2  2CO 2 + 4H 2 O (NH 4 ) 2 CO 3 (s) (in water)  2NH 4 + (aq) + CO 3 2- (aq) 8Mg + S 8  8MgS HNO 3 + LiOH  H 2 O + LiNO 3 2AgNO 3 + Pb  Pb(NO 3 ) 2 + 2Ag

88. CaCl 2 + Na 2 CO 3  NaCl + CaCO 3 CaCl 2 + NaOH  NaCl + Ca(OH) 2 CuSO 4 + NaOH  Na 2 SO 4 + Cu(OH) 2 NaHCO 3 + HCl  NaCl + H 2 O + CO 2

89. 12 a) 612 b)132 c)2214 d)1632 e)3216 f)2112 g)494102

90. 13.CaC 2 + 2H 2 O  Ca(OH) 2 + C 2 H 2 2KClO 3  2KCl + 3O 2 Zn + H 2 SO 4  H 2 + ZnSO 4 PCl 3 + 3H 2 O  H 3 PO 3 + 3HCl 3H 2 S + 2Fe(OH) 3  Fe 2 S 3 + 6H 2 O 14. SO 3 + H 2 O  H 2 SO 4 B 2 S 3 + 6H 2 O  2H 3 BO 3 + 3H 2 S Pb(NO 3 ) 2 + 2NaI  2NaNO 3 + PbI 2 2Hg(NO 3 ) 2  2HgO + 4NO 2 + O 2 Cu + 2H 2 SO 4  CuSO 4 + SO 2 + 2H 2 O

91. 19. a)232synthesis b)1322combustion c)612synthesis d) 111decomposition e) 1874combustion 20. a) 2966combustion b) 112decomposition c) 1653combustion d) 132synthesis e) 112synthesis

92. Na 2 S(s)  2Na + (aq) + S 2- (aq) Li 2 SO 4 (s)  2Li + (aq) + SO 4 2- (aq) FeCl 3 (s)  Fe 3+ (aq) + 3Cl - (aq) 2K + Br 2  2KBr 2Au 2 O 3  4Au + 3O 2 2C 6 H 6 + 15O 2  12CO 2 + 6H 2 O P 4 + 10F 2  4PF 5 H 2 SO 4  H 2 O + SO 3

93. Fe + CuSO 4  Cu + FeSO 4 Pb(NO 3 ) 2 + 2KI  PbI 2 + 2KNO 3 NaCl(s)  Na + (aq) + Cl - (aq) C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) HCl + NaOH  H 2 O + NaCl 2C 3 H 7 OH + 9O 2  6CO 2 + 8H 2 O 2Mg + O 2  2MgO (NH 4 ) 2 CO 3  H 2 O(l) + 2NH 3 (g) + CO 2 (g)