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Final Exam Review Stations Units 4-7

Final Exam Review Stations Units 4-7. 45 Questions in 80 minutes (TOTAL) 18 Questions = 40 points 32:00 timer. Station 1 (Bonding Unit 4). Which of the following chemical formulas is incorrect? BaOH 2 NH 4 Cl KNO 3 CaSO 4 Sr (C 2 H 3 O 2 ) 2. Station 1 (Bonding Unit 4).

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Final Exam Review Stations Units 4-7

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  1. Final Exam Review StationsUnits 4-7 45Questions in 80 minutes (TOTAL) 18 Questions = 40points 32:00 timer

  2. Station 1 (Bonding Unit 4) • Which of the following chemical formulas is incorrect? • BaOH2 • NH4Cl • KNO3 • CaSO4 • Sr(C2H3O2)2

  3. Station 1 (Bonding Unit 4) • Which of the following chemical formulas is incorrect? • BaOH2 • NH4Cl • KNO3 • CaSO4 • Sr(C2H3O2)2

  4. Station 2 (Bonding Unit 4) • What is the correct formula for copper(II) oxide? • Cu2O2 • Cu2O • CuO • CuO2 • None of these

  5. Station 2 (Bonding Unit 4) • What is the correct formula for copper(II) oxide? • Cu2O2 • Cu2O • CuO • CuO2 • None of these

  6. Station 3 (Bonding Unit 3) • Name the following compound: SnCO3 • Tin carbon trioxide • Tin carbonate • Tin (I) carbonate • Tin (II) carbonate • None of these

  7. Station 3 (Bonding Unit 3) • Name the following compound: SnCO3 • Tin carbon trioxide • Tin carbonate • Tin (I) carbonate • Tin (II) carbonate • None of these

  8. Station 4 (Bonding Unit 4) • Name the following compound: PCl3 • Phosphorus chloride • Monophosphorustrichloride • Phosphorus trichloride • Phosphorus chloride (III) • None of these

  9. Station 4 (Bonding Unit 4) • Name the following compound: PCl3 • Phosphorus chloride • Monophosphorustrichloride • Phosphorus trichloride • Phosphorus chloride (III) • None of these

  10. Station 5 (Bonding Unit 4) • How many double bonds does CO2 contain? • 0 • 1 • 2 • 3 • 4

  11. Station 5 (Bonding Unit 4) • How many double bonds does CO2 contain? • 0 • 1 • 2 • 3 • 4

  12. Station 6 (Bonding Unit 4) • Which of the following molecules is polar? • NH3 • O2 • CCl4 • CO2 • None of these is polar.

  13. Station 6 (Bonding Unit 4) • Which of the following molecules is polar? • NH3 • O2 • CCl4 • CO2 • None of these is polar.

  14. Station 7 (Reactions Unit 5) • What type of reaction is represented with the following chemical equation: CaSO4 + KBr CaBr2 + K2SO4 • Synthesis • Decomposition • Combustion • Single Replacement • Double Replacement

  15. Station 7 (Reactions Unit 5) • What type of reaction is represented with the following chemical equation: CaSO4 + KBr CaBr2 + K2SO4 • Synthesis • Decomposition • Combustion • Single Replacement • Double Replacement

  16. Station 8 (Chemical Reactions Unit 5) • The coefficient for H2O in the following equation is ________________. Ba(OH)2 + H3N  Ba3N2 + H2O • 2 • 3 • 4 • 5 • 6

  17. Station 8 (Chemical Reactions Unit 5) • The coefficient for H2O in the following equation is ________________. Ba(OH)2 + H3N  Ba3N2 + H2O • 2 • 3 • 4 • 5 • 6

  18. Station 9 (Chemical Reactions Unit 5) • Which of the following will be the precipitate in the reaction between CaCl2 and Na2SO4? • CaSO4 • CaNa • NaCl • ClSO4 • None of these

  19. Station 9 (Chemical Reactions Unit 5) • Which of the following will be the precipitate in the reaction between CaCl2 and Na2SO4? • CaSO4 • CaNa • NaCl • ClSO4 • None of these

  20. Station 10 (Chemical Reactions Unit 5) • Which of the following is the net ionic reaction for the reaction between CuI2 and Pb(NO3)2? • Cu2+ + 2NO3- Cu(NO3)2 • Pb2+ + 2I-  PbI2 • Cu2+ + 2I- + Pb2+ + 2NO3-  Cu2+ + 2NO3- + Pb2+ + 2I- • Cu2+ + 2I- + Pb2+ + 2NO3-  Cu2+ + 2NO3- + PbI2

  21. Station 10 (Chemical Reactions Unit 5) • Which of the following is the net ionic reaction for the reaction between CuI2 and Pb(NO3)2? • Cu2+ + 2NO3- Cu(NO3)2 • Pb2+ + 2I-  PbI2 • Cu2+ + 2I- + Pb2+ + 2NO3-  Cu2+ + 2NO3- + Pb2+ + 2I- • Cu2+ + 2I- + Pb2+ + 2NO3-  Cu2+ + 2NO3- + PbI2

  22. Station 11 (Moles Unit 6) • Convert 4.5 cg CO2 to molecules. • 6.2x1020 molecules • 6.2x1024 molecules • 1.2x1028 molecules • 1.2x1026 molecules

  23. Station 11 (Moles Unit 6) • Convert 4.5 cg CO2 to molecules. • 6.2x1020 molecules • 6.2x1024 molecules • 1.2x1028 molecules • 1.2x1026 molecules

  24. Station 12 (Moles Unit 6) • Calculate the mass of 4.3L of oxygen gas. • 3.1 grams • 6.1 grams • 31 g rams • 61 grams • 138 grams

  25. Station 12 (Moles Unit 6) • Calculate the mass of 4.3L of oxygen gas. • 3.1 grams • 6.1 grams • 31 g rams • 61 grams • 138 grams

  26. Station 13 (Moles Unit 6) • Calculate the percent by mass of N in ammonium chloride. • 1.05% N • 2.61% N • 10.5% N • 26.1% N • 36.6% N

  27. Station 13 (Moles Unit 6) • Calculate the percent by mass of N in ammonium chloride. • 1.05% N • 2.61% N • 10.5% N • 26.1% N • 36.6% N

  28. Station 14 (Moles Unit 6) • A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. The molecular mass is calculated to be 180.0 g/mol. Determine the molecular formula of the compound. • CH2O • C3H6O3 • C2H4O2 • C6H12O6 • C18H36O18

  29. Station 14 (Moles Unit 6) • A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. The molecular mass is calculated to be 180.0 g/mol. Determine the molecular formula of the compound. • CH2O • C3H6O3 • C2H4O2 • C6H12O6 • C18H36O18

  30. Station 15 (Stoichiometry Unit 7) If 1.7 grams of hydrogen is theoretically produced, what was my actual yield of hydrogen if my percent yield is 53.6%? • 91.1 grams of hydrogen • 3.17 grams of hydrogen • 0.911 grams of hydrogen • 0.304 grams of hydrogen • None of these

  31. Station 15 (Stoichiometry Unit 7) If 1.7 grams of hydrogen is theoretically produced, what was my actual yield of hydrogen if my percent yield is 53.6%? • 91.1 grams of hydrogen • 3.17 grams of hydrogen • 0.911 grams of hydrogen • 0.304 grams of hydrogen • None of these

  32. Station 16 (Stoichiometry Unit 7) P4 + 5O2 P4O10 • Determine the mass of tetraphosphorusdecoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined. • 57.3 grams of P4O10 • 88.7 grams of P4O10 • 146 grams of P4O10 • 25.0 grams of P4O10 • 50.0 grams of P4O10

  33. Station 16 (Stoichiometry Unit 7) P4 + 5O2 P4O10 • Determine the mass of tetraphosphorusdecoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined. • 57.3 grams of P4O10 • 88.7 grams of P4O10 • 146 grams of P4O10 • 25.0 grams of P4O10 • 50.0 grams of P4O10

  34. Station 17 (Stoichiometry Unit 7) • If the theoretical yield of the reaction is 53.6 grams, what is the percent yield if 51.4 grams is collected? • 1.04% • 10.4% • 0.96% • 95.8% • 104%

  35. Station 17 (Stoichiometry Unit 7) • If the theoretical yield of the reaction is 53.6 grams, what is the percent yield if 51.4 grams is collected? • 1.04% • 10.4% • 0.96% • 95.8% • 104%

  36. Station 18 (Stoichiometry Unit 7) P4 + 5O2 P4O10 If 57.3 grams of tetraphosphorusdecoxide formed when 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined. Some oxygen gas remains after the reaction. What mass of O2 remains after the reaction stops? • 0.06 grams of O2 • 49.94 grams of O2 • 0.03 grams of O2 • 32.3 grams of O2 • 17.7 grams of O2

  37. Station 18 (Stoichiometry Unit 7) P4 + 5O2 P4O10 If 57.3 grams of tetraphosphorusdecoxide formed when 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined. Some oxygen gas remains after the reaction. What mass of O2 remains after the reaction stops? • 0.06 grams of O2 • 49.94 grams of O2 • 0.03 grams of O2 • 32.3 grams of O2 • 17.7 grams of O2

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