<p> Name: ______</p><p>Teacher: ______</p><p>DO NOT OPEN THE EXAMINATION PAPER UNTIL YOU ARE TOLD BY THE SUPERVISOR TO BEGIN</p><p>Gonzaga High School CHEMISTRY 2202</p><p>FINAL EXAMINATION June 2014</p><p>Value: 80 Marks Duration: 2 Hours</p><p>General Instructions</p><p>This examination consists of two parts. Both parts are contained in this booklet and further general instructions are provided on appropriate pages.</p><p>Part I – Selected Response (40 marks) Select the letter of the correct response from those provided. Shade the letter on the Scantron card Do ALL questions in this section.</p><p>Part II - Constructed Response (40 marks) Answer ALL questions fully and concisely in the space provided. Show all work and use correct units and significant digits in all final answers.</p><p>Student Checklist</p><p>The items below are your responsibility. Please ensure that they are completed.</p><p> Write your name and teacher's name on the top of this page.  Write your name, teacher’s name, course name and number on the Part I answer sheet.  Check the exam to see that there are no missing pages.</p><p>ALL MATERIALS MUST BE PASSED IN WITH THIS EXAM. Use your time wisely. Good luck!</p><p>Chemistry 2202 Final Exam – June 2014 Page 1 Part I Selected Response Total Value: 40 Marks</p><p>1. Which isotope has 27 protons and 31 neutrons?</p><p>(A) Cobalt-27</p><p>(B) Cobalt-58</p><p>(C) Gallium-27</p><p>(D) Gallium-58</p><p>2. Which is defined as the amount of carbon atoms in a 12g sample of carbon-12?</p><p>(A) Atomic mass </p><p>(B) Avogadro’s number</p><p>(C) Limiting reagent</p><p>(D) Standard pressure</p><p>3. What is the number of hydrogen atoms in 2.3 moles of CH3COOH? </p><p>(A) 6.9</p><p>(B) 9.2</p><p>(C) 1.03 x 1024 </p><p>(D) 5.5 x 1024 </p><p>4. The imaginary element “vikingium” has two known isotopes, as shown by the data below. What is the average atomic mass of vikingium?</p><p>Isotope Percentage Abundance (%) Isotopic Atomic Mass (amu)</p><p> vikingium -274 80.00 273.9</p><p> vikingium -277 20.00 277.1</p><p>(A) 274.9 amu</p><p>(B) 276.3 amu</p><p>(C) 274.5 amu</p><p>(D) 275.7 amu</p><p>5. What is the molar mass of SnCl4●5H2O? </p><p>(A) 350.59 g/mol (B) 172.16 g/mol</p><p>(C) 305.59 g/mol (D) 172.19 g/mol</p><p>Chemistry 2202 Final Exam – June 2014 Page 2 6. A 33.55 g sample of a compound with the chemical formula Na2SOx contains 0.2662 mol. What is the identity of the compound? </p><p>(A) Na2SO</p><p>(B) Na2SO2</p><p>(C) Na2SO3</p><p>(D) Na2SO4 7. What is the number of moles in 27.52 g of PbS?</p><p>(A) 8.694 (B) 0.1150 (C) 6.584 X 103 (D) 266.78 8. Which term represents the volume of one mole of gas at STP?</p><p>(A) molar mass</p><p>(B) molar volume</p><p>(C) percent composition</p><p>(D) percent volume</p><p>9. What is the percentage of Calcium by mass in Ca(C2H3O2)2?</p><p>(A) 3.8%</p><p>(B) 25.4%</p><p>(C) 30.4%</p><p>(D) 40.5%</p><p>10. A compound has an empirical formula of C2HCl and a molar mass of 181.44 g/mol. What is the molecular formula of the compound? </p><p>(A) C2HCl</p><p>(B) C4H2Cl2</p><p>(C) C6H3Cl3</p><p>(D) C8H4Cl4</p><p>11. Which has low solubility in water?</p><p>(A) NaCl</p><p>(B) KNO3 </p><p>(C) MgS</p><p>(D) AgCH3COO</p><p>Chemistry 2202 Final Exam – June 2014 Page 3 12. What are the units for molar concentration? </p><p>(A) g/L</p><p>(B) L</p><p>(C) mg</p><p>(D) mol/L</p><p>13. Which substance, when dissolved in water, is considered to be a non-electrolyte?</p><p>(A) NaCl</p><p>(B) CuSO4</p><p>(C) C2H5OH</p><p>(D) NH4OH</p><p>14. What is the final concentration when 2.0 L of 1.75 mol/L H2SO4(aq) is diluted to a final volume of 6.4 L?</p><p>(A) 0.13 mol/L</p><p>(B) 0.83 mol/L</p><p>(C) 0.55 mol/L</p><p>(D) 7.5 mol/L</p><p>15. The solubility of KCl in water is 295 g/L at 25°C. Which term describes a KCl solution which is 375 g/L at 25°C? </p><p>(A) concentrated (B) dilute (C) saturated (D) supersaturated 16. Which term represents the amount of product obtained from a chemical reaction in a lab setting?</p><p>(A) actual yield (B) excess reagent (C) limiting reagent (D) theoretical yield</p><p>17. For the reaction: 2 K(s) + Cl2(g) → 2 KCl(s)</p><p>How many moles of potassium chloride will be produced if 1.54 mol of chlorine gas reacts?</p><p>(A) 0.39 mol (B) 0.77 mol (C) 1.54 mol (D) 3.08 mol</p><p>Chemistry 2202 Final Exam – June 2014 Page 4 Chemistry 2202 Final Exam – June 2014 Page 5 18. Which is a pipette?</p><p>(A)</p><p>(B)</p><p>(C)</p><p>(D)</p><p>18. Which is a network covalent solid at room temperature?</p><p>(E) CS2 (F) CuZn (G) LiCl</p><p>(H) SiO2</p><p>Chemistry 2202 Final Exam – June 2014 Page 6 19. How many valence electrons are in an atom of boron, B? (I) 2 (J) 3 (K) 5 (L) 7</p><p>20. Which has a double bond? </p><p>(M) F2</p><p>(N) O2</p><p>(O) N2</p><p>(P) H2</p><p>21. Which Lewis diagram is correct?</p><p>(A)</p><p>(B)</p><p>(C)</p><p>(D)</p><p>22. What is the shape around an atom with 1 bonding groups and 3 lone pairs? (Q) bent (v-shaped) (R) linear (S) tetrahedral (T) trigonal planar</p><p>23. Which contains London dispersion forces only?</p><p>(A) CCl4</p><p>(B) OCl2</p><p>(C) C2H3Cl</p><p>(D) PCl3</p><p>Chemistry 2202 Final Exam – June 2014 Page 7 24. Which shape repeats in the structure of diamond shown below?</p><p>(U) bent (v-shaped) (V) pyramidal (W) tetrahedral (X) trigonal planar</p><p>26. In order of decreasing polarity (most polar to least polar), what is the correct order of these bonds? i) S – H ii) P – H iii) Cl – H</p><p>(A) i > ii > iii (B) ii > i > iii (C) iii > i > ii (D) iii > ii > i</p><p>18. Which compound contains ionic bonding?</p><p>(Y) CCl4 (Z) CsBr</p><p>(AA) H2CO (AB) SiC</p><p>28. A student has two unknown substances, X and Y. Substance X does not conduct electricity as a solid or a liquid. Substance Y does conduct electricity as a solid and a liquid. What would be the most likely identities of substances X and Y?</p><p>X Y (A ) (B)</p><p>(C) (D )</p><p>Chemistry 2202 Final Exam – June 2014 Page 8 Chemistry 2202 Final Exam – June 2014 Page 9 29. Which represents the bonding between aluminum, Al, atoms and bromine, Br, atoms?</p><p>(A ) (B)</p><p>(C) (D )</p><p>30. Which compound is polar? (A) cis-1,2-dichloroethene (B)ethene (C)ethyne (D) trans-1,2-dichloroethene</p><p>31. The synthesis of which compound led to the modern definition of organic chemistry? (A) DNA (B)urea (C)benzene (D) polyester</p><p>32. Which is an aromatic hydrocarbon? (A) alkene (B) benzene (C) ether (D) ketone</p><p>33. Which is an alkyne?</p><p>(A) C6H6</p><p>(B) C6H10</p><p>(C) C6H12</p><p>(D) C6H14</p><p>34. What is the name of the compound below? </p><p>(A) 2-ethyl-6-methylheptane (B) 6-ethyl-2-methylheptane</p><p>Chemistry 2202 Final Exam – June 2014 Page 10 (C) 2,6-dimethyloctane (D) 3,7-dimethyloctane</p><p>35. Which is a structural isomer of this molecule?</p><p>(A)</p><p>(B)</p><p>(C)</p><p>(D)</p><p>36. Which reaction represents thermal reforming? (A) (B) (C) (D)</p><p>37. Which contains a carboxyl functional group? (A) hexanol (B) hexanone (C) hexanal (D) hexanoic acid</p><p>38. What possible product(s) form from the reaction of 1-butanol with ethanoic acid? (A) ethyl butanoate (B) butyl ethanoate (C) butyl ethyl ether (D) ethyl butyl ether</p><p>39. Which structure has delocalized electrons?</p><p>(A) (B)</p><p>(C)</p><p>(D)</p><p>40. Which reactant could be added to an alkene to produce an alcohol?</p><p>(A) H2</p><p>(B) H2O</p><p>Chemistry 2202 Final Exam – June 2014 Page 11 (C) Br2 (D) HBr</p><p>End of Part I</p><p>Part II Constructed Response Total Value: 40 Marks</p><p>Answer ALL questions in the space provided. Show all workings and report all final answers with correct significant digits and units. </p><p>Value 2 41.(a) Calculate the mass of 12.45 L of Argon, Ar(g), at STP.</p><p>2 (b) Calculate the percent composition of each element in Rb2SO4.</p><p>25. 26. </p><p>Chemistry 2202 Final Exam – June 2014 Page 12 3 (c) i) Caffeine has the following percent composition: carbon 49.48%, hydrogen 5.19%, oxygen 16.48% and nitrogen 28.85%. Calculate the empirical formula.</p><p>1 ii) If the molar mass of the above compound is 194.19 g/mol, determine the molecular formula.</p><p>27. Value 41. (continued)</p><p>2 (d) Calculate the volume of a 0.350 mol/L solution that would contain exactly 1.00 g of sodium carbonate, Na2CO3.</p><p>(e) A solution of K2SO4 (aq) has a potassium ion concentration of 0.455 mol/L. </p><p> i) Write a balanced dissociation equation.</p><p>2</p><p> ii) What is the K2SO4(aq) concentration?</p><p>3 (f) Given the following balanced equation; what mass of Al2O3(s) must be decomposed to produce 80.0g of oxygen gas?</p><p>Chemistry 2202 Final Exam – June 2014 Page 13 2 Al2O3(s) → 4Al(s) + 3O2(g)</p><p>28. Value 41. (continued)</p><p>3 (g) For the reaction: NaOH(s) + HNO3(aq) → NaNO3(aq) + H2O(l)</p><p>5.0 of sodium hydroxide, NaOH(s) is reacted with 50.0 mL of 1.25 mol/L HNO3(aq). </p><p>(i) Determine the limiting reagent.</p><p>Chemistry 2202 Final Exam – June 2014 Page 14 1 (ii) Calculate the concentration of NaNO3(aq) produced. </p><p>29. Value 3 42.(a) Complete the following table for CH3NH2.</p><p>Lewis Diagram</p><p>VSEPR Shape diagram</p><p>Name of shape around each central atom</p><p>2 (b) Explain why a molecule of H2O is polar. Justify your answer with a diagram.</p><p>Chemistry 2202 Final Exam – June 2014 Page 15 2 (c) Explain, using the appropriate bonding theory, why metals are malleable.</p><p>Chemistry 2202 Final Exam – June 2014 Page 16 30. Value 42. (continued)</p><p>3 (d) Rank the following substances in order of increasing boiling points. Justify your answer. </p><p>NaCl H2O CH4 NH3</p><p>5 43.(a) Complete the table with either a structural diagram or IUPAC name.</p><p>IUPAC Name Structural Diagram</p><p>1,3-diethylcyclopentane</p><p> o-dibromobenzene</p><p>5-ethyl-2,3-dimethylheptanal</p><p>31. Value 43. (continued)</p><p>Chemistry 2202 Final Exam – June 2014 Page 17 2 (b) Draw and name two isomers for C3H8O. </p><p>Structure 1: Structure 2:</p><p>Name: Name:</p><p>4 (c) Provide the missing reactant or product for the following three reactions.</p><p>Reaction 1</p><p>+ + </p><p>Reaction 2</p><p>+ + HBr</p><p>Isomer 1 Isomer 2</p><p>Reaction 3</p><p>+ F2</p><p>End of Exam</p><p>Chemistry 2202 Final Exam – June 2014 Page 18</p>