CHEM 1411 SAMPLE FINAL EXAM

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1 PART I - Multiple Choice (2 points each) CHEM 1411 SAMPLE FINAL EXAM 1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following expresses this distance in meters? A x m B x m C x 10 7 m D x 10 6 m 2. Acetic acid boils at o F. What is the boiling point in degrees Celsius? A o C B o C C o C D o C 3. Select the answer with correct number of significant figures for the following calculation: g / (15.4 ml 13.2 ml) = A g/ml B g/ml C. 2 g/ml D. 2.1 g/ml 4. Bromine is the only non-metal that is a liquid at room temperature. Consider the isotope bromine-81, 81 35Br. Select the combination which lists the correct atomic number, number of neutrons, and mass number, respectively: A. 35, 46, 81 B. 35, 81, 46 C. 81, 46, 35 D. 46, 81, Which of the following names is correct for the given chemical formula? A. I 2 O 5, iodine pentoxide B. LiNO 3, lithium nitrate C. PbO, lead(i) oxide D. H 2 SO 4, hydrosulfuric acid 6. Which of the following chemical formulas is not correct for the given chemical name? A. ferric oxide, Fe 2 O 3 B. calcium hydroxide, Ca(OH) 2 C. tetrasulfur dinitride, S 4 N 2 D. potassium chlorite, KClO 3 7. What is the mass in grams of mole of the common antacid calcium carbonate? A x 10 2 g B g C x 10 2 g D x 10 3 g 8. Which one of the following reactions is not balanced? A. 2 C 6 H 6 (l) + 15 O 2 (g) > 12 CO 2 (g) + 6 H 2 O (g) B. B 2 O 3 (s) + 6 HF (l) > 2 BF 3 (g) + 3 H 2 O (l) C. UO 2 (g) + 4 HF (l) > UF 4 (s) + 4 H 2 O (l) D. 2 B 5 H 9 (l) + 12 O 2 (g) > 5 B 2 O 3 (s) + 9 H 2 O (g) Practice Final, CHEM 1411 Page 1

2 9. Which of the following is not a chemical change? A. burning coal B. making bread rise using baking soda C. boiling an egg D. boiling water 10. Which of the following is improperly labeled? A. Cu, transition metal B. Mg, alkaline earth metal C. Br, halogen D. U, noble gas 11. Which of the following has a bond order of 3? I) N 2 II) CN III) O 2 IV) C 2 2 A. I and II B. I only C. I, II, and IV D. II and III 12. Which of the following is a nonelectrolyte in water? I) HF II) ethanol, C 2 H 5 OH III) CH 3 OCH 3 IV) KClO 3 A. II and III B. I, II, and III C. III only D. IV only 13. How many milliliters of 1.50 M KOH solution are needed to supply mole of KOH? A ml B ml C ml D ml 14. Which of the following compounds is water soluble? I) NiCl 2 II) Ag 2 S III) Cs 3 PO 4 IV) (NH 4 ) 2 SO 4 A. IV only B. I, II, and III C. I, II, and IV D. I, III, and IV 15. Which of the following reactions will occur? (I) Ni (s) + ZnSO 4 (aq) > Zn (s) + NiSO 4 (aq) (II) Pb (s) + 2 Ag(NO 3 ) 2 (aq) > 2 Ag (s) + Pb(NO 3 ) 2 (aq) (III) Zn (s) + Ca 2+ (aq) > Ca (s) + Zn 2+ (aq) (IV) 2 Al (s) + 3 FeCl 3 (aq) > 3 Fe (s) + 2 AlCl 3 (aq) A. I only B. II only C. II and IV only D. I and III only Practice Final, CHEM 1411 Page 2

3 16. Which of the following is a weak base? A. NaOH B. Ca(OH) 2 C. NH 3 D. RbOH 17. How many kj of heat must be removed from 1000 g of water (specific heat = J /g o C) to lower the temperature from 18.0 C to 12.0 C? A. 2.5 x 10 2 kj B. 1.4 kj C. 4.2 kj D. 25 kj 18. From the following heats of reaction, 2 C (graphite) + H 2 (g) > C 2 H 2 (g) H o = 227 kj/mole 6 C (graphite) + 3 H 2 (g) > C 6 H 6 (l) H o = 49 kj/mole calculate H o for the reaction 3 C 2 H 2 (g) > C 6 H 6 (l) A. 632 kj/mole B. 632 kj/mole C. 178 kj/mole D. 178 kj/mole 19. The heat of combustion of fructose, C 6 H 12 O 6, is 2812 kj/mole. Using the following information, calculate H f for fructose. C 6 H 12 O 6 (s) + 6 O 2 (g) > 6 CO 2 (g) + 6 H 2 O (l) H o = 2812 kj H f of CO 2 = kj/mole H f of H 2 O = KJ/mole A kj B kj C kj D kj 20. What is the kinetic energy in J and cal of a 45 g golf ball moving at 61 m/s? A. 168 J, 40 cal B. 84 J, 20 cal C. 84 J, 350 cal D. 3.8 J, 16 cal 21. What is the frequency of radiation that has a wavelength of 589 nm? A x s 1 B s 1 C x s 1 D x s The statement, "electrons fill degenerate orbitals singly to the maximum extent" is called A. Aufbau principle B. Hund's rule C. Pauli exclusion principle D. none of these 23. For n = 4, what are the possible values of l? A. 3, 2, 1 B. 4, 3, 2, 1 C. 3, 2, 1, 0 D. 4, 3, 2, 1, 0 Practice Final, CHEM 1411 Page 3

4 24. Arrange the following atoms in order of increasing atomic radius (smallest to largest): N, K, As, Fr A. N<K<As<Fr B. N<As<K<Fr C. As<K<N<Fr D. Fr<K<As<N 25. How many unpaired electrons are in the Lewis dot symbol of a chlorine atom? A. 7 B. 3 C. 5 D Which of the following molecules is polar? A. NH 3 B. BF 3 C. CO 2 D. C 2 H Which one of the following atoms or ions has the largest radius? A. K + B. Cl C. K D. Na 28. Which of the following atoms is the most electronegative? A. Mg B. Cl C. B D. I 29. Which one of the following atoms or ions is isoelectronic with neon, Ne? A. F B. Al 3+ C. Na + D. all of these 30. Determine the oxidation number of sulfur in S 2 O 3 2. A. +3 B. +2 C. +4 D How many total valence electrons are in the SO 4 2 ion? A. 32 e B. 30 e C. 14 e D 28 e 32. What is the hybridization of the central carbon atom in CS 2 and the approximate bond angle around the carbon? A. sp 2, 107 o B. sp 3, 120 o C. sp 2, 120 o D. sp, 180 o 33. The electron-pair geometry and molecular geometry of boron trichloride are A. tetrahedral, tetrahedral B. tetrahedral, trigonal planar C. trigonal planar, trigonal planar D. tetrahedral, trigonal pyramidal 34. How many moles of N 2 gas occupy a volume of 11.2 liters at STP? A mol B mol C mol D mol Practice Final, CHEM 1411 Page 4

5 35. Which one of the following cubic unit cells contains only two atoms? A. simple cubic cell B. face centered cubic cell C. body centered cubic cell D. none of these Practice Final, CHEM 1411 Page 5

6 PART II - Show work (5 points each) Please write your complete work in the space provided. Partial credit will be given. 1. The density of mercury, the only metal to exist as liquid at room temperature, is 13.6 g/cm 3. What is the density in pounds per cubic inch (lb/in 3 )? ( 1.00 lb = g, 1 in = 2.54 cm) 2. Lithium, is used in dry cells and storage batteries and in high temperature lubricants, it has two naturally occurring isotopes; 6 Li and 7 Li. Calculate the atomic mass of lithium. Isotope Mass (amu) Abundance (%) 6 Li Li A mixture of g of aluminum metal and g of O 2 is allowed to react. a) Identify the limiting reactant. b) Calculate the mass of aluminum oxide formed. c) Determine the mass of the excess reactant present in the vessel when the reaction is complete. d) What is the percentage yield for the reaction if reaction mixture produces 120 g of aluminum oxide? Practice Final, CHEM 1411 Page 6

7 4. For the electronic transition from n = 3 to n = 8 in the hydrogen atom, calculate a) the energy change, and b) the wavelength of light that corresponds to this energy. 5. Calculate the standard enthalpy change, H o, for the following gas phase reaction using bond energy data. Bond Dissociation Energies H H H H H-Cl 435 kj/mol \ C-H 413 kj/mol C=C + H-Cl H - C - C - H C-C 348 kj/mol \ C=C 614 kj/mol H H Cl H C-Cl 328 kj/mol 6. Draw the Lewis dot structure for the SO 3 2 ion and determine a) the electron domain geometry b) the molecular geometry c) the hybridization of the sulfur atom d) the approximate bond angles Practice Final, CHEM 1411 Page 7

8 Answers Part I - Multiple-Choice 1. B 11. C 21. C 31. A 2. C 12. A 22. B 32. D 3. D 13. D 23. C 33. C 4. A 14. D 24. B 34. C 5. B 15. C 25. D 35. C 6. D 16. C 26. A 7. B 17. D 27. C (K has a larger radius than Cl ) 8. C 18. B 28. B 9. D 19. C 29. D 10. D 20. B 30. B Part II - Show-Work g X cm 3 X 1 lb = lb/in 3 1 in g 2. (0.0750)( amu) + (0.9250)( amu) = amu amu = amu 3. The Fabulous Four Steps 1) Write the balanced chemical reaction. 4 Al (s) + 3 O 2 (g) > 2 Al 2 O 3 (s) 2) Calculate the moles of Given Substances. Moles of Al = g = mol g/mol Moles of O 2 = g = mol g/mol Practice Final, CHEM 1411 Page 8

9 3) Calculate the moles of Desired Substance (Al 2 O 3 ). a) moles of Al 2 O 3 = mol Al X 2 mol Al 2 O 3 = mol Al 2 O 3 based on Al 1 4 mol Al b) moles of Al 2 O 3 = mol O 2 X 2 mol Al 2 O 3 = mol Al 2 O 3 based on O mol O 2 Keep the smaller answer, mol of Al 2 O 3. The limiting reactant is therefore Al. 4) Convert your answer in Step 3 to the units asked for (grams). (1.527 mol)( g/mol) = g of Al 2 O 3 will be formed. Calculation of Excess Reactant that Remains (O 2 ) after the Reaction is Complete Moles of O 2 remaining = total moles of O 2 initially moles of O 2 reacted Total moles of O 2 initially present = mol Moles of O 2 that react with the limiting reactant (Al, mol) is mol Al X 3 mol O 2 = mol O mol Al Moles of O 2 remaining as unreacted excess = mol mol = mol Grams of O 2 remaining = ( mol)( g/mol) = g Percent Yield of Al 2 O 3 = 120 g X 100 = 77.1% g 4. a) E = (2.18 X J)(1/3 2 1/8 2 ) = 2.08 X J b) = hc = (6.63 X J s)(3.00 X 10 8 m/s) = 9.56 X 10 7 m or 956 nm E 2.08 X J 5. Bonds broken minus bonds formed: H = [ (1 mol)(614 kj/mol) + (1 mol)(435 kj/mol) ] [ (1 mol)(348 kj/mol) + (1 mol)(328 kj/mol) + (1 mol)(413 kj/mol) ] = 1049 kj 1098 kj = 40 kj Practice Final, CHEM 1411 Page 9

10 6. These illustrations of the sulfite ion are from an introduction to chemical bonding at Since there are a total of four atoms plus lone pairs (four electron domains ) around the central sulfur, the overall geometry is tetrahedral and the molecular geometry is trigonal pyramidal. The hybridization of the sulfur atom in the first structure is therefore sp 3. However, the sulfur is not simply sp 3 hybridized in the second structure, which has an expanded octet around the sulfur atom. Hybridizations that allow more than an octet of electrons around an atom are sp 3 d (10 electrons) and sp 3 d 2 (12 electrons), but not sp, sp 2, or sp 3. Furthermore, to form a -bond, we must have unhybridized p-orbitals on the sulfur and oxygen atoms. This p orbital will not be present if the hybridization is sp 3, sp 3 d, or sp 3 d 2. For simplicity, we can assign the hybridization of the sulfur as sp 3 based on the first structure, but in order to more accurately describe the bonding here and in other molecules with combinations of expanded octets and multiple bonds (double or triple bonds) in their dot structures, we must probably turn to molecular orbital theory. These illustrations are from the Wikipedia article for sulfites at A space-filling model of the sulfite anion The structure of the sulfite anion Practice Final, CHEM 1411 Page 10

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