New Material Sample Questions Fall 2023

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CHEM 1113 Sample New Material Questions Fall 2023 Chapter 9: Lattice Energy 1. Arrange the following solids in order of increasing lattice energy strength: MgI 2 , NaI, CaI 2 A. NaI < CaI 2 < MgI 2 B. NaI < MgI 2 < CaI 2 C. MgI 2 < CaI 2 < NaI D. NaI < CaI 2 ≈ MgI 2 Chapter 10: Covalent Bonding 2. Identify the best Lewis structure for COCl 2 . A B C D 3. Which of the following is the best Lewis structure of SPO - ? A. B. C. D. 4. Which of the following describes the best Lewis structure for ozone, O 3 ? A. Two single bonds and seven lone pairs of electrons B. One single bond, one double bond and six lone pairs of electrons C. Two single bonds and eight lone pairs of electrons D. Two double bonds and five lone pairs of electrons 5. Which statement is true about the Lewis structure shown for chlorate, ClO 3 − ? A. This structure is not an exception to the octet rule. B. The formal charge on the chlorine atom is −1. C. This is the best Lewis structure for ClO 3 − . D. The Cl−O bond order is 1⅓.
6. Which of these Lewis structures are incorrect? A. 1 and 2 are incorrect B. 2 and 3 are incorrect C. 1 and 3 are incorrect D. 1, 2 and 3 are incorrect 7. What is the formal charge on each element in the structure given below? P S Br A. 0 +1 0 B. +1 0 0 C. +1 +1 ‒1 D. 0 +2 ‒1 8. Which of the following species are exceptions to the octet rule? 1. BF 3 2. SF 4 3. PO A. 1 and 2 are exceptions. B. 1 and 3 are exceptions. C. 2 and 3 are exceptions. D. 1, 2 and 3 are exceptions. 9. Using the given electronegativities, which of these bonds is the most polar? A. O − Br B. C − O C. P − Cl D. N − S 10. Which of the following statements about the electronegativity scale is false? A. The smaller the atomic size of the element, the higher the electronegativity. B. A C‒Cl bond is less polar than a S‒O bond. C. The difference in electronegativity of the atoms determines if a bond is classified as covalent, polar covalent, and ionic. D. Ionic bonding occurs between atoms of similar electronegativity. 11. Select the false statement. A. A C−O bond is more polar than a N−O bond. B. In a C−Br bond, the negative end of the dipole is on the C. C. A C≡C bond is nonpolar covalent. D. CaCO 3 contains both ionic and covalent bonds. 1 2 3
12. Given the information in the table, which of the statements below are true? 1. X−A is a longer bond than X−B. 2. X−A is a weaker bond than X−C. 3. X−C is a shorter bond than X=C. A. Only 1 and 2 are true. B. Only 2 and 3 are true. C. Only 1 and 3 are true. D. 1, 2 and 3 are all true. 13. Choose the false statement. A. The greater the bond order, the stronger the bond. B. Breaking bonds is always an exothermic process. C. A Y=Y bond is always shorter than a Y−Y bond. D. An X−Cl bond is always stronger than an X−Br bond. 14. Using the bond energies given, calculate ΔH rxn for the balanced chemical equation below. A. 4345 kJ/mol B. 2351 kJ/mol C. -1207 kJ/mol D. 2245 kJ/mol 15. Using the bond energies given, calculate Δ H rxn for the balanced chemical equation below. A. −180 kJ/mol B. +1070 kJ/mol C. +1688 kJ/mol D. +3340 kJ/mol Chapter 11: Molecular Shape and Bonding Theories 16. In the best Lewis structure for ICl 4 – , what are the electron geometry and the molecular shape around the central iodine atom? A. Electron geometry : Tetrahedral & Molecular shape : Tetrahedral B. Electron geometry : Trigonal bipyramidal & Molecular shape : See-Saw C. Electron geometry : Octahedral & Molecular shape : Square pyramidal D. Electron geometry : Octahedral & Molecular shape : Square planar Bond Bond Length (pm) Bond Energy (kJ/mol) X-A 227 --- X-B --- 312 X-C 173 291 Bond Energy (kJ/mol) A-H 425 S=S 319 S-H 347 A=S 688 A-A 351 Bond Bond Energy (kJ/mol) C−O 358 C−H 413 H−H 432 O−H 467
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17. What are the bond angles indicated by α and β in the structure below? A. α = 90°, β = 180° B. α = 120°, β = <109.5° C. α = 120°, β = 180° D. α = 90°, β = <109.5° 18. What is the hybridization on the atoms labelled 1, 2, and 3? A. 1: sp 2 , 2: sp, 3: sp B. 1: sp 2 , 2: sp 3 , 3: sp 2 C. 1: sp 3 , 2: sp, 3: sp 2 D. 1: sp 3 , 2: sp 3 , 3: sp 3 19. Which of the following statements is true? A. A pi bond is formed when two half-filled sp 3 hybrid orbitals overlap. B. A nitrogen atom with sp hybridization must form a double bond. C. A sigma bond is formed when two half-filled unhybridized s orbitals overlap. D. A carbon atom with sp 2 hybridization can form a triple bond. Use the following structure to answer questions 20 - 22. 20. What hybridization is necessary on the carbon atom labeled α in the structure above? A. sp B. sp 2 C. sp 3 D. sp 3 d 21. What is the molecular geometry around the carbon atom labeled in the structure above? A. tetrahedral B. trigonal pyramidal C. trigonal planar D. bent 22. What is the approximate H – C – C bond angle labeled in the structure above? A. 90° B. 109.5° C. 120° D. 180° O H O || | || HO – C – CH 2 – C – CH 2 – C – OH | OH
23. Which of the following molecules contains polar bonds but is not a polar molecule? A. CH 2 Cl 2 B. SF 4 C. SiF 4 D. PF 3 24. How many and bonds are present in the structure for caffeine shown to the right? A. 25 , 4 B. 25 , 8 C. 21 , 4 D. 21 , 8 25. Which of the following contains dipole-dipole forces? I. SiH 4 II. H 2 O III. SBr 4 A. I & III B. I & II C. II & III D. 1, II and III 26. Which choice below has the greatest dispersion forces among its molecules? A. I B. III C. II ≈ III D. IV Chapter 12: Liquids and Solids 27. Which of the following pairs of compounds has the one with the greater boiling point written first? A. CH 4 CCl 4 B. C. D. CH 3 OCH 3 C 2 H 5 OH
28. Determine the amount of heat, in kJ, required to vaporize 1.55 kg of water at its boiling point. ΔH vap of water at 100°C is 40.7 kJ/mol. A. 3.50 × 10 3 kJ B. 1.14 × 10 6 kJ C. 2.11 kJ D. 686 kJ 29. Ethylene glycol (antifreeze, C 2 H 6 O 2 , MM = 62.07 g/mol), has a freezing point of −12.9°C. Calculate how much energy is released when 10.0 moles of 0.0°C liquid ethylene glycol is cooled to −12.9°C solid ethylene glycol. A. 99 kJ B. 2.0 x 10 4 kJ C. 6.2 x 10 3 kJ D. 120 kJ 30. The normal boiling point of Br 2 ( l ) is 332 K. At 283 K, the vapor pressure of Br 2 ( l ) is 0.144 atm. What is its enthalpy of vaporization? A. 22.3 kJ/mol B. 2.30 kJ/mol C. 30.9 kJ/mol D. 110. kJ/mol 31. In which of the following places would the boiling point of water be highest? A. In a pressure cooker where the pressure is about 1400 torr. B. In the city of New York where the pressure is about 760 torr. C. At the peak of Mt. Everest. D. In Boulder, Colorado. 32. Which type of intermolecular forces are present in all pure liquid substances? A. hydrogen-bonding B. dipole-dipole C. dispersion D. ion-dipole 33. What is the vapor pressure, in mmHg, of acetic acid at 25°C if it has a normal boiling point of 118 °C and a ΔH vap of 23.4 kJ/mol? A. 2.92 × 10 -39 mmHg B. 7.16 × 10 3 mmHg C. 758 mmHg D. 80.6 mmHg Specific heat capacity, C 2 H 6 O 2 (l) 2.46 J/(g∙K) Heat of fusion, C 2 H 6 O 2 9.9 kJ/mol
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Use the following phase diagram to answer questions 34 - 37. 34. Which of the arrows in the phase diagram represents condensation? A. A B. B C. C D. None of these 35. For this substance, what phase would be present at 1.0 atm and 380 K? A. solid B. liquid C. gas D. Cannot tell from the data given. 36. What phases are in equilibrium at point D? A. solid, liquid and gas B. only solid and gas C. only liquid and gas D. There are no phases in equilibrium at point D. 37. What is the normal boiling point of the substance? A. 273.2 K B. 373 K C. 273 K D. 647 K Chapter 13: Solutions 38. Choose the pair of compounds that are soluble in each other: I. CH 3 OCH 3 in H 2 O II. CH 3 OH in CH 2 Cl 2 III. CHCl 3 in NH 3 A. I, II, and III B. I and II C. II and III D. III only 39. For which of the following substances is carbon tetrachloride a better solvent in comparison to water? C 7 H 16 (heptane), NaHCO 3 , HCl, I 2 A. Only C 7 H 16 and I 2 B. Only HCl and NaHCO 3 C. Only I 2 D. Only C 7 H 16
40. In a 0.1 M solution of NaCl in water, which one of the following will be closest to 0.1? A. the mole fraction of NaCl. B. the weight percent of NaCl. C. the molality of NaCl. D. the mole fraction, weight percent and molality of NaCl are all about 0.1. 41. An aqueous solution containing 292.0 g of magnesium nitrate per liter solution has a density of 1.108 g/mL. What is the molality of this solution? A. 2.00 m B. 2.41 m C. 5.50 m D. 6.39 m 42. A potassium bromide solution is 7.55% KBr by mass and its density is 1.03 g/mL. What mass of KBr is contained in 35.8 mL of the solution? A. 2.78 g B. 2.70 g C. 4.88 g D. 2.62 g 43. The vapor pressure above a sugar-water solution at 25°C is 21.4 torr. What is the mole fraction of sugar in this solution? Data: sugar is a nonvolatile solute The vapor pressure of pure water at 25°C is 23.8 torr. A. 0.899 B. 0.101 C. 1.00 D. 0.500 44. A solution contains a mixture of two volatile substances A and B. The mole fraction of substance A is 0.35. At 32°C the vapor pressure of pure A is 87 mmHg and the vapor pressure of pure B is 122 mmHg. What is the total vapor pressure of the solution at this temperature? A. 110 mmHg B. 209 mmHg C. 99.3 mmHg D. 73.22 mmHg 45. What mass of glucose (C 6 H 12 O 6 ) should be dissolved in 10.0 kg of water to obtain a solution with a freezing point of – 4.2°C? K f (water) = 1.86 °C/m A. 0.023 kg B. 4.1 kg C. 0.41 kg D. 14.1 kg
46. Which aqueous solution has the highest boiling point? A. 1.25 M C 6 H 12 O 6 B. 1.25 M KNO 3 C. 1.25 M Ca(NO 3 ) 2 D. None of the above (they all have the same boiling point) 47. A cucumber is placed in a concentrated salt solution. What will most likely happen? A. Salt will precipitate out. B. Salt will flow into the cucumber. C. Water will flow from the solution to the cucumber. D. Water will flow from the cucumber to the solution. 48. A 5.00 g sample of an unknown compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 25 torr at 25.0 °C. Assuming that each solute molecule dissociates into two particles when dissolving in water, what is the molar mass of the solute? A. 1560 g/mol B. 18,600 g/mol C. 37,200 g/mol D. 74,400 g/mol 49. The freezing point of a 1.90 m aqueous electrolyte solution is −6.57 °C. What is the value of the van’t Hoff factor for this solution? For water: K f = 1.86°C/ m. A. 1.86 B. 0.283 C. 3.45 D. 0.537 50. Determine the freezing point of a 250. g benzene solution after dissolving 0.14 mol of a nonelectrolyte. For benzene: K f = 4.3°C/ m and the normal freezing point is 5.5 °C. A. 2.4 °C B. 3.1 °C C. 5.5 °C D. 7.9 °C
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