CHEMISTRY Practice Exam #5 - SPRING 2014 (KATZ)

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1 CHEMISTRY Practice Exam #5 - SPRING 2014 (KATZ) Name: Score: This is a multiple choice exam. Choose the BEST answer from the choices which are given and write the letter for your choice in the space provided. All questions are equally weighted. Any specific reasoning or notes which lead to your answer may be included in the space provided. 1. Which of the following contains ionic bonding? A) CO B) SrF2 C) Al D) OCl2 2. Which of the following contains covalent bonds? A) BaO B) CsCl C) ClF D) Cu 3. Which of the following represents the Lewis structure for N? A) B) C) D) 4. Which of the following statements is TRUE? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Solid ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity 5. Determine the chemical formula for the compound formed between Ca and N. A) Ca2N3 B) Ca3N2 C) CaN2 D) CaN 6. Which of the following reactions is associated with the lattice energy of Li2O (ΔH latt)? A) Li2O(s) 2 Li+(g) + O2 (g) B) 2 Li+(aq) + O2 (aq) Li2O(s) C) 2 Li+(g) + O2 (g) Li2O(s) D) Li2O(s) 2 Li+(aq) + O2 (aq) 7. Identify the compound with the highest magnitude of lattice energy. A) NaCl B) KCl C) LiCl D) CsCl

2 8. Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS A) CaS < MgO < LiI B) LiI < CaS < MgO C) MgO < CaS < LiI D) LiI < MgO < CaS 9. A triple covalent bond contains of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs 10. Identify the number of bonding pairs and lone pairs of electrons in water. A) 1 bonding pair and 1 lone pair B) 1 bonding pair and 2 lone pairs C) 2 bonding pairs and 2 lone pairs D) 2 bonding pairs and 1 lone pair 11. Place the following elements in order of increasing electronegativity. Sr N Na A) Sr < Na < N B) Na < N < Sr C) Sr < N < Na D) N < Sr < Na 12. Which molecule or compound below contains an ionic bond? A) CO2 B) NH4NO3 C) SiF4 D) OCl2 13. Arrange aluminum, nitrogen, phosphorus and indium in order of increasing electronegativity. A) Al < In < N < P B) Al < In < P < N C) In < Al < P < N D) In < P < Al < N

3 14. Choose the best Lewis structure for XeI2. A) B) C) D) 15. Choose the best Lewis structure for NO3. A) B) C) D) 16. Using Lewis structures and formal charge, which of the following ions is most stable? OCN ONC NOC A) OCN " B) ONC " C) NOC D) None of these ions are stable according to Lewis theory 17. Use the bond energies provided to estimate ΔH rxn for the reaction below. XeF2 + 2 F2 XeF6 ΔH rxn =? Bond Bond Energy (kj/mol) Xe-F 147 F-F 159 A) -429 kj B) +159 kj C) -270 kj D) +176 kj

4 18. Which ionic compound would be expected to have the highest lattice energy? A) Rb2O B) SrO C) In2O3 D) CO2 19. Of the following elements, which has the highest electronegativity? A) S B) Cl C) Ti D) Se 20. Select the Lewis structure in which formal charges are minimized for the periodate anion, IO Determine the electron geometry (eg) and molecular geometry (mg) of CH3 +1. A) eg=tetrahedral, mg=tetrahedral B) eg=tetrahedral, mg=trigonal pyramidal C) eg=trigonal planar, mg=bent D) eg=trigonal planar, mg=trigonal planar 22. Determine the electron geometry (eg) and molecular geometry (mg) of NCl3. A) eg=tetrahedral, mg=tetrahedral B) eg=linear, mg=trigonal planar C) eg=trigonal planar, mg=bent D) eg=tetrahedral, mg=trigonal pyramidal 23. Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons. A) C1 = tetrahedral, C2 = linear B) C1 = trigonal planar, C2= bent C) C1 = bent, C2 = trigonal planar D) C1 = trigonal planar, C2 = tetrahedral

5 24. What is the molecular shape of ClO3F as predicted by the VSEPR theory? (Chlorine is the central atom.) A) trigonal pyramidal B) square planar C) square pyramidal D) tetrahedral 25. Determine the electron geometry (eg) and molecular geometry (mg) of IF2 -. A) eg=tetrahedral, mg=bent B) eg=trigonal planar, mg=bent C) eg=trigonal planar, mg=linear D) eg=trigonal bipyramidal, mg=linear 26. Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2 A) NCl3 > NO2 > N2O B) NO2 > N2O > NCl3 C) N2O > NO2 > NCl3 D) NCl3 > N2O > NO2 27. Which of the following molecules has a net dipole moment? A) BeCl2 B) SF2 C) KrF2 D) CO2 28. Describe a pi bond. A) side by side overlap of p orbitals B) end to end overlap of p orbitals C) s orbital overlapping with the end of a p orbital D) overlap of two s orbitals 29 A molecule containing a central atom with sp hybridization has geometry. A) linear B) trigonal bipyramidal C) trigonal planar D) tetrahedral

6 30. List the number of sigma bonds and pi bonds in a double bond. A) 1 sigma, 1 pi B) 2 sigma, 1 pi C) 2 sigma, 2 pi D) 1 sigma, 2 pi 31. How many of the following molecules contain at least one pi bond? C2H6 Cl2CO C2Cl4 SeS3 A) 0 B) 1 C) 3 D) Which one of the following statements about orbital hybridization is incorrect? A) The carbon atom in CH4 is sp 3 hybridized B) sp hybrid orbitals lie at 180 to each other. C) The nitrogen atom in NH3 is sp 2 hybridized D) sp 2 hybrid orbitals are coplanar, and at 120 to each other. 33. According to valence bond theory, the triple bond in ethyne (acetylene, C2H2) consists of A) three σ bonds and no π bonds. B) one σ bond and two π bonds C) two σ bonds and one π bond. D) no σ bonds and three π bonds. 34. What is the O-S-O bond angle in SO3 2-? A) less than B) C) 120 D) greater than Determine the shape (geometry) of PCl3 and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.) A) sp B) sp 2 C) sp 3 D) sp 3 d 36. Give the change in conditions to go from a liquid to a gas. A) increase heat or reduce pressure B) increase heat or increase pressure C) cool or reduce pressure D) cool or increase pressure

7 37. What is the strongest type of intermolecular force acting between molecules of H2? A) ion-dipole B) dipole-dipole C) dispersion D) hydrogen bonding 38. Place the following compounds in order of increasing strength of intermolecular forces. A) NH2CH3 < CO2 < F2 B) F2 < NH2CH3 < CO2 C) NH2CH3 < F2 < CO2 D) F2 < CO2 < NH2CH3 CO2 F2 NH2CH3 39. Place the following substances in order of increasing boiling point. CH3CH2OH He CH3OCH3 A) He < CH3OCH3 < CH3CH2OH B) CH3CH2OH < He < CH3OCH3 C) CH3CH2OH < CH3OCH3 < He D) CH3OCH3 < He < CH3CH2OH 40. Which is expected to have the highest magnitude of dispersion forces between molecules? A) C3H8 B) C12H26 C) F2 D) Be Cl2 41. The heat of vaporization of water at 100 C is kj/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 C. " A) 20.3 kj of heat are absorbed. B) 20.3 kj of heat are released. C) 81.3 kj of heat are absorbed. D) 81.3 kj of heat are released. 42. Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0 C to gaseous CCl4 at 76.8 C (the normal boiling point for CCl4). The specific heat of CCl4(l) is J/(g C), its heat of fusion is 3.27 kj/mol, and its heat of vaporization is kj/mol. A) kj B) 1.43 kj C) 5.74 kj D) 6.28 kj

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