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

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   

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