CH 101 Exam 4 Spring 2012

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Chemistry

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Dec 6, 2023

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CH 101 Ellis Exam 4 Name _______________________________________________ MC 22 needs benzene resonance structures and MC 25-29 need glycine. The Periodic Table, Table 10.1 and Table 4.1 will be provided by your instructor at the beginning of the exam. Multiple Choice Questions. Each one is worth 1.5 points, 84 points total. 1. Elemental diatomic chlorine is a __________ molecule. a. polar covalent b. metalloid c. metallic d. ionic e. nonpolar covalent 2. The symbol for the element with the atomic number Z = 20 is __________. a. K b. Ca c. Ne d. Ar e. Na 3. Using the VSEPR model, predict the molecular geometry of SiF 4 . a. linear b. bent c. trigonal planar d. tetrahedral e. trigonal pyramidal 4. The charge on the sulfur in iron (III) sulfide is __________. a. +3 b. +2 c. +1 d. -1 e. -2 5. How many hybrid orbitals will the central atom in H 2 O have? a. 1 b. 2 c. 3 d. 4 e. 5 6. The strongest bonds are __________. a. metallic b. ionic c. covalent d. hydrogen e. none of the above 7. The angular momentum quantum number for the last electron in potassium is __________ . a. 0 b. 1 c. 2 d. 3 e. 4 8. The value of m s for the last electron in sodium would be ______________ . a. 0 b. 1 c. 2 d. 3 e. none of these 9. What is the oxidation number of nitrogen in NH 4 Cl? a. +2 b. +3 c. +4 d. -2 e. -3 10. ∆H is equal to __________. a. a bomb calorimeter b. the heat at constant pressure c. specific heat capacity d. potential energy e. thermal equilibrium 11. The principal quantum number for the last electron in argon is __________ . a. 0 b. 1 c. 2 d. 3 e. 4 12. A molecular bond has 12 bonding electrons and 8 antibonding electrons. Its bond order is ___________. a. zero b. one c. two d. three` e. four 13. The bonds in __________ are the weakest. a. oxygen b. ozone c. carbon dioxide d. nitrogen 14. MgCl 2 is held together by a(n) __________. a. sigma bond b. metallic bond c. pi bond d. covalent bond e. ionic bond 15. Which of the following molecules has the shortest and strongest bond? a. carbon dioxide b. chlorine c. nitrogen d. oxygen e. hydrogen

16. According to molecular orbital theory, He 2 does not form because it has ___________. a. equal numbers of sigma and pi molecular orbitals b. equal numbers of bonding and antibonding electrons c. filled all surrounding regions of space with its lone pairs of electrons d. filled p orbitals but not s orbitals e. completed its orbitals with electronegative atoms 17. What is the approximate bond angle in NH 3 ? a. 90 b. 109.5 c. 120 d. 180 18. Soap mixes well with both grease and water because soap is composed of __________ sections. a. polar b. nonpolar c. both of these d. neither of these 19. The number of sigma bonds in ethyne (C 2 H 2, skeletal structure is HCCH) is __________. a. two b. three c. four d. five e. six 20. Use the VSEPR model to predict the molecular geometry of PH 3 . a. linear b. trigonal pyramidal c. trigonal planar d. bent e. tetrahedral 21. Which of the following hybridization schemes allows the formation of two π bonds? a. sp b. sp 2 c. sp 3 d. sp 3 d e. sp 3 d 2 22. The diagram to the side depicts _________. a. triple bonds b. ionic metals Benzene Resonance here c. coordinate covalent bonds d. molecules with dipole moments e. resonance structures 23. Which of these best describes the bond between C and Cl? a. ionic b. nonpolar covalent c. polar covalent d. metallic e. none of these 24. How many neutrons are in P-32? a. 15 b. 16 c. 17 d. 31 e. 32 Consider the amino acid glycine, shown to the right, Glycine here for multiple choice questions 25-29. 25. The hybridization of atom a is ___________. a. sp b. sp 2 c. sp 3 d. sp 3 d e. sp 3 d 2 26. The electron geometry of atom b is ___________. a. linear b. trigonal pyramidal c. trigonal planar d. bent e. tetrahedral 27. The hybridization of atom c is __________. a. sp b. sp 2 c. sp 3 d. sp 3 d e. sp 3 d 2 28. The molecular geometry of atom d is ___________. a. linear b. trigonal pyramidal c. trigonal planar d. bent e. tetrahedral 29. Glycine contains __________ π bonds. a. 1 b. 2 c. 3 d. 4 e. 5

30. Protease inhibitors have been developed in attempts to stop the development of __________ . a. tuberculosis b. rabies c. polio d. AIDS e. MRSA 31. The ___________ molecule is crucial for absorbing harmful UV radiation in the atmosphere. a. oxygen b. ozone c. carbon dioxide d. nitrogen 98 32. How many electrons are in Tc ? 43 a. 43 b. 98 c. 55 d. 141 e. can not be determined 33. The electron sea model for metallic bonding accounts for all of the following except__________. a. ductility b. malleability c. polar covalent bonds d. ability to conduct electricity e. ability to conduct heat 34. Mass = 1 amu, charge = +1. a. Electron b. Proton c. Anion d. Neutron e. Isotope 35. To which period does zinc belong? a. 1 b. 2 c. 3 d. 4 e. 5 36. Which of the following is the net ionic reaction for ammonium sulfate and cobalt (II) acetate? a. ammonium ion plus sulfate yields ammonium sulfate b. ammonium ion plus acetate yields ammonium acetate c. cobalt ion plus sulfate yields cobalt (II) sulfate d. cobalt ion plus acetate yields cobalt (II) acetate e. there is no precipitation reaction 37. Sodium sulfate contains __________ oxygens. a. one b. two c. three d. four e. five 38. Which of these best describes the bond between Sr and O? a. ionic b. nonpolar covalent c. polar covalent d. metallic e. none of these 39. Which of the following best describes the bonds in mononitrogen dioxide? a. ionic b. metallic c. hydrogen d. covalent e. none of these 40. A molecule with the formula DR 3 has the molecular geometry of trigonal pyramidal. How many electron groups are around the central atom? a. two b. three c. four d. five e. six 41. In the combustion reaction between methane (CH 4 , found in natural gas) and oxygen to yield carbon dioxide and water, which of the following will have a coefficient of 2? a. methane and oxygen b. oxygen and water c. carbon dioxide and methane d. water e. all reactants and products have a coefficient of one 42. H 2 SO 4 is ___________ electrolyte. a. a strong b. a weak c. not an 43. Elemental sodium is held together by a(n) __________. a. sigma bond b. metallic bond c. pi bond d. covalent bond e. ionic bond

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