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1. Standardized Test Preparation Chapter 6 Preview Multiple Choice Short Answer Extended Response

2. Standardized Test Preparation Chapter 6 Multiple Choice • 1. A chemical bond results from the mutual attraction of the nuclei for • A.electrons. • B. neutrons. • C. protons. • D. dipoles.

3. Standardized Test Preparation Chapter 6 Multiple Choice • 1. A chemical bond results from the mutual attraction of the nuclei for • A.electrons. • B. neutrons. • C.protons. • D.dipoles.

4. Standardized Test Preparation Chapter 6 Multiple Choice • 2. A polar covalent bond is likely to form between two atoms that • A. are similar in electronegativity. • B.are of similar size. • C. differ in electronegativity. • D. have the same number of electrons.

5. Standardized Test Preparation Chapter 6 Multiple Choice • 2. A polar covalent bond is likely to form between two atoms that • A. are similar in electronegativity. • B. are of similar size. • C. differ in electronegativity. • D. have the same number of electrons.

6. Standardized Test Preparation Chapter 6 Multiple Choice • 3. The Lewis structure of HCN contains • A. one double bond and one single bond. • B. one triple bond and one single bond. • C. two single bonds. • D. two double bonds.

7. Standardized Test Preparation Chapter 6 Multiple Choice • 3. The Lewis structure of HCN contains • A. one double bond and one single bond. • B.one triple bond and one single bond. • C.two single bonds. • D.two double bonds.

8. Standardized Test Preparation Chapter 6 Multiple Choice • 4. According to VSEPR theory, the molecular geometry for is • A. tetrahedral. • B.trigonal-pyramidal. • C.bent or angular. • D. None of the above

9. Standardized Test Preparation Chapter 6 Multiple Choice • 4. According to VSEPR theory, the molecular geometry for is • A.tetrahedral. • B.trigonal-pyramidal. • C.bent or angular. • D.None of the above

10. Standardized Test Preparation Chapter 6 Multiple Choice • 5. Which molecule contains a double bond? • A. COCl2 • B.C2H6 • C.CF4 • D.SF2

11. Standardized Test Preparation Chapter 6 Multiple Choice • 5. Which molecule contains a double bond? • A.COCl2 • B.C2H6 • C.CF4 • D. SF2

12. Standardized Test Preparation Chapter 6 Multiple Choice • 6. Which molecule is polar? • A.CCl4 • B.CO2 • C.SO3 • D.none of these

13. Standardized Test Preparation Chapter 6 Multiple Choice • 6. Which molecule is polar? • A.CCl4 • B.CO2 • C.SO3 • D. none of these

14. Standardized Test Preparation Chapter 6 Multiple Choice • 7. What is the hybridization of the carbon atoms in C2H2? • A. sp • B. sp2 • C. sp3 • D.The carbon atoms do not hybridize in C2H2.

15. Standardized Test Preparation Chapter 6 Multiple Choice • 7. What is the hybridization of the carbon atoms in C2H2? • A.sp • B.sp2 • C.sp3 • D.The carbon atoms do not hybridize in C2H2.

16. Standardized Test Preparation Chapter 6 Multiple Choice • 8. Which of the following compounds is predicted to have the highest boiling point? • A.HCl • B. CH3COOH (Note: the two oxygen atoms bond to the carbon) • C.Cl2 • D. SO2

17. Standardized Test Preparation Chapter 6 Multiple Choice • 8. Which of the following compounds is predicted to have the highest boiling point? • A. HCl • B. CH3COOH (Note: the two oxygen atoms bond to the carbon) • C.Cl2 • D. SO2

18. Standardized Test Preparation Chapter 6 Multiple Choice • 9. An unknown substance is an excellent electrical conductor in the solid state and is malleable. What type of chemical bonding does this substance exhibit? • A.ionic bonding • B.molecular bonding • C.metallic bonding • D.cannot determine from the information given

19. Standardized Test Preparation Chapter 6 Multiple Choice • 9. An unknown substance is an excellent electrical conductor in the solid state and is malleable. What type of chemical bonding does this substance exhibit? • A. ionic bonding • B.molecular bonding • C.metallic bonding • D.cannot determine from the information given

20. Standardized Test Preparation Chapter 6 Short Answer • 10. What does the hybridization model help explain?

21. Standardized Test Preparation Chapter 6 Short Answer • 10. What does the hybridization model help explain? • Answer: Hybridization explains how the orbitals of an atom become rearranged when the atom forms covalent bonds.

22. Standardized Test Preparation Chapter 6 Short Answer • 11. Explain why ionic crystals are brittle.

23. Standardized Test Preparation Chapter 6 Short Answer • 11. Explain why ionic crystals are brittle. • Answer: Ionic crystals are brittle because shifting of the layers of ions results in large repulsive forces that cause the layers to part completely.

24. Standardized Test Preparation Chapter 6 Extended Response • 12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and has a boiling point of 118°C. Which substance has the stronger intermolecular forces? Briefly explain your answer.

25. Standardized Test Preparation Chapter 6 Extended Response • 12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and has a boiling point of 118°C. Which substance has the stronger intermolecular forces? Briefly explain your answer. • Answer:Naphthalene has the stronger intermolecular forces even though it is nonpolar, because its boiling point is higher than that of acetic acid. Boiling point is directly correlated to strength of intermolecular forces; the stronger the intermolecular forces, the more energy needed to break all the intermolecular forces, and therefore the higher the boiling point. Naphthalene is so large that its dispersion forces are greater than the sum of the dispersion forces and hydrogen bonding in acetic acid.

26. Standardized Test Preparation Chapter 6 Extended Response • 13. Describe and explain the potential energy changes that occur during the formation of a covalent bond.

27. Standardized Test Preparation Chapter 6 Extended Response • 13. Describe and explain the potential energy changes that occur during the formation of a covalent bond. • Answer: There is a repulsive region at small bond distances, a minimum well at an intermediate bond distance, and an asymptotic region at large bond distances. The repulsive region is due to the repulsion between the two positive nuclei at distances where the nuclei are close to each other. The asymptotic region is where the atoms are far apart and therefore do not interact with each other. The potential energy decreases as the atoms come closer together and are attracted to each other. The minimum well is the region where the attractive forces are balanced by the repulsive forces. This distance is the equilibrium bond length.