1. Chapter 6 Review

2. 1. What intermolecular forces predominate when rubbing alcohol (CH 3 CHOHCH 3 ) and water are mixed? a.hydrogen bonding b.induced dipole attractions c.Van der Waals attractions d.London dispersion forces

3. 2. At room temperature water is a liquid, while carbon dioxide is a gas, and sodium chloride is a solid. Which of the following is the best explanation for this observation? a.water is the lightest substance and sodium chloride is the heaviest b.attractive forces between particles is greatest in sodium chloride and weakest in carbon dioxide c.carbon dioxide contains oxygen and oxygen is a gas at room temperature d.sodium chloride contains a metal while water and carbon dioxide do not

4. 3. Which of the following form hydrogen bonds? a.H 2 b.Cl 2 c.both of the above d.neither of the above

5. 4. Put the following substances in order from weakest attractive forces to strongest attractive forces. Sodium chloride, carbon monoxide, drinking water a.sodium choride, carbon monoxide, drinking water b.carbon monoxide, sodium chloride, drinking water c.sodium chloride, drinking water, carbon monoxide d.carbon monoxide, drinking water, sodium chloride

6. 5. Which of the following tables is accurate? a.Ionic: High melting point High conductivity High hardness Covalent: Low melting point Low conductivity Low hardness b.Ionic: Low melting point High conductivity High hardness Covalent: High melting point Low conductivity Low hardness c.Ionic: High melting point Low conductivity Low hardness Covalent: Low melting point High conductivity High hardness d.Ionic: Low melting point Low conductivity Low hardness Covalent: High melting point High conductivity High hardness

7. 6. The melting point of a compound is 1200°C. The compound is most likely a(n) a.ionic compound b.covalent compound c.catatonic compound d.noble gas

8. 7. Which molecule will not undergo hydrogen bonding? a.HF b.NH 3 c.H 2 O d.CH 4

9. 8. Which combination of atoms can form a polar covalent bond? a.H and H b.N and N c.H and Br d.Na and Br

10. 9. Which of the following would you expect to have the highest boiling point? a.fluorine b.bromine c.chlorine d.iodine

11. 10. What type of intermolecular forces are represented by the diagram below? a.dipole-dipole forces b.ionic bonding c.London dispersion forces d.hydrogen bonding 1.What type of intermolecular forces are represented by the diagram below? dipole-dipole forces ionic bonding London dispersion forces hydrogen bonding

12. 11. What type of intermolecular forces are represented by the diagram below? a.dipole-dipole forces b.ionic bonding c.London dispersion forces d.hydrogen bonding

13. 12. What type of intermolecular forces are represented by the diagram below? a.dipole-dipole forces b.ionic bonding c.London dispersion forces d.hydrogen bonding

14. 13. What type of intermolecular forces are represented by the diagram below? a.dipole-dipole forces b.ionic bonding c.London dispersion forces d.hydrogen bonding

15. 14. The melting and boiling points for water are significantly higher than other small molecules of similar mass, such as methane (CH 4 ). Which of the following forces is stronger in water than in the other substances and is therefore responsible for this observation? a.London dispersion forces b.covalent bonds c.dipole-dipole forces d.hydrogen bonds

16. 15. Which of the following elements would have the greatest force of attraction between like molecules? a.O 2 b.I 2 c.H 2 d.N 2

17. 16. Based on the strength of intermolecular forces, which of the following covalent compounds would be expected to have the highest melting point? a.H 2 O b.CO 2 c.SO 2 d.CH 4

18. 17. Attractive forces that exist between particles are called what? a.intermolecular forces b.intramolecular forces c.heteromolecular forces d.intravenous-molecular forces

19. 18. What takes place within the electron cloud of an atom? a.Electrons acquire positive charge. b.Electrons acquire negative charge. c.Electrons are fixed in positions. d.Electrons are in constant motion.

20. 19. How is an induced dipole created? a.by an electron positioning next to it b.by an electron inversion near it c.by dipoles placed on both sides of it d.by the presence of a dipole next to it

21. 20. Polarizability is defined how? a.by how easily an atom changes shape and charge b.by how deformable an atomic nucleus is c.by how deformable an electron cloud is d.by how easily an electron changes shape and charge

22. 21. What does the following say about the polarizability of the anions of the following compounds: F 2, Cl 2, Br 2 —that as their mass increases, their melting point increases? a.Polarizability decreases with decreasing mass in a column of the periodic table. b.Polarizability increases with decreasing mass in a column of the periodic table. c.Polarizability decreases with increasing mass in a column of the periodic table. d.Polarizability increases with increasing mass in a column of the periodic table.

23. 22. Which is the correct order of polarizability for the following, from least to most? a.H 2 S, H 2 O, H 2 Se b.H 2 Se, H 2 O, H 2 S c.H 2 O, H 2 Se, H 2 S d.H 2 O, H 2 S, H 2 Se

24. 23. How would the following—HCl, HF, and HBr—be ranked from least to most polarizable? a.HCl, HF, HBr b.HF, HCl, HBr c.HF, HBr, HCl d.HBr, HCl, HF

25. 24. How would the following, Ne, Kr, Ar, He, be ordered from lowest to highest melting point? a.He, Ne, Ar, Kr b.Kr, He, Ar, Ne c.He, Ar, Ne, Kr d.Kr, Ar, Ne, He

26. 25. To what is the positive region of a polar molecule attracted? a.a magnet b.the positive region of a neighboring molecule c.the negative region of a neighboring molecule d.to a non-polar molecule, thus inducing a dipole

27. 26. Which bond would have the greatest dipole? a.Si-H b.H-H c.O-H d.Br-H

28. 27. Which of the following would have no dipole? a.H-H b.H-F c.H-C d.H-Cl

29. 28. Which of the following will form hydrogen bonds? a.methanol, CH 3 OH b.water, H 2 O c.neither of the above d.both of the above