KEY-FinalExamStudyGuide_Fall2013

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Name ___________________________ Date ___________________ Class __________________ CHAPTER 8, Covalent Bonding (continued) Polar Molecules (pages 239–240) 9. Circle the letter of each sentence that is true about polar molecules. a. Some regions of a polar molecule are slightly negative and some are slightly positive. b. A molecule containing a polar bond is always polar. c. A molecule that has two poles is called a dipolar molecule. d. When polar molecules are placed in an electric field, they all line up with the same orientation in relation to the charged plates. 10. Are the following molecules polar or nonpolar? a. H 2 O ______________________ polar c. NH 3 ______________________ polar b. CO 2 ______________________ nonpolar d. HCl ______________________ polar Attractions Between Molecules (pages 240–241) 11. What causes dispersion? Dispersion forces are caused by the motion of electrons. 12. Is the following sentence true or false? Dispersion forces generally increase in strength as the number of electrons in a molecule increases. ___________________ true 13. The strongest of the intermolecular forces are ______________________ hydrogen bonds . Intermolecular Attractions and Molecular Properties (pages 243–244) 14. What determines the physical properties of a compound? The physical properties depend on the type of bonding in the compound. 15. Use Table 8.4 on page 244. Complete the following table comparing ionic and covalent compounds. Characteristic Ionic Compound Covalent Compound Representative unit Physical state Melting point Solubility in water formula unit solid high usually high molecule solid, liquid, or gas low high to low © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 76 Guided Reading and Study Workbook
Name ___________________________ Date ___________________ Class __________________ GUIDED PRACTICE PROBLEM GUIDED PRACTICE PROBLEM 19 (page 239) 19. Identify the bonds between atoms of each pair of elements as nonpolar covalent, moderately polar covalent, very polar covalent, or ionic. Analyze a. H and Br b. K and Cl c. C and O d. Br and Br Step 1. What is the most probable type of bond for each electronegativity difference range? Electronegativity Difference Range Most Probable Type of Bond 0.0–0.4 ________________________ nonpolar covalent __ 0.4–1.0 ________________________ moderately polar covalent __ 1.0–2.0 ________________________ very polar covalent __ 2.0 ________________________ ionic __ Calculate Step 2. From Table 6.2 on page 177, determine the electronegativity values and differences for each pair of elements. a. H 2.1, Br 2.8 ; difference 0.7 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. K 0.8 , Cl 3.0; difference c. C 2.5 , O 3.5; difference d. Br 2.8, Br 2.8 ; difference 0 Step 3. Refer to Table 8.3 on page 238 to determine the most probable type of bond for each compound. a. ______________________________ moderately polar covalent b. ______________________________ ionic c. ______________________________ very polar covalent d. ______________________________ nonpolar covalent Evaluate 2.2 Step 4. How do you know that your answers are correct? The answers are consistent with the magnitudes of the electronegativity differences. 1 Chapter 8 Covalent Bonding 77
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KEY-FinalExamStudyGuide_Fall2013

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