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T182 Chemistry: Matter and Change Name Date Class Name Date Class CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY Covalent Bonding Section 9.2 Naming Molecules In your textbook, read about how binary compounds and acids are named from their formulas. Section 9.1 The Covalent Bond For each statement below, write true or false. In your textbook, read about the nature of covalent bonds. false 1. Binary molecular compounds are generally composed of a metal and a nonmetal. Use each of the terms below just once to complete the passage. covalent bond molecule sigma bond exothermic pi bond false 2. The second element in the formula of a binary compound is named using the suffix -ite. When sharing of electrons occurs, the attachment between atoms that results is called false 3. The prefix tetra- indicates three atoms. a(n) (1) covalent bond . When such an attachment is formed, bond dissociation true 4. The prefix hexa- indicates six atoms. energy is released, and the process is (2) exothermic . When two or more true 5. In naming the first element in a formula, the prefix mono- is not used. atoms bond by means of electron sharing, the resulting particle is called a(n) true 6. For binary acids, the hydrogen part of the compound is named using the prefix hydro-. (3) molecule . If the electrons shared are centered between the two atoms, the attachment is called a(n) (4) sigma bond . If the sharing involves the overlap of false 7. An oxyacid contains only two elements. parallel orbitals, the attachment is called a(n) (5) pi bond . false 8. If the name of the anion of an oxyacid ends in -ate, the acid name contains the suffix -ous. In your textbook, read about single and multiple bonds and bond strength. In your textbook, read about naming molecular compounds and oxyacids. Circle the letter of the choice that best completes the statement or answers the question. For each item in Column A, write the letter of the matching item in Column B. 6. In what form do elements such as hydrogen, nitrogen, and oxygen normally occur? Column A Column BStudy Guide for Content Mastery Answer Key a. as single atoms c. as molecules containing three atoms c 9. CO a. hydrobromic acid b. as molecules containing two atoms d. as molecules containing four atoms 7. How many electrons are shared in a double covalent bond? i 10. CO2 b. dinitrogen tetroxide g 11. H2CO3 c. carbon monoxide a. none b. one c. two d. four e 12. NH3 d. nitrous acid b 13. N2O4 e. ammonia 8. Bond length is the distance between c. the nuclei of two attached atoms. d 14. HNO2 f. nitric acid a. two molecules of the same substance. d. the orbitals of two attached atoms. f 15. HNO3 g. carbonic acid b. the electrons in two attached atoms. a 16. HBr h. bromic acid 9. Which of the following relationships relating to bond length is generally correct? h 17. HBrO3 i. carbon dioxide a. the shorter the bond, the stronger the bond b. the shorter the bond, the weaker the bond c. the shorter the bond, the fewer the electrons in it d. the shorter the bond, the lower the bond dissociation energy Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 9 49 50 Chemistry: Matter and Change • Chapter 9 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.

Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.Study Guide for Content Mastery Answer Key Name Date Class Name Date Class CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY Section 9.3 Molecular Structures Section 9.4 Molecular Shape In your textbook, read about Lewis structures. In your textbook, read about the VSEPR model. For each statement below, write true or false. Circle the letter of the choice that best completes the statement. true 1. A structural formula shows the arrangement of the atoms in a molecule. 1. The VSEPR model is used mainly to a. determine molecular shape. false 2. The central atom in a molecule is the one with the highest electron b. write resonance structures. c. determine ionic charge. affinity. d. measure intermolecular distances. true 3. In molecules, hydrogen is always a terminal atom. 2. The bond angle is the angle between a. the sigma and pi bonds in a double bond. false 4. The number of bonding pairs in a molecule is equal to the number of b. the nucleus and the bonding electrons. c. two terminal atoms and the central atom. electrons. d. the orbitals of a bonding atom. false 5. To find the total number of electrons available for bonding in a positive 3. The VSEPR model is based on the idea that ion, you should add the ion charge to the total number of valence electrons a. there is always an octet of electrons around an atom in a molecule. of the atoms present. b. electrons are attracted to the nucleus. c. molecules repel one another. false 6. The electrons in a coordinate covalent bond are donated by both the d. shared and unshared electron pairs repel each other as much as possible. bonded atoms. true 7. Resonance occurs when more than one valid Lewis structure can be 4. The shape of a molecule whose central atom has four pairs of bonding electrons is written for a molecule. a. tetrahedral. b. trigonal planar. c. trigonal pyramidal. d. linear. true 8. Nitrate is an example of an ion that forms resonance structures. 5. The shape of a molecule that has two covalent single bonds and no lone pairs on the true 9. The carbon dioxide molecule contains two double bonds. central atom is false 10. All electrons in an atom are available for bonding. a. tetrahedral. b. trigonal planar. c. trigonal pyramidal. d. linear. true 11. In the sulfate ion (SO42Ϫ), 32 electrons are available for bonding. 6. The shape of a molecule that has three single covalent bonds and one lone pair on the false central atom is 12. When carbon and oxygen bond, the molecule contains ten pairs of bonding electrons. a. tetrahedral. b. trigonal planar. c. trigonal pyramidal. d. linear.Chemistry: Matter and Change T183 In your textbook, read about resonance structures and exceptions to the octet rule. In your textbook, read about hybridization. Use each of the terms below just once to complete the passage. For each item in Column A, write the letter of the matching item in Column B. Column A Column B carbon carbon dioxide hybridization sp3 identical methane sp phosphorus trihydride c 13. Odd number of valence electrons a. O3 b 14. Fewer than 8 electrons around an atom b. BF3 The formation of new orbitals from a combination or rearrangement of valence electrons d 15. More than 8 electrons around central atom c. NO is called (7) hybridization . The orbitals that are produced in this way are a 16. More than one valid Lewis structure d. SF6 (8) identical to one another. An example of an element that commonly undergoes such formation is (9) carbon . When this atom combines its three p orbitals and its one s orbital, the orbitals that result are called (10) sp3 orbitals. An example of a molecule that has this type of orbital is (11) methane . Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 9 51 52 Chemistry: Matter and Change • Chapter 9 Study Guide for Content Mastery

T184 Chemistry: Matter and Change Name Date Class Name Date Class CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY CHAPTER 9 STUDY GUIDE FOR CONTENT MASTERY Section 9.5 continued Section 9.5 Electronegativity and Polarity In your textbook, read about bond polarity. In your textbook, read about electronegativity. Using the table of electronegativities on the preceding page, circle the letter of the choice that best completes the statement or answers the question. Use the table of electronegativities below to answer the following questions. 1 Electronegativities of Some Elements 8. Unequal sharing of electrons between two bonded atoms always indicates H a. a nonpolar covalent bond. c. a polar covalent bond. 2.20 3 4 Metal 567 89 b. an ionic bond. d. a polar molecule. Li Be Metalloid BCNOF 0.98 1.57 2.04 2.55 3.04 3.44 3.98 9. When electronegativities of two bonded atoms differ greatly, the bond is 11 12 Nonmetal 13 14 15 16 17 Na Mg 0.93 1.31 Al Si P S Cl a. polar covalent. b. coordinate covalent. c. polar covalent. d. ionic. 1.61 1.90 2.19 2.58 3.16 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 10. What is the electronegativity difference that usually is the dividing line between covalent K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br and ionic bonds? 0.82 1.00 1.36 1.54 1.63 1.66 1.55 1.83 1.88 1.91 1.90 1.65 1.81 2.01 2.18 2.55 2.96 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 a. 1.0 b. 1.7 c. 2.7 d. 4.0 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I 0.82 0.95 1.22 1.33 1.6 2.16 2.10 2.2 2.28 2.20 1.93 1.69 1.78 1.96 2.05 2.1 2.66 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 11. The symbol ␦ϩ is placed next to which of the following? c. a positive ion Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At a. the less electronegative atom in a polar covalent bond d. the nucleus 0.79 0.89 1.10 1.3 1.5 1.7 1.9 2.2 2.2 2.2 2.4 1.9 1.8 1.8 1.9 2.0 2.2 b. the more electronegative atom in a polar covalent bond 87 88 89 Fr Ra Ac 0.7 0.9 1.1 1. What is the meaning of the term electronegativity? 12. A nonpolar covalent bond is one in which c. electrons are shared equally. the tendency of an atom to attract electrons a. electrons are transferred. d. both electrons are provided by the same atom. b. electrons are shared unequally. 2. Which element has the highest electronegativity? What is the numerical value? What are the 13. Molecules containing only polar covalent bonds c. are always ionic. name and group number of the chemical family that has the highest overall electronegativities? a. are always polar. d. are always nonpolar. b. may or may not be polar. fluorine; 3.98; halogens; group 7AStudy Guide for Content Mastery Answer Key 3. Which element has the lowest electronegativity? What is the numerical value? What are the 14. What factor other than electronegativity determines whether a molecule as a whole is name and group number of the chemical family that has the lowest overall electronegativities? polar or not? francium; 0.7; alkali metals; group 1A a. temperature b. its geometry c. its physical state d. its mass 4. What general trend in electronegativity do you note going down a group? Across a period? 15. Which of the following correctly describes the compound water, H2O? Electronegativity tends to decrease. Electronegativity tends to increase. a. ionic c. polar overall, with nonpolar covalent bonds b. nonpolar overall, with polar covalent bonds d. polar overall, with polar covalent bonds 5. How are the electronegativity values used to determine the type of bond that exists 16. Which of the following correctly describes the compound carbon tetrachloride, CCl4? between two atoms? a. ionic c. polar overall, with nonpolar covalent bonds The values are subtracted. b. nonpolar overall, with polar covalent bonds d. polar overall, with polar covalent bonds In your textbook, read about the properties of covalent compounds. 17. A molecule of ammonia, NH3, is a. nonpolar because it is linear. For each statement below, write true or false. b. polar because it is linear. c. nonpolar because there is no electronegativity difference. true 6. Ionic compounds are usually soluble in polar substances. d. polar because there is an electronegativity difference and the molecule is trigonal pyramidal. false 7. In a covalent molecular compound, the attraction between molecules tends to be strong. Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 9 53 54 Chemistry: Matter and Change • Chapter 9 Study Guide for Content Mastery Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.