Chapter 9 Chemical Bonding: General Concepts
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1 Chapter 9 Chemical Bonding: General Concepts Multiple Choice Section Sodium tends to form ions which have the electronic configuration of a noble gas. What is the electronic configuration of the noble gas which the sodium ion mimics? a. 1s 2 b. 1s 2 2p 6! c. 1s 2 2s 2 2p 6 d. 1s 2 2s 2 2p 6 3s 2 e. 1s 2 2s 2 2p 6 3s 2 3p 6 Section Bromine tends to form simple ions which have the electronic configuration of a noble gas. What is the electronic configuration of the noble gas which the bromide ion mimics? a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4p 6 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4p 6 4d 10 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 6! d. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 e. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d The atoms in the nitrogen molecule, N 2, are held together by a. a single covalent bond b. a double covalent bond! c. a triple covalent bond d. an ionic bond e. a magnetic dipole bond 17. The atoms in the oxygen molecule, O 2, are held together by a. a single covalent bond! b. a double covalent bond c. a triple covalent bond d. an ionic bond e. a magnetic dipole bond 18. The atoms in the hydrogen fluoride molecule are held together by! a. a single covalent bond b. a double covalent bond c. a triple covalent bond d. an ionic bond 187
2 e. a magnetic dipole bond 19. The Lewis symbol for the carbon atom shows valence electrons. The number of bonds which carbon usually forms in order to complete its valence shell and obey the octet rule is a. 4, 1 b. 4, 2 c. 2, 4 d. 4, 3! e. 4, The Lewis symbol for the nitrogen atom shows valence electrons. The number of bonds which nitrogen usually forms in order to complete its valence shell and obey the octet rule is. a. 5, 1 b. 5, 2 c. 3, 4! d. 5, 3 e. 5, Complete the Lewis structure for HClO 3 from the skeletal template presented below by filling in the bonds and the remaining valence electrons (those which are not in the bonds). If the valence shells are filled to the usual limit (maximum of 8), what is the sum of the absolute values of all the formal charges in the molecule? a. 0 b. 1 c. 2 d. 3! e. 4 O H O Cl O 29. The compound shown immediately below is an example of H O H H C C C H 188
3 ! b. a ketone c. an acid d. a hydrocarbon e. an amine 30. The compound shown immediately below is an example of H O H C C C C H H b. an acid c. an amine! d. a ketone e. a hydrocarbon 31. The compound shown immediately below is an example of b. a ketone! c. an aldehyde d. an acid e. an amine O H C C C H 33. The compound shown immediately below is an example of b. a ketone c. an aldehyde d. an acid! e. an amine H H C C N H 189
4 34. The compound shown immediately below is an example of a. an acid b. an alcohol c. an aldehyde! d. an amine e. a ketone H C C C N H H 35. The compound shown immediately below is an example of! b. a ketone c. an aldehyde d. an acid e. an amine H C C O H 37. The compound shown immediately below is an example of b. a ketone c. an aldehyde! d. an acid e. an amine O H C C C O H Section Which one of the following bonds is the most polar one of the set? 190
5 a. H Br b. H Cl! c. H F d. H I e. H N Section Which one of the following is the least electronegative element of the set presented? a. F b. N c. C d. O! e. H Section Which one of the following is the least electronegative element of the set presented? a. N b. O c. Cl d. Br! e. I Section Based on electronegativity considerations, which one of the following listed species should be the strongest oxidizing agent? a. Ne b. Kr c. Br 2! d. Cl 2 e. S Section The formal charge on the oxygen atom in the carbon monoxide molecule is a. -2 b. -1 c. 0! d. +1 e The formal charge on the carbon atom in the carbonate ion is 191
6 a. -2! b. 0 c. +1 d. +2 e. +4 Section Complete the Lewis structure for HClO 3 from the skeletal template presented below by filling in the bonds and the remaining valence electrons (those which are not in the bonds). If the valence shells are filled to the usual limit (maximum of 8), what is the formal charge on the chlorine atom? a. -1 b. 0 c. +1! d. +2 e. +3 O H O Cl O 192
7 Section A student drew four possible Lewis structures for HBrO 4 A. O B. O C. O D. O H O Br O H O Br O H O Br O H O Br O O O O O Complete these Lewis structures presented above by filling in the remaining valence electrons (those which are not in the bonds). Based on these structures, the preferred structure would be the structure shown as in which the sum of the absolute values of the formal charges on all the atoms is, a. A, 4 b. B, 2! c. C, 0 d. D, 6 e. D, 0 Section Draw a correct Lewis structure for CH 2 Cl 2. Based on this Lewis structure, the calculated value for the formal charge on the carbon atom is! a. 0 b. +4 c. +2 d. -2 e. -4 Section Draw a correct Lewis structure for H 3 C NH 2. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is a. -2 b. +3 c. -3 d. +2! e
8 Section How many resonance structures, if any, can be drawn for the O 3 molecule? a. 1 (no resonance)! b. 2 c. 3 d. 4 e. 5 Section How many resonance structures, if any, can be drawn for the nitrate ion? a. 1 (no resonance) b. 2! c. 3 d. 4 e. 5 Section How many resonance structures, if any, can be drawn for the BF 3 molecule?! a. 1 (no resonance) b. 2 c. 3 d. 4 e
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