CH31CC~1 - CHAPTERS 22 CHEM 162-2011 Some PRACTICE PROBLEMS...

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CHAPTERS 22 CHEM 162-2011 Some PRACTICE PROBLEMS CHAPTER 22 - TRANSITION METALS AND COORDINATION CHEMISTRY COORDINATION COMPOUNDS E. Tavss, PhD 1
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CHAPTER 21 - TRANSITION METALS AND COORDINATION CHEMISTRY 1 Chem 162-2007 Final exam + answers Chapter 22 – Transition Metals and Coordination Chemistry Coordination Compounds How many of the following compounds exhibit geometric isomers? I. Pt(NH 3 ) 2 Cl 2 II. [Co(NH 3 ) 6 ]Cl 3 III. [Ni(NH 3 ) 4 (NO 2 ) 2 ] IV. K 2 [CoCl 4 ] A. 0 B. 1 C . 2 D. 3 E. 4 I. Pt(NH 3 ) 2 Cl 2 In the square planar form, this molecule can exist as cis- and trans-isomers, which are geometric isomers. Note: In the tetrahedral form, this molecule cannot exist as geometric isomers. However, this molecule has been identified in class as only existing as square-planar. II. [Co(NH 3 ) 6 ]Cl 3 In the octahedral form, the six NH 3 groups occupy all possible positions. Hence, there are no cis-trans isomers. Therefore, there are no geometric isomers. III. [Ni(NH 3 ) 4 (NO 2 ) 2 ] In the octahedral form, the two nitro groups can be cis to each other or trans to each other. Hence, this molecule can exist as cis- and trans-isomers, which are geometric isomers. IV. K 2 [CoCl 4 ] In the square planar form, the chlorides occupy all possible positions. Hence, there are no cis-trans isomers. Therefore, there are no geometric isomers. 2
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15 Chem 162-2007 Final exam + answers Chapter 22 – Transition Metals and Coordination Chemistry Coordination Compounds In the compound Na[FeCl 2 (C 2 O 4 )(NH 3 )(CO)], which of the following is acting as a Lewis acid? A. Cl - B . Fe 3+ C. NH 3 D. Na + E. CO A. Cl - is acting as a Lewis base. B. Fe 3+ is acting as a Lewis acid. C. NH 3 is acting as a Lewis base. D. Na + is acting as a counterion. E. CO is acting as a Lewis base. 3
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25 Chem 162-2007 Final exam + answers Chapter 22 – Transition Metals and Coordination Chemistry Coordination Compounds Which of the following coordination compounds will form a precipitate when treated with an aqueous solution of AgNO 3 ? A. [Cr(NH 3 ) 3 Cl 3 ] B . [Cr(NH 3 ) 6 ]Cl 3 C. [Cr(NH 3 )Cl](NO 3 ) 2 D. Na 3 [Cr(CN) 6 ] E. K 3 [CrCl 6 ] Ag + reacts with Cl - to form a AgCl precipitate. If a Cl - is a ligand in a complex ion, then it is covalently bonded to the metal ion. A covalent bond is a strong bond, so Ag + won’t react with this type of Cl - . On the other hand, if the Cl - is a counter ion, then it is bonded to water molecules by ion-dipole bonds. Ion-dipole bonds are weak bonds, so Ag + will react with this type of Cl - . A. These chloride ions are ligands (covalently bonded), so they won’t react with Ag + to form a precipitate. B. These chloride ions are counterions (ion-dipole bonded), so they will react with Ag + to form a precipitate. C.
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This document was uploaded on 11/02/2011 for the course GEN CHEM 162 at Rutgers.

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CH31CC~1 - CHAPTERS 22 CHEM 162-2011 Some PRACTICE PROBLEMS...

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