#CD0DB~1 - CHEM 161-2007 CHAPTER 10 BONDING THEORY AND...

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CHEM 161-2007 CHAPTER 10 – BONDING THEORY AND MOLECULAR STRUCTURE PRACTICE PROBLEMS DR. ED TAVSS VSEPR, polarity and bond angles Hybridization, σ & π bonds Please note that the type of bond orbital for terminal group atoms followed one set of rules (non- hybridization) using Hill & Petrucci, but followed a different set of rules (hybridization) taught in the Zumdahl & Zumdahl textbook. The Rutgers chemistry faculty generally follows the Hill & Petrucci rules (terminal atoms not hybridized; i.e., terminal atom bonding via p-orbitals) 1
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VSEPR, POLARITY AND BOND ANGLES 43 Chem 161-2006 Final Exam Chapter 10 – Bonding theory and Molecular Structure (VSEPR) Molecular structure, angles and polarity (VSEPR) What is the electron group geometry for XeF4? A. tetrahedral B. trigonal planar C. trigonal bipyramidal D. octahedral E. linear . . : F : . . .. | . . : F ― Xe ― F : . . . . | . . : F : . . D 2
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23 Chem 161-2006 Final Exam Chapter 10 – Bonding theory and Molecular Structure (VSEPR) Molecular structure, angles and polarity (VSEPR) Rank the Cl-C-Cl bond angles in the compounds below from smallest to largest? (Smallest angle first, largest angle last) I. NCl 3 II. SiCl 4 III. Cl 2 O IV. BCl 3 A. IV<II<I<III B. I<IV<II<III C . III<I<II<IV D. I<II<III<IV E. II<IV<III<I . . : Cl : . . | . . <109.5 o : Cl ― N ― Cl : . . . . . . . . :Cl: . . | . . :Cl―Si―Cl : 109.5 o . . | . . :Cl: . . . . . . . . :Cl O Cl : <<109.5 o . . . . . . . . : Cl : . . | . . : Cl ― B ― Cl : 120 o . . . . C 3
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16 Chem 161-2006 Final Exam Chapter 10 – Bonding theory and Molecular Structure (VSEPR) Molecular structure, angles and polarity (VSEPR) The molecular geometries of POCl3 and PCl5 may be described as A. tetrahedral and trigonal bipyramidal B. octahedral and trigonal bipyramidal C. trigonal bipyramidal and see-saw D. square planar and trigonal bipyramidal E. tetrahedral and square pyramidal . . : Cl : . . | . . : Cl― P ― Cl : Tetrahedral . . | . . : O : . . . . . . : Cl : : Cl : . . . . : Cl ― P ― Cl : Trigonal bipyramidal . . | . . : Cl : . . A 4
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7 Chem 161-2006 Final Exam Chapter 10 – Bonding theory and Molecular Structure (VSEPR) Molecular structure, angles and polarity (VSEPR) Which of the following molecules is/are polar? BF 3 C C Cl H Cl H C C Cl H H Cl CO 2 1 2 3 4 5 PCl 3 A . 1 and 4 B. 1 and 3 C. 2, 3 and 5 D. 3 and 4 E. 1, 2, 3, 4 and 5 . . : Cl : . . | . . Polar : Cl ― P ― Cl : . . . . . . . . : F : . . | . . Non-polar : F ― B ― F : . . . . Cl H | | C = C Non-polar | | H Cl Cl Cl | | C = C Polar | | H H . . . . : O = C = O : Non-polar A 5
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15 Chem 161-2005 Hourly Exam III Chapter 8 – Bonding: General Concepts Molecular structure, angles, and polarity (VSEPR) What are the bond angles around each of the indicated atoms? CH 3 CH 2 CH N CH CH 3 OH .. .. N O A. 180 ° ~ 120 B. < 109.5 < 109.5 C. ~ 120 ~ 120 D. < 109.5 180 E . < 120 < 109.5 N has three effective electron pairs and is therefore trigonal planar, with bond angles of 120 o . However, since the pi electrons need a little extra room, the CNC bond angle is a little less than 120 o . Oxygen has four effective electron pairs around it. Therefore, the COH bond angle should be 109.5 o . However, since non-bonding electron pairs require a little extra room the COH bond angle is a little under 109.5 o .
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#CD0DB~1 - CHEM 161-2007 CHAPTER 10 BONDING THEORY AND...

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