C121 11-3 lec36GL

C121 11-3 lec36GL - Lecture 36 December 5, 2011 Review...

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Lecture 36 December 5, 2011 Review Today: Problems from: Chapter 13: Bonding Lewis Structures / Formal Charges / Resonance Structures Bond Enthalpies Chapter 14: Covalent Bonding / Orbitals VSEPR / Hybridization Molecular Orbital Diagrams Chapter 16: Intermolecular Forces Trends in IMF’s Vapour Pressure Phase Diagrams Chapter 17: Solutions Colligative Properties
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Decide which is the most likely structure for a molecule containing two nitrogen atoms and one oxygen atom: NNO or NON ? Does this structure have any resonance structures ?
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Calculate the bond dissociation energy in kJ for the (O-H) bond in H 2 O 2 , given D(H 2 ) = 435 kJ/mole D(O 2 ) = 495 kJ/mole D(O-O) = 139 kJ/mole UH f ˚(H 2 O 2 ) = -139.7 kJ/mole
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Describe the molecular shape, atomic hybridization and molecular polarity for each of the following (a) SiH 4 (b) C 2 Cl 4 (c) I 3 - and (d) SO 2
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Using M.O. diagrams, order the following molecules in order of increasing bond length: C 2 , F 2 , CN + , H 2 For how many of these does bond order decrease if one e- is removed ?
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Arrange the following compounds in order of increasing boiling points: ethyl methyl ether, C 2 H 5 OCH 3 , 2-methylpropane, C 4 H 10 , acetone, CH 3 COCH 3
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This note was uploaded on 12/10/2011 for the course CHEM 121 taught by Professor Leech during the Fall '11 term at Simon Fraser.

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C121 11-3 lec36GL - Lecture 36 December 5, 2011 Review...

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