Lecture 22 (10am) Chapter 10 and Chapter 11 November 17 2009

Lecture 22 (10am) Chapter 10 and Chapter 11 November 17...

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Chapter 10 (just a little bit) and onto Chapter 11 Lecture 22 November 17, 2009
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What is the molecular shape of NOCl as predicted by the VSEPR theory? (A) linear (B) trigonal planar (C) bent (D) tetrahedral (E) trigonal pyramidal
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A. trigonal pyramidal B. square planar C. square pyramidal D. tetrahedral E. octahedral What is the molecular shape of ClO 3 F as predicted by the VSEPR theory?
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Use VSEPR theory to decide which one of the following molecules and ions will definitely have at least one 90 o bond angle in it. (In each case except water, the central atom is the first one in the formula.) (A) AlCl 4 - (B) NH 3 (C) PCl 5 (D) CO 2 (E) H 2 O
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Exam 3 material stops here … Chapter 11 is not on the third exam
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Chapter 11
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Valence Bond Theory General premise: a covalent bond forms when orbitals of 2 atoms overlap and the overlap region (between the two bonded nuclei) is
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Unformatted text preview: occupied by a pair of electrons Bond strength depends on the attraction of the bonded nuclei for the shared electrons, so the greater the orbital overlap, the stronger the bond Hybridization involves the mixing of different orbitals of an atom to form new “Hybrid Orbitals” Hybrid Orbitals: sp, sp 2 , sp 3 , sp 3 d, sp 3 d 2 Listed above are the 5 common types of hybridization – you will see a link between the 5 basic electron group geometries (linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral) Examples of molecules with hybridization of central atom: sp: BeF 2 , HgCl 2 sp 2 : BF 3 , SO 3 sp 3 : CH 4 , NH 3 , H 2 O, NH 4 + sp 3 d: PF 5 , SF 4 , BrF 3 sp 3 d 2 : SF 6 , ClF 5 , XeF 4 , PF 6-...
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This note was uploaded on 10/22/2011 for the course CHEM 1200 taught by Professor Mcintosh during the Spring '08 term at Rensselaer Polytechnic Institute.

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Lecture 22 (10am) Chapter 10 and Chapter 11 November 17...

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