Chapter3 - 3.15 3.17 a) tetrahedral, V-shaped b)...

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Chapter 3 Homework 3.1 a) LCAO theory: Acronym for L inear C ombination of A tomic O rbitals; it is a sophisticated theory for the representation of bonding in covalent molecules. b) Sigma orbitals: A molecular orbital in which the increased electron density lies between the two nuclei involved in the bonding. c) VSEPR theory: The acronym for V alence S hell E lectron P air R epulsion theory, a method of predicting molecular shape using simple electron pair concepts of bonding. d) Hybridization: This theory involves the concept of mixing atomic orbitals on a central atom to give hybrid orbitals that have the directions to give the maximum overlap with the atomic orbitals of the surrounding atoms. e) Don’t do, we skipped this section. 3.3 BO = [(bonding electons)-(antibonding electrons)]/2 BO = (2-1)/2 BO = ½ 3.5
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The electron configuration for the N 2 + ion is: 3.11
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Unformatted text preview: 3.15 3.17 a) tetrahedral, V-shaped b) tetrahedral, trigonal pyramidal c) trigonal bipyramidal, linear d) octahedral, square planar 3.21 Oxygen difluoride and phosphorus trichloride. The bond angles will be reduced as a result of the presence of the lone pairs. 3.23 a) sp 3 b) sp 3 c ) s p 3 d d) sp 3 d 2 3.27 Hydrogen selenide, because with more electrons, the dispersion forces would be greater (the slightly weaker dipole-dipole interaction than that of hydrogen sulfide is a less important factor). 3.31 Ammonia, because the neighboring molecules will hydrogen-bond to each other, providing a strong intermolecular force and hence a higher boiling point than phosphane, which has the weaker dipole-dipole interactions. 3.29 Just get the shapes, we didnt discuss point groups: a) Trigonal pyramidal b) Trigonal planar c) Tetrahedral d) Octahedral...
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Chapter3 - 3.15 3.17 a) tetrahedral, V-shaped b)...

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