Chapter 9 - University of Dayton Academic Webserver

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$MATH 219 - Differential Equations Quiz 3 Name Solutions Date ...$

300 Chapter 9: Molecular Structures Larger alkanes will all follow the same pattern. Since they are saturated, all the carbon atoms have four bonds, and every one of them will have a tetrahedral shape and tetrahedral bond angles. 40. (a) Write the Lewis structure. Use the VSEPR model to determine the electron-pair geometry of each of the atoms. Use Table 9.2 to determine the hybridization of the central atom using the electron-pair geometry. The bond angles are associated with the electron-pair geometry also, so use Figure 9.4. H H C H H C H H C C H C Look at the first two C atoms (the two farthest to the left): They are both of type AX 4E 0, so the electron-pair geometry is tetrahedral and these C atoms have sp 3 . hybridization. The sp 3 -hybridized C atoms have tetrahedral bond angles of approximately 109.5°. Look at the second two C atoms (the two farthest to the right): They are both of type AX 2E 0, so the electron-pair geometry is linear and these C atoms have sp hybridization. The sp-hybridized C atoms have linear bond angles of approximately 180°. (b) The shortest carbon-carbon bond is the triple bond. That can be confirmed by looking up the bond lengths in Table 8.1. (c) The strongest carbon-carbon bond is the triple bond. That can be confirmed by looking up the bond energies in Table 8.2. 41. The first bond between two atoms must always be a σ bond. When more than one pair of electrons are shared between atoms, they are always part of π bonds. So the second bond in a double bond and the second and third bonds in a triple bond are always π bonds. (a) π H σ C σ N. (b) (c) H σ . . N π σ .. N π σ H H σ .. π H H H C N N N σ σ H .. π . 42. The first bond between two atoms must always be a σ bond. When more than one pair of electrons are shared between atoms, they are always part of π bonds. So the second bond in a double bond and the second and third bonds in a triple bond are always π bonds. (a) (b) (c) π O σ C π σ S. . . .. . H σ . . σ N H σ .. O. σ H H σ C σ H π σ C σ C σ σ H H π σ O C C H .. ..
43. Use the method described in the answer to questions 38 and 41. (a) The structure has 12 sigma bonds. (b) The structure has four pi bonds. . C π σ π O C H σ π σ C C σ σ σ π H H C σ σ σ σ .. O σ C H σ H .. Chapter 9: Molecular Structures 301 (c) Look at the C atom bonded to the N atom: It is of type AX 2E 0, so the electron-pair geometry is linear and this C atom has sp hybridization. (d) Look at the C atom bonded both O atoms: It is of type AX 3E 0, so the electron-pair geometry is triangular planar and this C atom has sp 2 hybridization. Look at the C atom bonded to only one O atom: The type is AX 4E 0, so the electron-pair geometry is tetrahedral this C atom has sp 3 hybridization. (e) Look at the double bonded O atom: The type is AX 1E 2, so the electron-pair geometry triangular planar and this O atom has sp 2 hybridization. 44. Use the method described in the answer to questions 38 and 42. . π σ σ π N C C C π σ σ H (a) As seen above, the structure has six sigma bonds. (b) As seen above, the structure has three pi bonds. (c) Look at the C atom bonded to the N atom: It is of type AX 2E 0, so the electron-pair geometry is linear and these C atoms have sp hybridization. (c) Look at the N atom: It is of type AX 1E 1, so the electron-pair geometry is linear and it has sp hybridization. (e) Both H-bearing C atoms are type AX 3E 0, so the electron-pair geometry is triangular planar and both of them have a hybridization of sp 2 . Molecular Polarity 45. We need the Lewis structures and molecular shapes of CH 4, NCl 3, BF 3, and CS 2. H H H C H .. . .. .. . . .. .. .. .. . . . . .. F N Cl Cl B Cl .. .. F .. F. H σ σ H .. .. S .. .. C S
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