Exam 9: Molecular Geometry: Shape Determines Function

A) a decreasing effective nuclear charge.
B) a decrease in the number of lone pairs.
C) an increase in atomic radius.
D) an increase in the polarity of the molecules.
E) an increasing effective nuclear charge.

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A) They have different molecular formulas.
B) They are different structural isomers.
C) They are stereoisomers but not optical isomers.
D) They are optical isomers.
E) They are achiral.

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A) the same as the H-O-H angle in water.
B) exactly 109.5 $\degree$ .
C) greater than 109.5 $\degree$ .
D) less than 109.5°.
E) 120°.

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A) C₂H₂
B) H₂CO
C) CH₃Cl
D) C₂H₄
E) C₂H₂Cl₂

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A) SiF₄
B) KrF₄
C) SF₄
D) C₂H₄
E) C₂H₂

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A) Valence bond theory describes a bond as the overlap of atomic orbitals between two atoms.
B) Enhanced electron density between two positively charged nuclei attracts the nuclei together and forms the bond.
C) Hybridization of atomic orbitals is necessary to account for the molecular geometry.
D) In valence bond theory, hybridization determines the molecular shape or geometry.
E) Statements A-D are all correct.

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A) sp²
B) sp³
C) sp³d
D) sp
E) sp³d²

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A) CF₄
B) NF₃
C) F₂O
D) NF₂^-
E) NH₃

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The structure with all formal charges eq...

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A) SO₂
B) N₂O
C) HCN
D) CO₂
E) BeH₂

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C1 and C2 are sp² hybridized. B...

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A) ( $\sigma$ )
B) ( $\pi$ )
C) ( $\sigma$ *)
D) ( $\pi$ *)
E) s

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A) SO₂
B) OCS
C) ICl₃
D) I₃^-
E) C₂H₂

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A) carbon-oxygen
B) carbon-sulfur
C) carbon-nitrogen
D) carbon-hydrogen
E) carbon-chlorine

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A) linear
B) trigonal planar
C) tetrahedral
D) trigonal bipyramidal
E) octahedral

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A) H₂O
B) H₂S
C) ICl₃
D) I₃^-
E) SO₂

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A) $\left( \sigma _ { 2 s } \right) ^ { 2 } \left( \sigma _ { 2 s } ^ { * } \right) ^ { 2 } \left( \pi _ { 2 p } \right) ^ { 4 } \left( \sigma _ { 2 p } \right) ^ { 2 } \left( \pi _ { 2 p } ^ { * } \right) ^ { 2 } \left( \sigma _ { 2 p } ^ { * } \right) ^ { 2 }$
B) $\left( \sigma _ { 2 s } \right) ^ { 2 } \left( \sigma _ { 2 s } ^ { * } \right) ^ { 2 } \left( \pi _ { 2 p } \right) ^ { 6 } \left( \sigma _ { 2 s } \right) ^ { 2 } \left( \pi _ { 2p } ^ { * } \right) ^ { 2 }$
C) $\left( \sigma _ { 2 s } \right) ^ { 2 } \left( \sigma _ { 2 s } ^ { * } \right) ^ { 2 } \left( \sigma _ { 2p } \right) ^ { 2 } \left( \pi _ { 2 p } \right) ^ { 4 } \left( \pi _ { 2 p } ^ { * } \right) ^ { 4 }$
D) $\left( \sigma _ { 2 s } \right) ^ { 2 } \left( \sigma _ { 2 s } ^ { * } \right) ^ { 2 } \left( \pi _ { 2 p } \right) ^ { 4 } \left( \sigma _ { 2 p } ^ { * } \right) ^ { 2 } \left( \pi _ { 2 p } ^ { * } \right) ^ { 4 }$
E) $\left( \sigma _ { 2 s } \right) ^ { 2 } \left( \sigma _ { 2 s } ^ { * } \right) ^ { 2 } \left( \pi _ { 2p } \right) ^ { 4 } \left( \sigma _ { 2 p } \right) ^ { 2 } \left( \sigma _ { 2 p } ^ { * } \right) ^ { 2 } \left( \pi _ { 2 p } ^ { * } \right) ^ { 2 }$

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A) linear
B) bent
C) tetrahedral
D) trigonal pyramidal
E) trigonal planar

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