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# Molecular Geometry: Bond Angles, Planarity, Hybridization

CHEM-KHXS@P

Which of the statements that follow is MOST appropriate regarding the following molecule?

A

All of the atoms highlighted in blue are in the same plane. The C=O bond is formed by ${ sp }^{ 2 }-{ sp }^{ 2 }$ and $p-p$ overlap. The N-C-N angle is larger than the C-N-S angle. Expecting the N-S-O angle to be approximately 109${ }^{ \circ }$ is reasonable since the S has four groups of electrons around it. This molecule has 6 atoms with tetrahedral electron pair geometry.

B

All of the atoms highlighted in blue are in the same plane. The C=O bond is formed by ${ sp }^{ 3 }-{ sp }^{ 3 }$ and $p-p$ overlap. The N-C-N angle is smaller than the C-N-S angle. Expecting the N-S-O angle to be approximately 120${ }^{ \circ }$ is reasonable since the S has four groups of electrons around it. This molecule has 3 atoms with tetrahedral electron pair geometry.

C

All of the atoms highlighted in blue are not in the same plane. The C=O bond is formed by ${ sp }^{ 2 }-{ sp }^{ 2 }$ and $p-p$ overlap. The N-C-N angle is larger than the C-N-S angle. Expecting the N-S-O angle to be approximately 90${ }^{ \circ }$ is reasonable since the S has four groups of electrons around it. This molecule has 10 atoms with trigonal planar electron pair geometry.

D

All of the atoms highlighted in blue are not in the same plane. The C=O bond is formed by ${ sp }^{ 2 }-{ sp }^{ 2 }$ and $p-p$ overlap. The N-C-N angle is larger than the C-N-S angle. Expecting the N-S-O angle to be approximately 109${ }^{ \circ }$ is reasonable since the S has four groups of electrons around it. This molecule has 10 atoms with trigonal planar electron pair geometry.