The planar configuration at the nitrogen atom and hindered rotation about the C − N bond in amides is to be explained. Concept introduction: Geometry of an atom is determined by the number of electron groups around it. For four electron groups, the geometry is tetrahedral. For three electrons groups, the geometry is trigonal planar, and for two electron group, it is linear. An electron group is a lone pair or a bond. A single bond, a double bond, and a triple bond all count as just one electron group each. Molecules in which an atom with a lone pair or a multiple bond is present next to a single bond can exhibit resonance. The groups attached to a single bond can rotate relatively freely around the bond axis as it does not involve any change in the overlap of the bonding orbitals. Groups attached to a double or triple bond cannot easily rotate around the bond axis as this involves a substantial reduction in overlap of bonding orbitals, equivalent to breaking of one (or two ) bonds.

Question

Want to see the full answer?

Answer 1

Question

Chapter 3, Problem 3.56P

Interpretation Introduction

Interpretation:

The planar configuration at the nitrogen atom and hindered rotation about the C−N bond in amides is to be explained.

Concept introduction:

Geometry of an atom is determined by the number of electron groups around it. For four electron groups, the geometry is tetrahedral. For three electrons groups, the geometry is trigonal planar, and for two electron group, it is linear.

An electron group is a lone pair or a bond. A single bond, a double bond, and a triple bond all count as just one electron group each.

Molecules in which an atom with a lone pair or a multiple bond is present next to a single bond can exhibit resonance.

The groups attached to a single bond can rotate relatively freely around the bond axis as it does not involve any change in the overlap of the bonding orbitals.

Groups attached to a double or triple bond cannot easily rotate around the bond axis as this involves a substantial reduction in overlap of bonding orbitals, equivalent to breaking of one (or two ) bonds.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Choose the Lewis structure for the compound below: H2CCHOCH2CH(CH3)2 HH H :d H H H C. Η H H HH H H H H. H H H HH H H H H H- H H H C-H H H HHHH

Each of the highlighted carbon atoms is connected to hydrogen atoms.

く Complete the reaction in the drawing area below by adding the major products to the right-hand side. If there won't be any products, because nothing will happen under these reaction conditions, check the box under the drawing area instead. Note: if the products contain one or more pairs of enantiomers, don't worry about drawing each enantiomer with dash and wedge bonds. Just draw one molecule to represent each pair of enantiomers, using line bonds at the chiral center. More... No reaction. Explanation Check O + G 1. Na O Me Click and drag to start drawing a structure. 2. H + 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 000 Ar P