Chapter 5, Problem 5.49SP

(a)

Interpretation Introduction

Interpretation:

The electron-dot structure for the amino acid glycine showing the lone pairs and the multiple bonds has to be drawn.

Concept introduction:

Electron-dot structure: It is a diagram in which dots are placed around the chemical symbol of an element to show its valence electrons. It is also called as Lewis dot diagrams.

(b)

Interpretation Introduction

Interpretation:

The approximate values for the $\text{H}-\text{C}-\text{H},\text{O}-\text{C}-\text{O}\text{and}\text{H}-\text{N}-\text{H}$ bond angles have to be determined.

Concept introduction:

VSEPR theory:

• Using VSEPR theory, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Bond angle is the angle between two bonds of a molecule and it is determined based on the electron-domain geometry.

  [Bond angles: tetrahedral = $\text{109}{\text{.5}}^{\text{o}}$, trigonal planar = ${\text{120}}^{\text{o}}$, T-shape = ${\text{90}}^{\text{o}}$]

(c)

Interpretation Introduction

Interpretation:

The hybrid orbitals used by the carbon and nitrogen atoms have to be determined.

Concept introduction:

Hybridization:

• It is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.
• Geometry of a molecule can be predicted by knowing its hybridization.
• ${\text{sp}}^{\text{3}}$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.
• ${\text{sp}}^2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.
• $\text{sp }$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.