Chapter 4, Problem 4.86CP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures for acetone have to be drawn.

Concept introduction:

Lewis structures are also known as Lewis dot structures which represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

(b)

Interpretation Introduction

Interpretation:

The geometry around the carbon atoms of two Lewis structures of acetone has to be determined.

Concept introduction:

Molecular geometry can be predicted from the structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

• Count the number of valence electron pairs (bond pairs and lone pairs).
• Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.
• If there are only two bond pair electrons, the molecule is linear.
• If there are three bond pair electrons, the molecule is shaped like a trigonal planar.
• If there are four bond pair electrons, the molecule is shaped as a regular tetrahedral.
• Repulsion between lone pair-bond pair of electrons effect the geometry of molecules.

(c)

Interpretation Introduction

Interpretation:

The polar bonds in the Lewis structures of acetone have to be determined.

Concept introduction:

Covalent bonds are formed by sharing of electrons between atoms.

The polarity of a bond is arises due to the difference in electronegativity of atoms present in that bonding.