Chapter 10, Problem 10.69QP

(a)

Interpretation Introduction

Interpretation:

The Lewis structures of ${\text{BF}}_{\text{3}}$ has to be drawn and shape of ${\text{BF}}_{\text{3}}$, planar or nonplanar has to be stated.

Concept Introduction:

• Lewis theory is about how electrons are arranged in the outer most valence shell of an atom so as to bond with the other atom in a molecule. Thus, the Lewis dot structure represents the bonding as well as the lone pairs and bond pairs of electrons.
• Planarity: The given molecules is said to be planar, only when all its atoms or ions lie on the same plane. If not so, then the molecule is said to be non-planar.

(b)

Interpretation Introduction

Interpretation:

The Lewis structures of ${\text{ClO}}_{\text{3}}{}^{-}$ has to be drawn and shape of ${\text{ClO}}_{\text{3}}{}^{-}$, planar or nonplanar has to be stated.

Concept Introduction:

• Lewis theory is about how electrons are arranged in the outer most valence shell of an atom so as to bond with the other atom in a molecule. Thus, the Lewis dot structure represents the bonding as well as the lone pairs and bond pairs of electrons.
• Planarity: The given molecules is said to be planar, only when all its atoms or ions lie on the same plane. If not so, then the molecule is said to be non-planar.

(c)

Interpretation Introduction

Interpretation:

The Lewis structure has to be drawn for ${\text{H}}_{\text{2}}\text{O}$ and direction of the resultant dipole moment in ${\text{H}}_{\text{2}}\text{O}$ has to be shown.

Concept Introduction:

Lewis structure:

Lewis theory is about how electrons are arranged in the outer most valence shell of an atom so as to bond with the other atom in a molecule. Thus, the Lewis dot structure represents the bonding as well as the lone pairs and bond pairs of electrons.

Bond moment:

In polar molecules, there will be a bond between a high electronegative atom and a least electronegative atom. The high electronegative atom pulls the shared pair of electrons towards itself and acquires a partial negative charge on it and creates a partial positive charge on the least electronegative atom. This is known as charge separation and the overall phenomenon is known as bond moment. It is a vector quantity which means it has both magnitude and direction.

Resultant dipole moment:

If all possible bond moments of a polar molecule are with different magnitudes, then a net dipole moment will be resulted which is known as the resultant dipole moment. If the bond moments are with same magnitudes, then there won’t be a resultant dipole moment since all the bond moments cancel with each other. So, the resultant dipole moment depends on the magnitude of bond moments. It is independent of the directions of bond moments.

(d)

Interpretation Introduction

Interpretation:

The Lewis structure has to be drawn for ${\text{OF}}_2$. and ${\text{OF}}_2$ is polar and non-polar has to be found.

Concept Introduction:

Lewis structure:

Lewis theory is about how electrons are arranged in the outer most valence shell of an atom so as to bond with the other atom in a molecule. Thus, the Lewis dot structure represents the bonding as well as the lone pairs and bond pairs of electrons.

Polarity:

In a molecule, if a covalent bond is existing between two different electronegative atoms, then there will be charge separation between the two atoms. One atom acquires a partial positive charge and the other atom acquires a partial negative charge. This phenomenon is known as polarity. So, if a molecule is said to be polar then there will be charge separation in the molecule which can have dipole moment whereas if a molecule is said to be non-polar then there will not be any charge separation in the molecule and hence do not have dipole moment in it.

(e)

Interpretation Introduction

Interpretation:

The Lewis structure has to be drawn for $\text{OSeO}$. and bond angle of $\text{OSeO}$ has to be estimated.

Concept Introduction:

Lewis structure:

Lewis theory is about how electrons are arranged in the outer most valence shell of an atom so as to bond with the other atom in a molecule. Thus, the Lewis dot structure represents the bonding as well as the lone pairs and bond pairs of electrons.

Bond angle:

In a particular geometry, the angle formed between two adjacent bonds of a same atom is known as the bond angle. The bond angle between two bonds differs with respect to a particular geometry.