Chapter 1, Problem 78CP

(a)

Interpretation Introduction

Interpretation:

To identify the hybridization state of boron atom, bond angle of $\text{O-B-O}$ and to draw all the lone pairs present in the given compound.

Concept introduction:

The atomic orbitals mix together to form a hybrid orbital which is suitable for forming bonds between the atoms to form a compound.  This mixing of hybrid orbitals is known as hybridization.  The hybridization determines the geometry of the particular atom in the compound.  Shortly to say

$s{p}^{3}hybridized$ =tetrahedral

trigonal pyramidal(if one lone pair of electron is present)

bent geometry (if two lone pair of electrons are present)

$s{p}^{2}hybridized$ =trigonal planar

$sp$ $hybridized$ =linear

To identify: To identify the hybridization state of boron atom in given compound

(b)

Interpretation Introduction

Interpretation:

To identify the hybridization state of boron atom, bond angle of $\text{O-B-O}$ and to draw all the lone pairs present in the given compound.

Concept introduction:

The atomic orbitals mix together to form a hybrid orbital which is suitable for forming bonds between the atoms to form a compound.  This mixing of hybrid orbitals is known as hybridization.  The hybridization determines the geometry of the particular atom in the compound.  Shortly to say

$s{p}^{3}hybridized$ =tetrahedral

trigonal pyramidal(if one lone pair of electron is present)

bent geometry (if two lone pair of electrons are present)

$s{p}^{2}hybridized$ =trigonal planar

$sp$ $hybridized$ =linear

To predict: To predict the bond angle of $\text{O-B-O}$ and to justify why the bond angle deviates.

(c)

Interpretation Introduction

Interpretation:

To identify the hybridization state of boron atom, bond angle of $\text{O-B-O}$ and to draw all the lone pairs present in the given compound.

Concept introduction:

The atomic orbitals mix together to form a hybrid orbital which is suitable for forming bonds between the atoms to form a compound.  This mixing of hybrid orbitals is known as hybridization.  The hybridization determines the geometry of the particular atom in the compound.  Shortly to say

$s{p}^{3}hybridized$ =tetrahedral

trigonal pyramidal(if one lone pair of electron is present)

bent geometry (if two lone pair of electrons are present)

$s{p}^{2}hybridized$ =trigonal planar

$sp$ $hybridized$ =linear

To draw: To draw all the lone pair of electrons in the given compound