Chapter 1, Problem 1.3P

Interpretation Introduction

(a)

Interpretation:

The Lewis structure for ${\text{HCCl}}_{\text{3}}$ is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(b)

Interpretation:

The Lewis structure for ${\text{NH}}_{\text{3}}$ is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(c)

Interpretation:

The Lewis structure for ${\left[{\text{NH}}_{\text{4}}\right]}^{+}$ is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.

Interpretation Introduction

(d)

Interpretation:

The Lewis structure for ${\left[{\text{H}}_{\text{3}}\text{O}\right]}^{+}$ is to be drawn is to be drawn with unshared pairs and the formal charges.

Concept introduction:

The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.

The rules to draw Lewis structure are given as,

• Determine the electronegativity and the number of valence electrons contributed by each atom.

• Generally, the lowest electronegativity atom is the central atom.

• Write the skeleton structure of the molecule.

• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.

• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.