Chapter 1, Problem 49P

Draw a Lewis structure for each of the following:

1. a. N₂H₄
2. 1. b. ${\text{CO}}_3^{2-}$
3. b. N₂H₂
4. c. CO₂
5. d. HOCl

Interpretation Introduction

Interpretation:

Lewis structure for ${\text{N}}_{\text{2}}{\text{H}}_{\text{4}}$ should be drawn.

Concept introduction:

• Lewis structure:

  A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

• The bond angel depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angel.
• For example, ${\text{sp}}^3$ carbon have bond angel of ${109.5}^0$,${\text{sp}}^2$ carbon have bond angel of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angel of  ${\text{180}}^{\text{0}}$.
• Lone-pair electrons are valence electrons that are not used in bonding.
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Lewis structure:

A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

Answer to Problem 49P

Lewis structure drawn for the ${\text{N}}_{\text{2}}{\text{H}}_{\text{4}}$(Dinitrogen Tetra hydride) molecule.

Explanation of Solution

${\text{N}}_{\text{2}}{\text{H}}_{\text{4}}$ Doesn’t contain Double or triple bond.

The two Nitrogen (N) atoms lie in the Center and the four lies outside.

Hydrogen atom need two electrons to fulfill the octet rule.

For the Lewis structure for the ${\text{N}}_{\text{2}}{\text{H}}_{\text{4}}$ molecule contains 14 valence electrons.

Interpretation Introduction

Interpretation:

Lewis structure for ${\text{CO}}^{\text{2-}}{}_{\text{3}}$ should be drawn.

Concept introduction:

• Lewis structure:

  A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

• The bond angel depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angel.
• For example, ${\text{sp}}^3$ carbon have bond angel of ${109.5}^0$,${\text{sp}}^2$ carbon have bond angel of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angel of  ${\text{180}}^{\text{0}}$.
• Lone-pair electrons are valence electrons that are not used in bonding.
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Lewis structure:

A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

Answer to Problem 49P

Lewis structure drawn for the ${\text{CO}}^{\text{2-}}{}_{\text{3}}$ (Carbonate ion)  molecule.

Explanation of Solution

${\text{CO}}^{\text{2-}}{}_{\text{3}}$ Carbonate ion has two negative charge and the valence electrons are arranged themselves to achieve the octet rule.

Oxygen has 6 valence electrons and Carbons have 4 valence electrons so Oxygen atom needs two electrons and Carbon atom needs 4 electrons atom to satisfy the octet rule as shown above the structural molecule is kept in a bracket for better presentation of Lewis structure because the Negative charge lies in the right top end of the bracket.

Interpretation Introduction

Interpretation:

Lewis structure for ${\text{N}}_{\text{2}}{\text{H}}_{\text{2}}$ should be drawn.

Concept introduction:

• Lewis structure:

  A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

• The bond angel depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angel.
• For example, ${\text{sp}}^3$ carbon have bond angel of ${109.5}^0$,${\text{sp}}^2$ carbon have bond angel of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angel of  ${\text{180}}^{\text{0}}$.
• Lone-pair electrons are valence electrons that are not used in bonding.
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Lewis structure:

A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

Answer to Problem 49P

Lewis structure for the given molecule ${\text{N}}_{\text{2}}{\text{H}}_{\text{2}}$ is drawn below;

The ${\text{N}}_{\text{2}}{\text{H}}_{\text{2}}$ Lewis structure has the 12 valence electrons.

The total valence electrons are spatially arranging themselves for fulfillment of octet rule.

Dinitrogen hydride (${\text{N}}_{\text{2}}{\text{H}}_{\text{2}}$) .

Explanation of Solution

Interpretation Introduction

Interpretation:

Lewis structure for ${\text{CO}}_{\text{2}}$ should be drawn.

Concept introduction:

• Lewis structure:

  A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

• The bond angel depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angel.
• For example, ${\text{sp}}^3$ carbon have bond angel of ${109.5}^0$,${\text{sp}}^2$ carbon have bond angel of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angel of  ${\text{180}}^{\text{0}}$.
• Lone-pair electrons are valence electrons that are not used in bonding.
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Lewis structure:

A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

Answer to Problem 49P

Lewis structure for the given molecule ${\text{CO}}_{\text{2}}$ is drawn below;

Explanation of Solution

Carbon(C) is the least electronegative atom in the ${\text{CO}}_{\text{2}}$ Lewis structure and threfore at the center of the structure .

The Lewis structure for complete  the octate for all of the atom in the structure .

The total valence electrons are 16.

Carbond dioxide contai n one Carbon molecule and Two Oxygen molecule.

Carbond molecule contain 4 electrons and the Oxygen molecule contain the 6 Electrons as the  valence electron.

There is a double bond inbetween Crabond and Oxygen atom and posses Linear structure (${180}^0$).

The structure can lie in one plane so it is alos planar in nature.

The total valnce electron arrange themselves sapatially to satisfy the octate rule.

Interpretation Introduction

Interpretation:

Lewis structure for $\text{HOCl}$ should be drawn.

Concept introduction:

• Lewis structure:

  A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

• The bond angel depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angel.
• For example, ${\text{sp}}^3$ carbon have bond angel of ${109.5}^0$,${\text{sp}}^2$ carbon have bond angel of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angel of  ${\text{180}}^{\text{0}}$.
• Lone-pair electrons are valence electrons that are not used in bonding.
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

Lewis structure:

A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.

Answer to Problem 49P

Lewis structure for the given molecule $\text{HOCl}$ is drawn below;

Hypochlorous acid possesses 14 electrons in their valence shell and the Oxygen atom is more electronegative than Chlorine atom.

Oxygen is resides at the center of the molecule Hypochlorous acid ($\text{HOCl}$) .

Explanation of Solution

Lewis structure for the given molecule $\text{HOCl}$ is drawn below;

Hypochlorous acid possesses 14 electrons in their valence shell and the Oxygen atom is more electronegative than Chlorine atom.

Oxygen is resides at the center of the molecule Hypochlorous acid ($\text{HOCl}$) .