Chapter 11, Problem 11.36QP

The melting points of the oxides of the third-period elements are given in parentheses: Na₂O (1275°C), MgO (2800°C), Al₂O₃ (2045°C), SiO₂ (1610°C), P₄O₁₀ (580°C), SO₃ (16.8°C), Cl₂O₇ (−91.5°C). Classify these solids in terms of crystal types.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{Na}}_2\text{O}$ solids is Ionic crystal.

Explanation of Solution

Sodium is a highly electropositive metal and Oxygen is a highly electronegative non-metal.  The bonding between electropositive metal and electronegative non-metal is undoubtedly ionic due to the huge electronegative difference between them.  Hence ${\text{Na}}_2\text{O}$ is an ionic crystal made of Sodium and Oxygen ions held together by ionic bond.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

$\text{MgO}$ solid is Ionic crystal.

Explanation of Solution

Magnesium is a highly electropositive metal and Oxygen is a highly electronegative non-metal.  The bonding between electropositive metal and electronegative non-metal is undoubtedly ionic due to the huge electronegative difference between them.  Hence, $\text{MgO}$ is an ionic crystal made of Sodium and Oxygen ions held together by ionic bond.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{Al}}_2{\text{O}}_3$ solids is Ionic crystal.

Explanation of Solution

${\text{Al}}_2{\text{O}}_3$ is an ionic compound and has ionic bond.  The type of crystal it forms is ionic crystal.

Aluminium is an electropositive metal and Oxygen is a highly electronegative non-metal.  The bonding between electropositive metal and electronegative non-metal is ionic due to the huge electronegative difference between them.  Hence ${\text{Al}}_2{\text{O}}_3$ is an ionic crystal made of Aluminium and Oxygen ions held together by ionic bond.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{SiO}}_2$ solid is Covalent crystal.

Explanation of Solution

${\text{SiO}}_2$ is covalent compound and is made of covalent bonds. The type of crystal it forms is covalent crystal.

The electronegativity difference between Silicon and Oxygen is not very high.  Hence, Silicon and Oxygen form covalent bond with each other.  In ${\text{SiO}}_2$ Silicon and Oxygen are linked by covalent bond.  These covalent linkages establish a network like structure of ${\text{SiO}}_2$ and it forms covalent crystals.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{P}}_4{\text{O}}_{10}$ is  Molecular crystal.

Explanation of Solution

${\text{P}}_4{\text{O}}_{10}$ is covalent compound and is made of covalent bonds.  The type of crystal it forms is molecular crystal.

The electronegativity difference between Phosphorus and Oxygen is not very high.  Hence, Phosphorus and Oxygen form covalent bond with each other.  ${\text{P}}_4{\text{O}}_{10}$ form molecular crystals consist of discrete ${\text{P}}_4{\text{O}}_{10}$ molecules.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{SO}}_3$ are  Molecular crystals.

Explanation of Solution

${\text{SO}}_3$ is covalent compound and is made of covalent bonds.  The type of crystal it forms is molecular crystal.

The electronegativity difference between Sulfur and Oxygen is not very high.  Hence, Sulfur and Oxygen form covalent bond with each other. ${\text{SO}}_{\text{3}}$ form molecular crystals consist of discrete ${\text{SO}}_{\text{3}}$ molecules.

Interpretation Introduction

Interpretation:

The following solids have to be classified in terms of crystal types.

${\text{(a) Na}}_2\text{O}\text{(b)}\text{MgO}\text{(c)}{\text{Al}}_2{\text{O}}_3\text{(d)}{\text{SiO}}_2\text{(e)}{\text{P}}_4{\text{O}}_{10}\text{ (f)}{\text{ SO}}_3\text{(g)}{\text{Cl}}_2{\text{O}}_7$

Concept Introduction:

• On the basis of the arrangement of the components, there are two distinct types of solids - crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.
• Crystalline solids, also known as crystals have their own sub-classification. The types of crystals can be summarized as follows –

  

• Crystals have well-defined regular, compact, orderly arrangement of their components of very long range order.  They are classified as – Ionic crystals, molecular crystals, covalent crystals and metallic crystals.
• In ionic crystals, ions of opposite charges are bind together by electrostatic force and are neatly stacked to form a regular and well-defined structure. Example:$\text{KCl}$, Rutile.
• In molecular crystal, molecules are arranged in such a fashion and in metallic crystal metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.
• In Covalent crystals the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.  Network solids are widely formed by group 14 elements and its compounds. Example: Diamond, Amethyst.
• All these types of solids differ in their respective intramolecular as well as intermolecular forces.  As a result, each type of solid has unique properties.

Answer to Problem 11.36QP

${\text{Cl}}_2{\text{O}}_7$ are  Molecular crystals.

Explanation of Solution

${\text{Cl}}_2{\text{O}}_7$ is covalent compound and is made of covalent bonds.  The type of crystal it forms is molecular crystal.

The electronegativity of Chlorine and Oxygen differs slightly.  Hence, Chlorine and Oxygen form covalent bond with each other. ${\text{Cl}}_{\text{2}}{\text{O}}_{\text{7}}$ forms molecular crystals consist of discrete ${\text{Cl}}_{\text{2}}{\text{O}}_{\text{7}}$ molecules.