Chapter 9, Problem 28Q

(a)

Interpretation Introduction

Interpretation:

The differences between the structures of following solids have to be highlighted and explained-

Diamond versus Graphite

Concept introduction:

                    A solid is anything that is firm and stable in shape. 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 have their own sub-classification. The types of solids can be summarized as follows –

    

                                                                        Figure 1

• Crystalline solids have well-defined regular, compact, orderly arrangement of their components of very long range order. They are termed as true solids. Ionic solids, molecular solids, covalent solids, atomic solids and metallic solids are the types of crystalline solids. 

• In ionic solids, 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.

• Amorphous solids lack such well defined arrangement of its components instead disordered or random arrangement does exist in them. They are termed as pseudosolids or super cooled liquids. Example: Glass, Wood etc.

• In molecular solid, molecules are arranged in such a fashion and in metallic solid metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.

• Non-metal atoms held together by weak London dispersion forces form atomic solids. Example: Solid Argon, Solid Krypton.

• In Covalent solids 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, Graphite.

(b)

Interpretation Introduction

Interpretation:

The differences between the structures of following solids have to be highlighted and explained-

• Silica versus Silicates versus Glass

Concept introduction:

                    A solid is anything that is firm and stable in shape. 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 have their own sub-classification. The types of solids can be summarized as follows –

    

                                                                        Figure 1

• Crystalline solids have well-defined regular, compact, orderly arrangement of their components of very long range order. They are termed as true solids. Ionic solids, molecular solids, covalent solids, atomic solids and metallic solids are the types of crystalline solids. 

• In ionic solids, 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.

• Amorphous solids lack such well defined arrangement of its components instead disordered or random arrangement does exist in them. They are termed as pseudosolids or super cooled liquids. Example: Glass, Wood etc.

• In molecular solid, molecules are arranged in such a fashion and in metallic solid metal atoms are arranged in such a manner. Example: Ice for molecular solid and almost all metals and alloys for metallic solids.

• Non-metal atoms held together by weak London dispersion forces form atomic solids. Example: Solid Argon, Solid Krypton.

• In Covalent solids 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, Graphite.