The solid which is soft, low melting point and its molten state, aqueous state are non-conducting has to be classified. Concept Introduction: A solid is anything that is firm and stable in shape. Physics and Chemistry do provide clear cut explanation for the structure of solids. The firm and dense nature of solids is due to the strong intermolecular forces between their components. On the basis of the arrangement of the components in a solid, 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 further 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. Amorphous solids lack such well defined arrangement of its components instead disordered or random arrangement does exist in them. They are termed as pseudo solids or super cooled liquids . Example: Glass, Wood etc. Ionic solids, molecular solids, covalent 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: KCl , Rutile. 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, 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.

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Chapter 12, Problem 12.37QP

Interpretation Introduction

Interpretation:

The solid which is soft, low melting point and its molten state, aqueous state are non-conducting has to be classified.

Concept Introduction:

A solid is anything that is firm and stable in shape. Physics and Chemistry do provide clear cut explanation for the structure of solids. The firm and dense nature of solids is due to the strong intermolecular forces between their components.

On the basis of the arrangement of the components in a solid, 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 further 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.

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

Ionic solids, molecular solids, covalent 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:KCl, Rutile.

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, 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.

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