The document provides an overview of solids, highlighting their definite shape, volume, and high density. It categorizes solids into crystalline and amorphous types, detailing the properties and examples of four types of crystalline solids: ionic, molecular, metallic, and covalent network solids. Key characteristics such as melting points, electrical conductivity, and structural arrangements are discussed for each type.

2. Applied Chemistry
 Name:
Matte Ullah
Roll No.:
16103123-028

3. Solids
Solids have:
 Definite shape
 Definite volume
 High density
 High Melting and boiling points
 Incompressibility factor
 Atoms are in vibratory motion

4. Types of solids
Solids are of two types.
 Crystalline solids:
The solids which have repetitive
arrangement of atoms and molecules are better known
as crystalline solids.
 Amorphous solids:
The solids which do not have
repetitive arrangement of atoms and molecules
are amorphous solids.

5. Properties of crystalline solids
 The crystalline solids exhibit regular repeating
structure represented by unit cells.
 These solids usually show specific and sharp melting
points.
 The diffractions through these crystals is found to be
very sharp.
 The breakage if any is observed only along the
crystallographic planes.

6. Types of Crystalline solids
There are four types of crystalline solids.
1. Ionic solids
2. Molecular solids
3. Metallic solids
4. Covalent network solids

7. Ionic solids
 Made up of positive and negative charges.
 Held together by electrostatic interactions.
 Hard and Brittle.
 High melting and boiling points.
 Insulators as solids.
 Conductors in molten state.
 Example is NaCl.

8. Molecular Solids
 Made up of molecules.
 Weak intermolecular forces.
 Weak conductors of electricity.
 Low melting and boiling points.

9. Metallic Solids
 Made up of metal cations surrounded by large number
of electrons.
 High melting and boiling points
 Good conductors of electricity.
 Range from soft and malleable very hard.

10. Covalent network solids
 Made of atoms which are covalently bonded to its
nearest neighbor atom.
 Hard and brittle.
 Very high melting and boiling points.
 Insulators or poor conductors of electricity.
 Examples are diamond and graphite.