The following Topics and Sub-Topics are covered in this chapter and are available on MSVgo:
The following Topics and Sub-Topics are covered in this chapter and are available on MSVgo:
Introduction
Matter exists in solid, liquid, and gaseous forms. Solids are known to exhibit rigidity as the molecules are in fixed positions and can only oscillate in mean positions. Contrary to the solids, fluids (liquid & gas) can flow because their molecules can move about freely as they are not tightly compacted. Here the focus is on Solid State Chemistry.
Before dwelling on the concept, you should understand why solids act differently from liquids. Due to the arrangement of atoms and molecules, the physical and chemical properties of solids vary. Depending on the type of atoms and molecules the chemical characteristic of every solid is different. These notes will help you revise for exams and succinctly explain Solid State Chemistry.
As we were discussing the peculiarity of solids, certain properties were being repeatedly mentioned. Below are the characteristic properties of solids:
The study of properties-functions, structures, and synthesis of solid materials is termed as Solid State Chemistry. It is also referred to as material chemistry. Solid State Chemistry is studied to understand the properties and characteristics of solids. The functions and properties are a consequence of the arrangement and alignment of constituents as well as the type of constituents. To learn more, you need to understand the types of solids and their properties.
There are definitively two types of Solid State. Solid states are differentiated based on the arrangement of constituting particles:
Below are all types and subtypes of solid states discussed briefly.
Crystalline Solid State
Crystalline solids are the substances wherein the constituent particles are arranged in a regular-ordered long-ranged arrangement. You can imagine constituent particles of Crystalline Solid State arranged in fixed order arranged in a geometric shape. Each shape is made up of a large number of smaller crystals.
Example: Quartz, Sodium chloride, Diamond, etc.
Characteristic properties of crystalline solids
Types of crystalline solids:
o Metallic solids
o Ionic solids
o Molecular solids
o Covalent solids
Metallic solids
The constituents are metallic elements.
Examples of metallic solids are Iron (Fe), Nickel (Ni), Gold (Au), etc.
Ionic solids
The constituents are ions. They are arranged in a regular pattern of cations and anions bound by coulombic forces.
Example: NaCl, MgO, etc.
Molecular solids
The constituent particles in molecular solids are molecules. These are further divided into 3 sub-types.
Non-Polar Molecular Solids
The constituent particles of this type of solid have a nonpolar covalent bond. The forces holding these particles are London forces or weak dispersion forces.
Example: F2, H2, etc.
Polar Molecular Solids
The constituent particles share polar covalent bonds, due to which they share strong dipole-dipole interactions
Example: HCl, NH3, etc.
Hydrogen-Bonded Molecular solids
These are the solids that consist of a bond between Hydrogen, Oxygen, Fluoride, and Nitrogen atoms called hydrogen bonds. Due to the hydrogen bonds, molecules are strongly held.
Example: H20, H2F, etc.
Covalent Solids
They are also called network solids. The constituent particles have covalent bonds between them across the entire solid structure.
Example: SiO2, CH4, etc.
Amorphous Solid State
Amorphous solids (in Greek amorphous- no form) consist of particles arranged in an irregular shape. The definite arrangements of particles are for short-range order. Meaning the periodic arrangement and regular order is only for short distances.
Example: Quartz glass, rubber, plastics, etc.
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