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One state of matter can be referred to as a “solid state.” Solid, liquid, and gas are the three states of matter we were taught in elementary school. There are more things to learn as we proceed from elementary school to high school. When it comes to an understanding the concept of solid-state,Â
They can, for example, withstand any force applied to their surface. However, the features of atoms, such as their arrangement and the forces acting between them, have a major role in determining the solid state of compounds.
Solids are classified into crystalline solid and amorphous solid.
Type of Solid
Crystalline solids and amorphous solids are the two main types of solids distinguished by the arrangement of their constituent particles.
Crystalline Solids
The term “real solids” refers to crystalline solids. There are two types of minerals: crystalline and non-crystalline. Table salt is an example of a solid that falls into this category. Solids that are crystallised have molecules, ions, or atoms in a symmetric pattern that repeats throughout the crystal. Solids have unit cells, which can be thought of as bricks in a wall. In a crystal lattice, each unit cell is linked to the next. There are seven crystal systems that rely on the atomic structure in each Bravais lattice (named after Auguste Bravais, a French scientist) and their structures can be hexagonal, tetragonal, rhombohedral, orthogonal, monoclinic, and triclinic.
Types of Crystalline Solids
Ionic, molecular, network covalent, and metallic solids are the four forms of crystalline solids.
Ionic solids
Cations and anion ions, which have opposite charges, make up the crystals of ionic compounds. Because of the strong attraction between opposite charges, it takes a lot of energy to break an ionic connection. Another way of putting it is that most ionic compounds have melting points ranging from 300 to 1,000 degrees Celsius. (572 to 1,832 degrees Fahrenheit).
Molecular solids
Van der Waals forces are molecular solids that are covalently bonded together through electrostatic forces. When two atoms share electrons, the larger atom’s electron cloud is more likely to contain them. This results in a weak or fluctuating polarity in covalent bonding. In contrast to ionic or covalent crystals, molecular crystals have lower melting points and less brittleness because of their lesser electrostatic connection between the two poles. For the most part, molecular solids are nonpolar substances. Nonpolar solvents like benzene or octane can be used to dissolve them.
Network Covalent Solids
A network solid does not include molecules. The crystals’ enormous size is a result of the crystals’ extensive network of covalent connections. Covalent bonds bind all of the atoms together in a network solid. The properties of ionic solids and network solids are numerous. Solids with extraordinarily high melting values are highly hard and brittle. Like ionic compounds, they do not dissolve in water or conduct electricity.
Amethysts, Diamonds, and rubies are all examples of network solids.
Amorphous Solids
Amorphous solids do not have a recurring lattice pattern among its particles. Also known as pseudo solids, they’re a mathematical concept. Amorphous solids include, for example, rubber, glass,gels, and the vast majority of polymers. In an amorphous solid, the bonds don’t break all at once, hence the melting point is not fixed. Rather, it melts over a wide range of temperatures gradually.molten glass or Candle wax can be described as melting into soft, flexible wax, or completely melting into water.
The edges of sliced amorphous solids may be curved rather than straight because they are not symmetrical. Refractive index, tensile strength and conductivity are the same no matter which way a force is applied. For this reason, they are known as isotropic.
Conclusion
Solid, liquid, and gas are the three states of matter we were taught about in elementary school. There are two types of Solids that are crystalline solid and amorphous solid. Crystalline solids are made up of atoms arranged in a symmetrical pattern that repeats throughout the crystal. Molecular solids and network solids have several features. Molecular crystals have lower melting points and less brittleness than ionic or covalent crystals. Amorphous solids are not symmetrical; therefore, the edges may be curved rather than straight when sliced.
Glass, rubber, pitch, and several plastics are all examples of amorphous solids. Crystalline solids, such as quartz, have a regular arrangement of SiO4 tetrahedrons.
