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Home / Chemistry / Classification Of Crystalline Solids - Part 1 | Testbook

Classification Of Crystalline Solids - Part 1 | Testbook

Last Updated on Mar 12, 2025
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The Solid State
Difference Between Isotropic and Anisotropic Zinc Blende Structure Amorphous Solids Crystalline Solids Metallic Bonds Packing in Solids Crystal Structure Interstitial Compounds Defects in Crystal Structure Frenkel Defect Bravais Lattice Phase Changes Unit Cell Density of Unit Cell Thermal Conductivity of Copper Carbon Nanotubes Polymorphism Fick's Law of Diffusion Ductility and Malleability Crystallization Types of Solids Charge Density and Melting Point Close Packing in Three Dimensions Conductors Crystal Salt Crystal Lattices and Unit Cells Dielectric Properties of Solids Difference Between Crystalline and Amorphous Solids Ductility Electrical Properties of Solids Materials Melting Point Structure of Zeolites "BCC Classification of Crystalline Solids Imperfections in Solids Schottky Defect Thermal Conductivity Unit Cell Packing Efficiency Voids in Solid State Lattice Enthalpy of an Ionic Solid Classification of Solids Based on Crystal Structure Fluorite Structure
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Crystalline solids are a common type of solid, with their classification based on the intermolecular forces that bind them together.

Contents

Molecular Solids

Molecular solids are typically insulating, soft, and low-density. Common examples include solid nitrogen, iodine, phosphorus, and carbon dioxide. These solids can be further divided into distinct categories.

Non-Polar Molecular Solids

Non-polar molecular solids have an even distribution of electrons, with no excess charge on either side. Examples include helium, neon, argon, and krypton. They are typically gases or liquids at room temperature and pressure. The molecules in these solids are held together by weak dispersion or London forces, which are weaker than ionic or covalent bonds.

Polar Molecular Solids

Polar molecular solids have a structure such that one side has a negative charge and the other side has a positive charge. They are held together by dipole-dipole forces of attraction. Their melting and boiling points are higher than non-polar molecular solids but still relatively low. Examples include water and carbon tetrachloride.

Hydrogen-Bonded Molecular Solids

Hydrogen-bonded molecular solids are characterized by strong intermolecular hydrogen bonds. They have higher boiling and melting points compared to polar and non-polar molecular solids. At room temperature and pressure, they exist as volatile liquids or soft solids. A common example is H2O2 (hydrogen peroxide).

1. Ionic Solids

Ionic solids are crystalline solids whose constituent particles are anions (negatively charged) and cations (positively charged). They are held together by strong electrostatic forces and have high melting and boiling points. They are soluble in polar solvents but not in non-polar solvents. An example is table salt (NaCl).

2. Covalent or Network Solids

Covalent solids are those in which atoms are held together by covalent bonds. This results in a giant molecule formed by a network of interconnected covalent bonds throughout the crystal. They have high melting and boiling points and are generally poor conductors, with the exception of graphite.

3. Metallic Solids

Metallic solids are those in which the constituent particles are metal atoms. These atoms lose their valence electrons, resulting in positively charged ions. These ions are held together by the sea of delocalized electrons, which can move freely throughout the crystal. This results in high thermal and electrical conductivity. All metals and alloys fall into this category.

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Frequently Asked Questions

Glass is a non-crystalline amorphous solid, often translucent, that has widespread practical, technical, and decorative use in window panes, tableware, and optics, for example. Glass is most commonly formed by the molten form’s accelerated cooling (quenching); other glasses exist spontaneously, such as volcanic glass.

An amorphous solid is a solid which lacks an ordered internal structure, unlike a crystalline solid. Rubber, silicone, and gels provide several examples of amorphous solids. The physical properties of amorphous solids are the same in both directions, unlike crystalline solids that have normal cleavage planes.

There are well-defined edges and faces of crystalline solids, diffract X-rays, and appear to have sharp melting points. Amorphous solids, on the other hand, have irregular or curved surfaces, do not have well-resolved x-ray diffraction patterns, and melt over a wide temperature spectrum.

Inherently, Amorphous is less effective than crystalline, being just around 7-10% efficient in light transfer relative to a crystalline panel of the same scale that usually has 12-15% efficiency. By contrast, over its life, crystalline remains at around 95 percent of its reported operational performance.

In their arrangements, amorphous solids do not have any order. There are four types of crystalline solids: ionic solids-Positive and negative ions are formed and electrostatic attractions are retained together. They are distinguished in the solid state by very high melting points and brittleness and are weak conductors.
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