Molecular solids are crystalline materials with distinct molecules arranged in repeating patterns, held by intermolecular forces like van der Waals forces, dipole-dipole interactions, and hydrogen bonds. These forces influence their melting points, hardness, and solubility. Molecular solids are categorized by the dominant intermolecular force, affecting their physical properties and conductivity.
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Molecular solids are crystalline materials where discrete molecules are arranged in a well-defined, repeating pattern
Types of Intermolecular Forces
The primary types of intermolecular forces in molecular solids are van der Waals forces, including London dispersion forces, dipole-dipole interactions, and hydrogen bonds
Influence on Physical Properties
The strength and nature of the intermolecular forces dictate the physical properties of molecular solids, such as their melting points, hardness, and solubility
Molecular solids can be categorized based on the dominant intermolecular force present, such as non-polar, polar, and hydrogen-bonded solids
The crystalline structure of a molecular solid is influenced by the symmetry and directionality of its intermolecular forces
Orthorhombic Lattice
Non-polar molecular solids, like solid iodine, form an orthorhombic lattice structure due to London dispersion forces
Hexagonal Lattice
Polar molecular solids, such as ice, form a hexagonal lattice structure due to hydrogen bonding, resulting in a lower density compared to liquid water
The type and strength of the intermolecular forces present in molecular solids largely determine their physical properties, such as softness, low melting and boiling points, and low density
Electrical Conductivity
Molecular solids are poor conductors of electricity due to the absence of free-moving charged particles
Thermal Conductivity
The thermal conductivity of molecular solids is low due to the loosely held molecules in the lattice structure
Molecular solids are generally softer and less dense than ionic or metallic solids
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Types of van der Waals forces in molecular solids
Include London dispersion forces, dipole-dipole interactions, hydrogen bonds.
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Impact of intermolecular forces on molecular solids' properties
Determine melting points, hardness, solubility.
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Nature of intermolecular vs. intramolecular forces
Intermolecular are weaker, electrostatic; intramolecular are stronger, covalent or ionic.
