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Solids can be classified on the basis of the bonds that hold the atoms or molecules together. Gasses don`t have a definite volume and occupy all the available space. Because these interactions are relatively weak, molecular solids tend to be soft and have low to moderate melting points. The kinetic molecular theory of gases can help us understand their properties. Key Difference – Ionic vs Molecular Solids. As you should remember from the kinetic molecular theory, the molecules in solids are not moving in the same manner as those in liquids or gases. Physical properties are governed by the intermolecular forces - forces attracting one molecule to its neighbours - van der Waals attractions or hydrogen bonds. Solid state means, the atoms, molecules or ions in that substance are tightly packed, avoiding the movement of those chemical species (unlike in … Solid substances are compounds that exist in a solid state at a given temperature and pressure. Interest in organic molecular solids extends to a range of fields including chemistry, physics, electrical engineering, and materials science. In chemistry, it applies to such topics as solid state reactivity, crystal engineering, theoretical approaches to crystal structure determination, and morphology control. Molecular substances tend to be gases, liquids or low melting point solids, because the intermolecular forces of attraction are comparatively weak. Molecular Solids . Metallic solids: Solids in which molecules are held by metallic bonds i.e. Let us look at the general properties of gases, liquids, and solids. Molecular solids are composed of discrete molecules held together by intermolecular forces. This approach categorizes solids as either molecular, covalent, ionic, or metallic. The main types of crystalline solids are ionic solids, metallic solids, covalent network solids, and molecular solids. Properties of Solids . The volume of a gas is the volume of the container. Chemical bonding - Chemical bonding - Molecular solids: The structures of molecular solids, which are solids composed of individual molecules, have also been touched on in the section on intermolecular forces. Melting and boiling points. Covalent molecules held together by intermolecular forces form molecular solids. Non conductor of electricity Example: Solid SO 2, Solid NH 3, HCl 3. Molecular solids are also poor conductors of electricity because their valence electrons are tightly held within each individual molecule. While the intermolecular forces are strong enough to hold the molecules in place, molecular solids typically have lower melting and boiling points than metallic, ionic, or network atomic solids, which are held together by stronger bonds. electrons are free and evenly spread out throughout the crystal. The properties of the different kinds of crystalline solids are due to the types of particles of which they consist, the arrangements of the particles, and the strengths of the attractions between them. The key difference between molecular solid and covalent network solid is that molecular solid forms due to the action of Van der Waal forces whereas covalent network solid forms due to the action of covalent chemical bonds.. We can categorize solid compounds in different ways – depending on the structure, composition, bonding, properties, applications, etc. Solid molecules simply vibrate and rotate in place rather than move about. Properties of gases. Iodine (I 2), sugar (C 12 H 22 O 11), and polyethylene are examples of compounds that are molecular solids at room temperature. You'll learn the properties of solids and liquids, discover the types of intermolecular attractions that occur between them and gain an understanding how phase changes happen. 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