Sugar and water-ice are common examples of a molecular solid. In general terms, a molecular solid is held together by Van Der Waals forces (bonds) which are rather weaker than ionic or covalent bonds.
molecular solids
Molecular solids are generally not malleable. They consist of molecules held together by weak intermolecular forces, such as van der Waals forces or hydrogen bonds, which do not allow for significant deformation without breaking. Instead, when subjected to stress, molecular solids are more likely to shatter or break rather than bend or deform like metals. This brittleness is a characteristic feature of many molecular solids.
You think probable to a glass.
It can be categorised into -Ionic -Covalent molecular -Metallic -Covalent network
At room temperature, the elements that exist as gases include hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine, argon, krypton, xenon, and radon. These elements are primarily nonmetals and noble gases, characterized by low molecular weights and weak intermolecular forces. Their gaseous state at room temperature is a result of their molecular structure and the energy of their particles, which allows them to remain in a gaseous form rather than condensing into liquids or solids.
Molecular solids
Ionic solids are typically harder than molecular solids because ionic bonds are stronger than intermolecular forces found in molecular solids. The ionic bonds in ionic solids result from the attraction between positively and negatively charged ions, contributing to their higher hardness compared to molecular solids, which are held together by weaker intermolecular forces.
The solid carbon compounds are mostly molecular solids.
molecular solids
Molecular solids have lower boiling points than ionic solids because the intermolecular forces between molecules in a molecular solid are weaker than the electrostatic forces between ions in an ionic solid. As a result, less energy is required to break apart the molecular interactions and transition to the gaseous phase in molecular solids compared to ionic solids with stronger ionic bonds.
Network solids have a three-dimensional structure with strong covalent bonds throughout, leading to a higher melting point compared to molecular solids which have weaker intermolecular forces. In network solids, a larger amount of energy is required to break the extensive network of covalent bonds, resulting in a higher melting point.
Yes. About 74% of the elements are metals and are generally solids.
Molecular solids are generally not malleable. They consist of molecules held together by weak intermolecular forces, such as van der Waals forces or hydrogen bonds, which do not allow for significant deformation without breaking. Instead, when subjected to stress, molecular solids are more likely to shatter or break rather than bend or deform like metals. This brittleness is a characteristic feature of many molecular solids.
Very much higher.
You think probable to a glass.
Ionic solids generally have higher melting points compared to molecular solids. This is because in ionic solids, strong electrostatic forces hold the ions together in a rigid lattice structure, requiring more energy to break these bonds and melt the substance. Molecular solids, on the other hand, are held together by weaker intermolecular forces, resulting in lower melting points.
It is true, all are solids.