Properties of solid

• Solids are like liquids in that particles are in contact with one another
• Intermolecular forces in solids are strong enough to hold the particles in place
• All substances are solids at low enough temperatures, except helium
• The temperature at which the solid state becomes the stable phase varies widely among substances
• Solids maintain their shape and do not fill their entire containers like gases
• Solids cannot be easily compressed like gases and have relatively high densities
• Crystalline solids have a regular, repeating three-dimensional structure
• Ionic crystals are composed of ions held together by the attraction of opposite charges
• Ionic solids have high melting points and are typically very brittle
• Examples of ionic crystals include NaCl, KCl, and MgCl2
• Covalent crystals are composed of atoms covalently bonded together in a never-ending fashion
• Covalent network solids are poor conductors of electricity and have high melting points
• Examples of covalent network solids are diamond and silicon dioxide (SiO2)
• Molecular crystals are composed of covalently bonded molecules
• Molecular solids typically melt at lower temperatures and are softer than ionic solids
• Ice is an example of a molecular solid
• Metallic crystals have the characteristic properties of metals and exhibit metallic bonding
• Metallic solids are good conductors of heat and electricity
• Metallic elements usually form cations when they make compounds
• Amorphous solids have no long-term structure or repetition
• Examples of amorphous solids include glass and many plastics
• Amorphous solids do not have sharp melting points and tend to break along curved surfaces
• Phase changes involve matter transitioning between gas, liquid, and solid states
• Adding heat to a substance in processes like melting, vaporization, and sublimation is endothermic
• Removing heat from a substance in processes like freezing and condensation is exothermic
• The melting point is the temperature at which a substance goes from a solid to a liquid
• The boiling point is the temperature at which a substance goes from a liquid to a gas
• Different equilibriums include liquid-vapor, liquid-solid, and solid-vapor equilibriums
• Molar heats of vaporization, condensation, fusion, freezing, and sublimation are involved in phase changes
• The molar heat of sublimation is the amount of energy needed to turn a solid directly into a gas
• Heating and cooling curves and phase diagrams are used to represent phase changes
• At low enough temperatures, all substances are solids except for helium
• The temperature at which the solid state becomes the stable phase varies widely among substances
• Solids cannot be easily compressed like gases and have relatively high densities
• Crystalline solids have a regular, repeating three-dimensional structure
• Ionic crystals are composed of positively charged ions (cations) and negatively charged ions (anions) arranged in a regular three-dimensional lattice structure
• Ionic solids have high melting points due to strong electrostatic forces of attraction (ionic bonds)
• Ionic solids are typically very brittle
• Covalent network solids are composed of atoms covalently bonded together in a never-ending fashion
• Examples of covalent network solids are diamond and silicon dioxide (SiO2)