kinetic molecular models of liquids and solids

• Surface tension is the amount of resistance needed to increase the surface area of liquids, created by the cohesive force between molecules.
• The stronger the intermolecular forces, the higher the viscosity of a liquid.
• Short range order is a regular pattern of arrangement of constituent particles.
• Between glass and water, glass has a lower specific capacity.
• Hydrogen is bonded with a F element.
• A force between a cation and a partially negatively charged ion is called an ion-ion interaction.
• Viscosity is the measure of a liquid’s resistance to flow, strongly dependent on the strength of a intermolecular force, with the stronger the intermolecular forces, the higher the viscosity of a liquid.
• Boiling point is the temperature at which its vapor pressure is equal to the external or atmospheric pressure, influenced by the existing intermolecular force, with the stronger the intermolecular force, the higher the boiling point of the liquid.
• Vapor pressure is the pressure of the vapor present at a equilibrium, with liquids having high vapor pressure having weak intermolecular forces, they exhibit volatility and readily evaporate from an open vessel, it increases with increasing temperature due to high kinetic energy of liquid particles causing it to break the intermolecular forces, to undergo evaporation/vaporization.
• Molar heat of vaporization is the amount of heat required to vaporized one mole of a substance at its boiling point.
• Cohesion refers to the attraction of molecules for other molecules of the same kind and water has a strong cohesive force to form hydrogen bonds.
• Adhesion refers to the attraction of molecules for other molecules of a different kind.
• Water has a large heat of vaporization which helps in regulating the temperature of Earth’s surface from the sun’s energy, and maintaining human body’s temperature through perspiration.
• Ice is less dense than water so it floats on the surface of water.
• Density is the mass per unit volume of a substance and water’s lower density in its solid form is due to the way hydrogen bonds are oriented as it freezes.
• Heat disrupts the intermolecular forces as molar heat vaporization increases.
• Water is hydrophilic as a polar substance interacts with and dissolves in water.
• Standard Heat of Vaporization is the energy required to vaporize 1 mole of liquid at 101 325 Pa.
• The density of water is 1 g/cm3; the density of ice is 0.0968
• Water is hydrophobic as nonpolar molecules like oils and fats do not interact with water and separate from it.
• Water is a universal solvent as water molecules are attracted to other polar molecules and to ions.
• Unit Cell is the smallest repeating unit of lattice.
• Amorphous solids have a random, disordered arrangement, short range order of regular pattern of arrangement of constituent particles, they gradually soften when they are heated and melt a wide range of temperatures, examples include glass, charcoal, and plastic containers.
• Specific Heat Capacity (C) is the amount of heat needed to raise the temperature of one gram of a substance by one degree Celsius.
• Space Lattice is the three-dimensional pattern formed by the points representing the location of these particles, it is the basic structure of the crystal.
• Heat of Vaporization is the amount of energy needed to change one gram of a liquid substance to a gas at constant temperature.
• Crystalline solids have a regular, highly ordered arrangement, long range order of regular pattern of arrangement of constituent particles, examples include amethyst, fluorite, and pyrite.
• Water has a high specific heat capacity which prevents bodies of water from generating large changes in their temperature conditions.
• Substance Specific Heat Capacity (J/kg^1.C^1) values are: Water 4200, Alcohol 2400, Sand 840, Granite 800, Ice 2100, Glass 670, Copper 390, Iron 460.