PROPERTIES OF SOLIDS AND LIQUIDS

PROPERTIES OF SOLIDS AND LIQUIDS

brief summary

Liquids and solids differ from gases therein the particles (atoms, molecules, or ions) are much closer together, therefore the total volume of a liquid or solid is far closer to the sum of the volumes of the particles. the quantity of a gas, as you'll recall from the chapter on “The Behavior of Gases,” is said to the quantity of the spaces between the particles and to not the quantity of the particles. At all temperatures above temperature , atoms and molecules are in constant random motion. The particles travel during a line unless they hit another particle. within the absence of any attractive forces, this molecular motion would cause all substances to be in gaseous form. the very fact that solid and liquid states exist tells us that there are forces that hold molecules and atoms together even once they aren't chemically bonded. The forces of attraction that hold atoms and molecules together in solid and liquid phases are called intermolecular forces of attraction. These forces are different from chemical bonds, which are called intramolecular forces. The phase (solid, liquid, or gas) of a substance is that the results of a contest between the molecular motion that pushes the molecules apart and therefore the attractive forces that pull them together. If the molecular motion is far greater than the attractive forces, the substance are going to be gaseous. If the molecular motion is almost an equivalent in strength because the attractive forces, the substance are going to be liquid, and if the molecular motion is far but the attractive forces, the substance are going to be solid. When the molecular motion is increased or decreased by changing the temperature, the connection between the molecular motion and therefore the attractive forces changes, and therefore the substance may change its phase. In the gaseous phase, the molecular motion dominates. The molecules of the substance are completely separated and move about independently of every other. The spaces between the molecules are very large compared to the dimensions of the particles, therefore the measured volume of a gas is really a measurement of the spaces between the molecules. as compared , the molecular structure of the liquid phase has some spaces between the particles that allow the particles to maneuver past each other , but the attraction between the particles is robust enough to stop them from moving very far apart. within the solid phase, the forces of attraction have completely overcome molecular motion, and therefore the movement of the particles has been reduced to vibrating in situ . The particles cannot move past each other and are held during a tightly-packed pattern, so there's little or no space between the particles. Properties of Solids The intermolecular forces of attraction in solids hold the particles so tightly in situ that they can't shy away from one another to expand their volume, nor can they flow past each other to vary shape. Therefore, solids hold their own shape and volume no matter their container. there's little or no empty space within the solid structure, so solids are virtually incompressible. Since molecules cannot pass one another within the structure, diffusion or mixing is actually non-existent beyond the surface layer. Properties of Liquids Attractive forces between molecules are a serious think about the behavior of the liquids. Since the particles during a liquid remain in-tuned with one another , liquids maintain their volume, but since the particles can flow past one another , liquids take the form of their container. 100 mL of liquid are going to be 100 mL in any container, but because the liquid molecules aren't held during a tightly-packed pattern like solids are, the molecules can move past each other , allowing the liquid to suit the form of the container.