State of Matter
States of Matter
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Solid
Molecules are tighly packed and harder than liquids and gases.
Examples: Ice, Coal, Salt
Amorphous solid-a solid which has a disordered atomic structure.
Examples: Glass, Rubber
Liquids flowing freely but of constant volume.
Examples: Water, Mercury, Alcohol
Viscosity-a measure of its resistance to gradual deformation by shear stress or tensile stress.
Surface tension-the force that acts on the surface of a liquid and tends to minimize the surface area. Surface tension can be broken by adding soap to water.
Gases
An airlike fluid substance which expands freely to fill any space available, irrespective of its quantity.
Examples: Water vapor, Hydrogen, Oxygen
Plasma seen in ionized gases distinct from a gas because it possesses free electrical charges (not bound to atoms or ions) cause plasma to be electrically conductive.
Examples: Stars, Lightning, fluorescent lights
Melting(Endothermic)
Become liquefied by heat.
Melting point-the temperature at which the solid melts to become a liquid. Endothermic
Freezing point-temperature at which they turn into solids. Exothermic
Vaporization (Endothermic)
Annihilation by vaporizing something.
Volatile-Easily evaporated at normal temperatures.
Boiling point-The temperature at which a liquid boils and turns to vapor. (Increase the pressure can change the boiling point.
Condensation-The process of becoming more dense, in particular. (Exothermic) Dynamic equilibrium- the rate of the forward/reverse reactions are equal.
Sublimation (Endothermic) the transition from the solid phase to the gas phase without passing through an intermediate liquid phase.
Decomposition (Exothermic) chemical reaction where one reactant yields two or more products.
Phase Diagrams a chart showing the thermodynamic conditions of a substance at different pressures and temperatures.
Triple point- temperature and pressure at which the solid, liquid, and vapor
Jun Ruan
Solid
Molecules are tighly packed and harder than liquids and gases.
Examples: Ice, Coal, Salt
Amorphous solid-a solid which has a disordered atomic structure.
Examples: Glass, Rubber
Liquids flowing freely but of constant volume.
Examples: Water, Mercury, Alcohol
Viscosity-a measure of its resistance to gradual deformation by shear stress or tensile stress.
Surface tension-the force that acts on the surface of a liquid and tends to minimize the surface area. Surface tension can be broken by adding soap to water.
Gases
An airlike fluid substance which expands freely to fill any space available, irrespective of its quantity.
Examples: Water vapor, Hydrogen, Oxygen
Plasma seen in ionized gases distinct from a gas because it possesses free electrical charges (not bound to atoms or ions) cause plasma to be electrically conductive.
Examples: Stars, Lightning, fluorescent lights
Melting(Endothermic)
Become liquefied by heat.
Melting point-the temperature at which the solid melts to become a liquid. Endothermic
Freezing point-temperature at which they turn into solids. Exothermic
Vaporization (Endothermic)
Annihilation by vaporizing something.
Volatile-Easily evaporated at normal temperatures.
Boiling point-The temperature at which a liquid boils and turns to vapor. (Increase the pressure can change the boiling point.
Condensation-The process of becoming more dense, in particular. (Exothermic) Dynamic equilibrium- the rate of the forward/reverse reactions are equal.
Sublimation (Endothermic) the transition from the solid phase to the gas phase without passing through an intermediate liquid phase.
Decomposition (Exothermic) chemical reaction where one reactant yields two or more products.
Phase Diagrams a chart showing the thermodynamic conditions of a substance at different pressures and temperatures.
Triple point- temperature and pressure at which the solid, liquid, and vapor