Properties of Liquids PDF

Properties SURFACE TENSION Phenomenon that occurs because of cohesive forces (attractions) between liquid molecules allows liquid to resist an external force due to cohesive of water molecules VISCOSITY Quantity that describes a fluid's resistance to flow; also called...

Properties SURFACE TENSION Phenomenon that occurs because of cohesive forces (attractions) between liquid molecules allows liquid to resist an external force due to cohesive of water molecules VISCOSITY Quantity that describes a fluid's resistance to flow; also called Dynamic/Absolute/Simple Viscosity Kinematic Viscosity - fluid's resistance to flow under gravitational forces VISCOSITY HIGH VISCOSITY; LOW VISCOSITY; STRONG IMF WEAKER IMF CAPILLARITY Refers to how a liquid can rise or fall in a small space that is wet or dry, and is caused by the intermolecular forces. When the adhesion force between the liquid and solid (pipe wall) exceeds the liquid's cohesion, the capillary rise phenomenon occurs. The narrower the tube, the higher will the liquid rise  VAPOR PRESSURE Pressure exerted by a gas/vapor in a equilibrium with its condensed phase (solid or liquid) in a closed system at a given temperature BOILING POINT temperature at which vapor pressure equals the surrounding atmospheric pressure. *different substances have different vapor pressures and therefore different boiling points. MOLAR HEAT OF VAPORIZATION energy required to transform a given quantity of a substance from liquid into gas at a given pressure Structure and Properties of Water  SOLID ✓ definite shape and volume ✓ rigid; can't compressed easily ✓ can't diffuse to another solid ✓ doesn't flow and can be stored in contained ✓ heating solid changes into liquid  SOLID ❑ Amorphous solids ✓ Solid without form, no repeating lattice pattern. ✓ also called “pseudo solids”. ✓ It melts gradually because bonds do not break all at once (like candle) ✓ Edges may be curved when cut  TYPES OF CRYSTALLINE SOLIDS  COVALENT SOLIDS ✓ There are no individual molecules. ✓ They are COVALENTLY BONDED IN A CONTINUOUS NETWORK result in huge crystals. ✓ Very hard and extremely high melting points. ✓ Do not dissolve in water and don't conduct electricity (like the DIAMOND) MOLECULAR SOLIDS ✓ Covalently bonded molecules attracted to each other by electrostatic force (Van der Waals) ✓ Shared electrons spend more time in electron clouds of larger atom causing weak or shifting polarity. ✓ Most are nonpolar that can't dissolve in water but rather in benzene or octane. ✓ Polar solid molecules like sugar can dissolve in water. METALLIC SOLIDS ✓ Opaque and lustrous that are malleable and ductile. ✓ The electron clouds of near atoms overlap so that electron becomes delocalized. The electron move with relative freedom from one atom to another. ✓ The electron mobility tells that they are good conductors of heat and electricity. ✓ Have high melting points except mercury and phosphorus. PETA: Create a 3D model of the following types of crystalline solid: Group 1: Ionic solid Group 2: Covalent solid Group 3: Molecular solid Group 4: Metallic solid