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Forces of Attraction, Liquids, Solids, & Phase Diagrams

Forces of Attraction, Liquids, Solids, & Phase Diagrams. Forces of Attraction(13-2). In tra molecular forces – within molecules In ter molecular Forces– attractions between particles (three types) Dispersion Forces – found in all particles/more in larger particles

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Forces of Attraction, Liquids, Solids, & Phase Diagrams

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  1. Forces of Attraction, Liquids, Solids, & Phase Diagrams

  2. Forces of Attraction(13-2) • Intramolecular forces – within molecules • Intermolecular Forces– attractions betweenparticles (three types) • Dispersion Forces – found in all particles/more in larger particles • Dipole – found in polar particles • Hydrogen Bonds – found in polar particles with H bonded to a “FON” element • Greater attractive forces between their particles give substances higher melting/boiling points (i.e. why F2 and Cl2 are gases, Br2 is a liquid and I2 is a solid)

  3. Liquids (13-3) • Surface tension – tendency of a liquid to “hold itself together” (minimize surface area) — this is due to IM forces (COHESION) • Capillary action – movement of liquids up small diameter tubes • cohesive forces – IM forces • adhesive forces – attractive forces between the molecules and a surface or container • Viscosity • measure of a liquids resistance to flow (syrup has a higher viscosity than water) • substances with large IM forces tend to be highly viscous

  4. Figure 4: It is possible to see that in water, the strength of the cohesion forces are larger than the strength of the adhesion forces. This results in the concave formation of water in the capillary tube. This is known as capillary attraction. Alternatively, the adhesion forces are evidently stronger than the cohesion forces which allows the mercury to bend in a convex formation away from the walls of the capillary tube. This is known as capillary repulsion.

  5. Capillary Action

  6. Viscosity

  7. Solids (13-3) • Density of solids –depends on the substance • Types of solids • Crystalline • They have a regular structure, in which the particles pack in a repeating pattern from one edge of the solid to the other. • Ionic (ex: ??) • Molecular (ex: ??) • Atomic • Covalent network (ex: ??) • Metallic (ex: ??) • Noble gases (ex: ??) • Amorphous (ex: ??) • literally, "solids without form") have a random structure, with little if any long-range order. Salt sugar (C12H22O11) Diamond Copper (Ne, Ar, Kr, and Xe) at negative pressure and temperatures below the triple-point temperature Wax

  8. Phase Diagrams (13-4) • Water’s versus carbon dioxide’s • Shows three phases as they exist at different pressure and temperature values (y and x axes) • Lines represent equilibrium between phases (or phase changes) • Which are endothermic / exothermic? • Triple point – equilibrium between all three phases (“boiling ice water”)

  9. Vapor Pressure (13-4) • the tendency of particles in the liquid phase to enter the gas phase at that temperature • open system–continuous evaporation/closed system–equilibrium • VP increases with increasing temp. • a liquid boils when VP = atmos. press

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