Liquids and Solids.

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Presentation transcript:

Liquids and Solids

Characteristics of Liquids and Solids What properties allow you to classify a substance as a solid, liquid, or gas?

Property Solid Liquid Gas Volume Shape Relative density Compressibility Fluid? Space between particles Diffusion rate Motion of particles (amount and type) Forces between particles?

Surface Tension Surface tension is the tendency for liquid surface to contract. Depends on IMFs Compounds that interfere with the IMFs and reduce surface tension are called surfactants.

The molecular basis of surface tension. Figure 12.18 The molecular basis of surface tension. the net vector for attractive forces is downward hydrogen bonding occurs across the surface and below the surface hydrogen bonding occurs in three dimensions

stronger cohesive forces Figure 12.19 Shape of water or mercury meniscus in glass. capillarity stronger cohesive forces adhesive forces H2O Hg

Liquid-gas equilibrium. Figure 12.4 Liquid-gas equilibrium.

Vapor pressure as a function of temperature and intermolecular forces. Vapor pressure = the pressure of the vapor resulting from evaporation of a liquid (or solid) above a sample of the liquid (or solid) in a closed container What factors affect the vapor pressure? Figure 12.6 Vapor pressure as a function of temperature and intermolecular forces.

Boiling Point Temperature at which the vapor pressure of the liquid = atmospheric pressure Normal boiling point vpliquid = 760 mmHg condensing point = boiling point

What if…? You are camping at a high altitude of 10,000 ft where the atmospheric pressure is 535 mmHg. If you boil an egg for 10 minutes will it be hard-boiled just right, overdone, or runny? Explain your choice.

Subliming Point Temperature at which the vapor pressure of the solid equals atmospheric pressure Depositing point = subliming point Iodine subliming

Dipole moment and boiling point. Figure 12.12 Dipole moment and boiling point.

Hydrogen bonding and boiling point. Figure 12.13 Hydrogen bonding and boiling point.

Molecular shape and boiling point. Figure 12.16 Molecular shape and boiling point. fewer points for dispersion forces to act more points for dispersion forces to act

Freezing Point Temperature at which liquid and solid are in equilibrium Not affected by pressure but does depend on IMFs and molar mass Melting point = freezing point

The hexagonal structure of ice. Figure 12.21 The hexagonal structure of ice.

The striking beauty of crystalline solids. Figure 12.22 The striking beauty of crystalline solids.

The crystal lattice and the unit cell. Figure 12.23 The crystal lattice and the unit cell. lattice point unit cell portion of a 3-D lattice portion of a 2-D lattice unit cell

Diffraction of x-rays by crystal planes. Figure 12.27 Diffraction of x-rays by crystal planes.

Table 12.5 Characteristics of the Major Types of Crystalline Solids Interparticle Forces Physical Behavior Particles Examples (mp,0C) Atomic Atoms Dispersion Soft, very low mp, poor thermal & electrical conductors Group 8A(18) [Ne-249 to Rn-71] Molecular Molecules Dispersion, dipole-dipole, H bonds Fairly soft, low to moderate mp, poor thermal & electrical conductors Nonpolar - O2[-219], C4H10[-138], Cl2 [-101], C6H14[-95] Polar - SO2[-73], CHCl3[-64], HNO3[-42], H2O[0.0] Ionic Positive & negative ions Ion-ion attraction Hard & brittle, high mp, good thermal & electrical conductors when molten NaCl [801] CaF2 [1423] MgO [2852] Metallic Atoms Metallic bond Soft to hard, low to very high mp, excellent thermal and electrical conductors, malleable and ductile Na [97.8] Zn [420] Fe [1535] Network Atoms Covalent bond Very hard, very high mp, usually poor thermal and electrical conductors