Liquids and Solids.

Name: Liquids and Solids.
Uploaded: 2017-08-22T17:34:56+00:00
Duration: PTM14S28
Channel: Lambert Leonard
Description: Liquids and Solids.

Liquids and Solids

Figure 16.1: Schematic representation of the three states of matter
Copyright © Houghton Mifflin Company. All rights reserved.

Bubble Pressure The net upward force on the top hemisphere of the bubble is just the pressure difference times the area of the equatorial circle: The surface tension force downward around circle is twice the surface tension times the circumference, since two surfaces contribute to the force: Copyright © Houghton Mifflin Company. All rights reserved.

毛細現象 The height h to which capillary action will lift water depends upon the weight of water which the surface tension will lift: The height to which the liquid can be lifted is given by Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.7: Nonpolar liquid mercury forms a convex meniscus in a glass tube.

Figure 16.6: A molecule in the interior of a liquid is attracted to the molecules surrounding it, whereas a molecule at the surface of liquid is attracted only by molecules below it and on each side of it. Copyright © Houghton Mifflin Company. All rights reserved.

Classifying Intermolecular Forces
Strong ionic attraction Recall lattice energy and its relations to properties of solid. The more ionic, the higher the lattice energy. Intermediate dipole-dipole forces Substances whose molecules have dipole moment have higher melting point or boiling point than those of similar molecular mass, but their molecules have no dipole moment. Weak London dispersion forces or van der Waal's force These forces alway operate in any substance. The force arisen from induced dipole and the interaction is weaker than the dipole-dipole interaction. In general, the heavier the molecule, the stronger the van der Waal's force of interaction. Hydrogen bond Certain substances such as H2O, HF, NH3 form hydrogen bonds,. Metallic bonding Forces between atom in metallic solids belong to another category. Valence electrons in metals are rampant. They are not restricted to certain atoms or bonds. Rather they run freely in the entire solid, providing good conductivity for heat and electric energy. Copyright © Houghton Mifflin Company. All rights reserved.

Strength of Intermolecular Forces
Covalent bonds > Hydrogen bonding > Dipole-dipole interactions > London forces 400 kcal > 12-16 kcal > 5-0.5 kcal > less than 1 kcal Copyright © Houghton Mifflin Company. All rights reserved.

Dipole-dipole interactions

Figure 16. 2: (a) The electrostatic interaction of two polar molecules
Figure 16.2: (a) The electrostatic interaction of two polar molecules. (b) The interaction of many dipoles in a condensed state. Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.3: The polar water molecule.

Hydrogen Bonds A covalent bond between -O-H ---- :O-
A covalent bond between -N-H----- :O- A covalent bond between F-H :O- A covalent bond between -O-H ---- :N- A covalent bond between -N-H---- :N- A covalent bond between F-H :N- A covalent bond between -O-H :F- A covalent bond between -N-H ---- :F- Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.4: The boiling points of the covalent hydrides of elements in Groups 4A, 5A, 6A, and 7A.

The phase diagram of water is complex
If water behaved more typically as a low molecular weight material, its phase diagram may have looked rather like this: Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.5: An instantaneous polarization can occur on atom a, creating instantaneous dipole.

What Kinds of Materials Form Liquids at Room Temperature
the strength of the bonds between the particles that form the substance (2) the atomic or molecular weight of these particles (3) the shape of these particles Copyright © Houghton Mifflin Company. All rights reserved.

Molecular Shape -130 36.1 -159.9 27.8 -16.5 9.5 Compound
Melting Point (oC) Boiling Point (oC) -130 36.1 -159.9 27.8 -16.5 9.5 Copyright © Houghton Mifflin Company. All rights reserved.

The Shape of the molecule also matters
n-pentane bp= k Copyright © Houghton Mifflin Company. All rights reserved.

Categories of Solids Based on the Solid Pack
Crystalline solids are three-dimensional analogs of a brick wall. They have a regular structure, in which the particles pack in a repeating pattern from one edge of the solid to the other. Amorphous solids have a random structure, with little if any long-range order. Polycrystalline solids are an aggregate of a large number of small crystals or grains in which the structure is regular, but the crystals or grains are arranged in a random fashion. Copyright © Houghton Mifflin Company. All rights reserved.

Categories of Solids Based on Bonds
ionic polar covalent Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.12: Examples of three types of cyrstalline solids.

Figure 16.8: Several crystalline solids

Figure 16.9: Three cubic unit cells and the corresponding lattices.

Figure 16.10: X-rays scattered from two different atoms may reinforce (constructive interference) or cancel (destructive interference) one another. Copyright © Houghton Mifflin Company. All rights reserved.

Figure 16.11: Reflection of X rays of wavelength

A conch shell on a beach. Source: Corbis

Figure 16.13: The closet packing arrangement of uniform spheres.

Figure 16.14: When spheres are closest packed so that the spheres in the third layer are directlly over those in the first layer (aba), the unit cell is the hexagonal prism illustrated here in red. Copyright © Houghton Mifflin Company. All rights reserved.

A section of a surface containing copper atoms (red) and an indium atom (yellow).

Figure 16.15: When spheres are packed in the abc arrangement, the unit cell is face-centered cubic.

Figure 16.16: The indicated sphere has 12 equivalent nearest neighbors.

Figure 16.17: The net number of spheres in a face-centered cubic unit cell.

Volume of a unit cell (2r, 4r, r)

Figure 16.18: In the body-centered cubic unit cell the spheres touch along the body diagonal.

Figure 16.19: The body-centered cubic unit cell with the center sphere deleted.

Figure 16.20: On the face of the body-centered cubic unit cell.

Figure 16.24: A representation of the energy levels (bands) in a magnesium crystal

Figure 16.25: Two types of alloys

Figure 16.26: The structures of (a) diamond and (b) graphite.

Figure 16.27: Partial representation of the MO energies in (a) diamond and (b) a typical metal

Graphite consitst of layers of carbon atoms.

Figure 16.28: The p orbitals (a) perpendicular to the plane of th carbon ring system in graphite can combine to form (b) an extensive pie bonding network. Copyright © Houghton Mifflin Company. All rights reserved.

Electrical Properties
Metallic Conductors, e.g. Cu, Ag... Semiconductors, e.g. Si, GaAs Superconductors, e.g. Nb3Sn, YBa2Cu3O7 Electrolytes, e.g. LiI in pacemaker batteries Piezoelectrics, e.g. a Quartz (SiO2) in watches Copyright © Houghton Mifflin Company. All rights reserved.

Liquids and Solids.

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