FINISHED_Final_Notebook_Jones

Evaporation
Vaporization 9 : The conversion of a liquid to a gas or vapor. | Evaporation 10 : When vaporization occurs
at the surface of a liquid that is not boiling.
Vapor Pressure
Vapor Pressure 11 : The measure of the force exerted by a gas above a liquid.
Boiling Point
Boiling Point(bp) 12 : The temperature at which the vapor pressure of the liquid is just equal to the
external pressure on the liquid. | Normal Boiling Point 13 : Defined as the boiling point of a liquid at a
pressure of 101.3 kPa.
Connection(s): Vaporization occurs when water becomes vapor in a teapot (like referenced in a
previous connection). Evaporation occurs at the surface of the ocean and other various bodies of
water as it shines down, which causes condensation (formation of clouds) and precipitation (rain).
Boiling point is pretty self-explanatory in its connection to the real world, as most people know that the
boiling point of water is approximately 212 o F, which is, obviously, the point at which water boils. The
Normal Boiling Point represents the boiling point of a liquid measured in the previously mentioned
units, Pascals (specifically 101.3 kPa [kilopascals]).
Summary: The interplay between the disruptive motions of particles in a liquid and the attractions
among the particles determines the physical properties of liquids. During evaporation, only those
molecules with a certain minimum kinetic energy can escape from the surface of the liquid. In a
system at a constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid.
When a liquid is heated to a temperature at which the particles throughout the liquid have enough
kinetic energy to vaporize, the liquid begins to boil
13.3 The Nature of Solids
A Model of Solids
Melting Point(mp) 14 : The temperature at which a solid changes into a liquid. | Freezing Point(fp) 15 :
The temperature at which a liquid changes into a solid.
Crystal Structure and Unit Cell
Crystal 16 : The particles in a crystal are arranged in an orderly, repeating, three-dimensional pattern
called a crystal lattice. | Unit Cell 17 : The smallest group of particles within a crystal that retains the
geometric shape of the crystal. | Allotropes 18 : Two or more different molecular forms of the same
element in the same physical state. | Amorphous Solid 19 : Lacks an ordered internal structure. Rubber,
plastic, and asphalt are examples of this. | Glass 20 : A transparent fusion product of inorganic
substances that have cooled to a rigid state without crystallizing.
Connection(s): Melting point can be witnessed when, say, ice melts. However, metals, and other
substances also have melting points, despite how solid they may seem at, perhaps, room
temperature. The freezing point is obviously the opposite of the melting point, and is witnessed when
water turns to ice in a freezer. A crystal or crystalline structure could be graphite, garnets, or gold,
which all have uniform internal patterns. A unit cell is part of these examples of crystals which retain
the geometric shape of the crystal. An example of an allotrope is a diamond, and another is graphite;
these are both different forms of condensed carbon, in the solid state. Amorphous solids are pretty
much anything that isn’t a crystalline solid. An example is glass, which does not achieve a fully
crystalline state, and, when broken, has jagged angles and uneven surfaces. Rubber, plastic, and
asphalt are other examples. A description of glass, which was mentioned earlier, is “a transparent
fusion product of inorganic substances that have cooled to a rigid state without crystallizing.”
Summary: The general properties of solids reflect the orderly arrangement of their particles and the
fixed locations of their particles. The shape of a crystal reflects the arrangement of the particles within
the solid. Allotropes are two or more different forms of the same element, crystalline solids have a
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