13+States+of+Matter

== =Outline 13.1= **Question** Energy an object has due to its motion //Kinetic// **Question** Matter consists of tiny particles in constant motion is called //Kinetic Theory// The particles in a gas are considered to be //Small and Hard Spheres// The motions of the particles in a gas are //Rapid, Constant, and Random// All collisions between particles in a gas are //Perfectly elastic// Force exerted by gas per unit of surface area is called //Gas pressure// An empty space with NO particles and NO pressure is called a //Vacuum// A device used to measure atmospheric pressure is called a //Barometer// The SI unit of pressure is called the //Pascal//
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1 atmosphere = 760mm Hg = 760 torr = 101.3 KPa = 101,300 Pa = 15 pounds per square inch.

Outline 13.2
13.2 The Nature of Liquids What factors can determine the physical properties of a liquid? Substances that can flow are referred to as liquids. Both liquids and gases are fluids. True or False? True. The interplay between the disruptive motions of particles in a liquid and the attractions among the particles determines the physical properties of liquid. What is the relationship between evaporation and kinetic energy? Evaporation using kinetic energy is called vaporization. Vapor pressure is a measure of the force exerted by a gas above a liquid. Increased temperature at a contained liquid increase the vapor pressure.

Outline 13.3
Outline 13.3 The Nature of Solids A Model for Solids Key Point Number One: The general properties of solids reflect the orderly arrangement in their particles and the fixed the locations of their particles. Key Point Number Two: The shape of a crystal reflects the arrangement of the particles. Melting point- Solid to liquid. Crystal- Arranged orderly, repeating and 3-D is called a lattice. Allotropes- Two or more different molecular forms of the same element in the same physical state. Amorphous Solid lacks an ordered internal structure. Glass- A transparent fusion produt of inorganics to a liquid. =Objectives= 13.1 13.2 13.3 13.4
 * What are the three assumptions of the kinetic theory as it applies to gasses?
 * How does kinetic theory explain gas pressure?
 * What is the relationship between the temperature in kelvins and the average kinetic energy of particles?
 * What factors determine the physical properties of a liquid?
 * What is the relationship between evaporation and kinetic energy?
 * When can a dynamic equilibrium exist between a liquid and its vapor?
 * Under what conditions does boiling occur?
 * How are the structure and properties of solids related?
 * What determines the shape of a crystal?
 * When can sublimation occur?
 * How are the conditions at which phases are in equilibrium represented on a phase diagram?

=Outlined Notes=
 * 13.1 The Nature of Gases

I.** __**Kinetic Theory and a Model for Gases**__ __**B. Kinetic Theory**__ - All matter consists of tiny particles that are in constant motion.
 * __A. Kinetic Energy__** - Energy an object has because of its motion.
 * 1.)** The particles in a gas are considered to be smal hard spheres with an insignificant volume.
 * 2.)** The motion of the particles in a gas is rapid, constant, and random.
 * 3.)** All collisions between particles in a gas are perfectly elastic.

__**B. Atmospheric Pressure**__ - Collisions of atoms and molecules in air with objects. __**C. Vaccum**__ - An empty space with no particles and no pressure. __**D. Barometer**__ - Device used to measure atmospheric pressure. __**E. Pascal(Pa)**__ - SI unit of pressure. __**F. Standard Atmosphere(atm)**__ - Pressure required to support 760mm of mercury in a mercury barometer at 25°C. 1.) Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object.
 * II.** __**Gas Pressure**__
 * __A. Gas Pressure__** - Force exerted by a gas per unit surface area of an object.


 * 13.2 The Nature of Liquids**

A.** The interplay between the disruptive motions of particles in a liquid and the attractions amoung the particles determines the physical properties of the liquid.
 * I.** **__A Model for Liquids__

A.__** __**Vaporization**__ **-** The conversion of a liquid to a gas or vapor.
 * II. __Evaporation
 * __B. Evaporation__** - When such a conversion occurs when the liquid is not being boiled.
 * 1)** During evaporation, only molecules with a certain minimum kinetic energy can escape from the surface of the liquid.

A. Vapor Pressure__ -** the measure of the force exerted by a gas above a liquid.
 * III.** **__Vapor Pressure
 * __B.__** In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium because the rate of evaporation equils the rate of condensation.
 * __C.__** An increase in temperature of a contained liquid increases the vapor pressure.

A. Boiling Point-__** Temperature at which the vapor pressure is equil to the external pressure of a liquid.
 * IV. __Boiling Point
 * __B. Normal Boiling Point-__** Boiling point of a liquid at a pressure of 101.3 kPa.


 * 13.3 The Nature of Solids

A. __A Model for Solids__** 7. The shape of the crystal depends on the arrangement of particles within it 8. The smallest group of particles within a crystal that retains the geometric shape of the crystal is a **__unit cell__** 9. A **__crystal lattice__** is a repeating array of any one of fourteen kinds of unit cells 10. __**Allotropes**__ 11. **__Non-Crystalline Solids__**
 * 1) **The general properties of solids reflect the orderly arrangement of their particles and the fixed locations of their particles**
 * 2) Since the particles in solids tend to vibrate about fixed points, solids don't flow
 * 3) When you heat a solid and kinetic energy increases, it's particles vibrate more rapidly
 * 4) __**Melting Point**__ - The temperature at which a solid changes into a liquid
 * 5) At this temperature the disruptive vibrations of particles are strong enough to overcome the attractions holding them in fixed positions
 * 6) Melting and freezing points of a substance are the same temperature and at that temperature the liquid and solid phases are in equillibrium
 * B. __Crystal Structures and Unit Cells__**
 * 1) Most solids are crystalline
 * 2) In a crystal the particles are arranged in an orderly, repeating, three-dimensional pattern called a **__crystal lattice__**
 * 3) **The shape of a crystal reflects the arrangment of particles within the solid**
 * 4) The type of bonding that exists between particles in crystals determine their melting points
 * 5) Not all solids melt when heated, some decompose
 * 6) **__Crystal Systems__**
 * A crystal has sides or faces
 * The angles at which the faces intersect are always the same for a given substance
 * Crystals are classified into seven crystal systems: cubic, tetragonal, orthorhombic, monoclinic, triclinic, hexagonal, rhombohedral
 * Some solid substances can exist in more than one form
 * **__Allotropes__** - two or more different molecular forms of the same element in the same physical state
 * Though they are composed of atoms of the same elements, but they have different properties
 * Some solids are amorphous
 * An amorphous solid lacks ordered internal structure
 * Atoms are randomly arranged
 * **__Glass__** - transparent fusion product of inorganic substances that have cooled to a rigid state without crystallizing


 * 13.4 Changes of Matter

A. __Sublimation__**
 * 1) **__Sublimation__** - a change of substance from solid to vapor without melting and passing to the liquid state
 * 2) **Occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature**
 * 3) **An example of sublimation would be dry ice [[image:http://www.ligo-wa.caltech.edu/graphics/dryice.jpg width="280" height="176"]]**
 * B. __Phase Diagrams__**
 * 1) **__Phase Diagram__** - graphs the relationships among the solid, liquid, and vapor states of a substance; gives the conditions of temperature and pressure at which a substance exists as a solid, liquid, and gas
 * 2) **The conditions of pressure and temperature at which two phases exist in equilibrium are indicated on a phase diagram by a line separating the phases**
 * 3) **__Triple Point__** - where all three curves meet; describes the only set of conditions at which all three phases can exist in equilibrium with one another
 * 4) The temperature of water is 0.017*C and the pressure is 0.61 kPa
 * 5) A decrease in pressure lowers the boiling point and raises the melting point
 * 6) An increase in pressure raises the boiling point and lowers the melting point

=Reference Pages=



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Sodium Chloride Crystal Lattice







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