Ch. 13 States of Matter Need I to Know Fuzzy
Learn 1. Describe the assumptions of the kinetic theory as it applies to solid, liquids, and gases.
2. Define the relationship between Kelvin temperature and average kinetic energy.
3. Identify the conditions for freezing, melting, evaporation, condensation, boiling, and sublimation.
4. Describe the equilibrium between a liquid and its vapor.
5. Describe how equilibrium conditions are represented in a phase diagram.
13.3 Liquids and SolidsGas Liquid Solid
Shape(e.g. fixed or not fixed)
Volume(e.g. definite or indefinite)
Density(relatively high, medium, or extremely low)
Compressibility(e.g. relatively high, low, or extremely low)
Fluidity(e.g. flows or does not flow)
Not fixed Not fixed
Definite Definite
Extremely low
Relatively high
LowExtremely low
flows does not flow
Diffusion(e.g. rapid, medium, or none)
rapid medium none
Kinetic Theory and the Nature of Gases
What is kinetic energy?energy of motion
The Kinetic Theory states:1) Matter is composed of _________.2) The particles move _____ in constant random motion.3) All collisions are perfectly __________.
Gas PressureWhat causes pressure?
result of _________ of particles
What is a vacuum?no _________ in a empty space
Atmospheric PressureWhat instrument measures atmospheric pressure?
____________
There are a variety of units used for pressure
SI unit - 101.3 kPa (____________)
other units of __________ pressure at sea level760 mm Hg = 29.9" (weatherman)760 torrs1 atm (atmosphere)14.8 psi (pounds per square inch - tires)
Conversion of PressureHow many kilopascals (kPa) in 1.5 atm?
1.5 atm |__________| = | |
1.5 atm | 101.3 kPa | = ________ kPa | 1 atm |
Kinetic Energy and Kelvin Temperature
What is meant by average Kinetic Energy?
Not all __________ are moving exactly the same speed
If Kinetic Energy increases, how will it effect the temperature?
> K.E. > temperature
What is absolute zero? (0 K = -273 oC) all particles stop __________
K.E. and temp. are directly related to the Kelvin scale.100 K --> 200 K
x K.E. = 2x K.E.
Standard TemperatureStandard temperature is 0oCWhat is STP?
Standard Temperature and Pressure0oC and 101.3 kPa
Remember ______ L of any gas at STP
The Nature of LiquidsLiquids and gases flow, but liquids are more strongly attracted by intermolecular forces.
Liquids cannot be ______________.
Evaporation or VaporizationWhat is evaporation?
The conversion of a liquid to a gas below its normal boiling point.
Only molecules with certain amount of K.E. can _______ from the surface.
Evaporation is known as a ________ process.Why?molecules with the highest amount of K.E. escape, leaving the molecules with the lowest K.E. behind.
Ex. perspiration sweat with higher K.E. evaporates, leaving cooler sweat, which cools you off
Evaporation in a closed containerEvaporation in a closed container
ex. terrariumparticles collide with the walls of a sealed container and produce a vapor pressure above the liquid.
What is dynamic equilibrium? ____________ rate = ___________ rate
increase temperature --> increases vapor pressure
Boiling Point of a LiquidWhen does a liquid boiling?
Boiling point occurs when the ______ pressure equals external air pressure.
bubbles form because the pressure _____ the bubbles equals the ____ pressure.
What is normal boiling point? refers to the boiling point at standard pressure.
Boiling point decreases as external air pressure decreases
sea level = 100oCDenver = 95oCMt. Everest = 60oC
SolidsAre solid particles moving?
vibrating about a fixed point
Solids are dense and incompressibleWhat is melting point?
temp. at which a solid turns into a liquid
solid melting> liquid<freezing
Type of Solid
Unitparticles
Characteristics Examples
Molecular
Covalent Network
Ionic
Metallic
_________Atoms connected by______ bonds
_______
Atoms surrounded by mobile valence e-
Very soft, very low melting point and poor conductivity
Fairly soft, low melting point, and poor conductivity
Very hard, high melting point, and poor conductivitySoft to hard, low to high melting point, and excellent conductivity
I2, H2O, NH3, CO2, C12H22O11
Diamond and quartz
NaCl, KBr, CaCO3
All metallic elements
Forces
Inter-molecular
Intra-molecularIntra-molecularIntra-molecular
Solid - CrystalsWhat are crystals?
atoms, ions, or molecules are arranged in an orderly, repeating 3D pattern
lattice - array of _______unit cell - smallest group of particles
within a crystal that retains the ________ shape
AllotropesWhat is an ___________?
2 or more different molecular forms of the same _________ in the same physical state
Ex. carbon diamond - 4 Cgraphite - 6 Cbuckey balls - 60 C
Ex. arsenic gray or white
AmorphousWhat is Amorphous? solids _______ an order to their internal
structureex. rubber, plastic, glass
glass is supercooled, no definite melting point, it gradually softens when heated
SublimationWhat is sublimation?
change a substance from a solid to a gas or vapor without passing through the _____ state
Ex. iodine, air fresheners, moth balls
Ex. dry ice --> CO2
Phase DiagramShows the relationship between the solid, liquid, and gas state and how temp and pressure affects them.
What is triple point? all _______phases can exist at equilibrium
Water Phase Diagram
PlasmaPlasma: The Fourth State of Mattergaseous mixture of electrons and positive
ions
partial plasma ex. fluorescent light, lightening bolts,
neon signs
"cold plasma" 50,000 -100,000 K"hot plasma" 10,000,000-1,000,000,000 K
(stars)