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

flowsdoes 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 Pressure

What causes pressure?result of _________ of particles

What is a vacuum?no _________ in a empty space

Atmospheric Pressure

What 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 Pressure

How 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 Temperature

Standard temperature is 0oC

What is STP? Standard Temperature and Pressure

0oC and 101.3 kPa

Remember ______ L of any gas at STP

The Nature of Liquids

Liquids 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

Solids

Are 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-molecular

Intra-molecular

Intra-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

Allotropes

What 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

Sublimation

What 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 Diagram

Shows 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

Plasma

Plasma: 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)