UNIT 3 States of Matter

SolidsLiquids

Gases

C4.3 B Describing three states of matter...

Solid - definite shape and volume

Liquid - definite volume, changes shape

Gas - changes shape and volume

Kinetic Molecular Theory

• All matter is made up of small particles.– Which are . . . .

• All of the particles are in constant motion.– Kinetic Energy = KE = ½ mv2

• Collision between particles are perfectly elastic (no energy is lost to the surroundings).

C2.2B Three types of particle motion

• Vibrational - moves around fixed point–solids, liquids, gases

• Translational - particles freely move past one another– liquids, gases

• Rotational - rotates around fixed axis–gases

Solids

• Amorphous –a random arrangement of the

particles with no repeating pattern.–No set melting point–Example: Glass, rubber,

chocolate

Crystalline

• Crystalline –a regular arrangement of the particles

with some kind of repeating pattern producing a crystal.–Known melting point–Crystal shapes are classified according

to their shapes into 7 systems

Crystal Structures (pg 281)

• Cubic• Tetragonal• Orthorhombic• Monoclinic• Triclinic• Hexagonal• Rhombohedral

Diamonds

• Cubic Crystal Structure• The hardest of all known

minerals, can only be scratched by another diamond.

The 4 C’s of Diamonds

• Cut• Color • Clarity • Carat• NOTICE – COST IS NOT A “C”

Cut• The brilliance is dependent on the

proportions and symmetry of the cut.–Round, princess, etc…–Rated with - Excellent, Very Good,

…

Color

• Usually colorless, but can occur in all colors.• DEF (Colorless)• All the way to Z (yellow)

Carat (not karat)

• One carat equal 0.2 grams• Measured to 0.001 carat and

rounded to 0.01 carats

Clarity• Fl (Flawless, no blemish under 10x)• V V S1 and V V S2

• VS1 and VS2

• SI1 and SI2

• I1, I2, I3 (obvious blemishes)

History of Engagement Ring• Became popular in 1477 – Archduke Maximillian of Hamburg and Mary of

Burgandy • De Beers Consolidate Mines, Ltd 1888 was created to

protect the investment of diamond mine investors from new mine found in S. Africa 1870.

• This flooded the market and by 1919 sales declined by 50%

• Ad campaign of 1939 made diamond ring of choice

World’s Largest/ Famous Diamonds

• Cullinan I – known as the Star of Africa–Largest cut diamond at 530 carats,

found in Tower of London as part of the crown jewels

http://www.si.edu/siphotos/science-nature/HOPE.GIF

The Blue Hope Diamond

• owned by Louis XIV• Stolen in French revolution and reappeared in

1830• Bought by Henry Phillip Hope of London• Cursed- two of the owner had their entire

families die just one year apart• Found in Smithsonian

Colored Diamonds

• Colored Diamonds are a result of impurities

Life Gems

• Making diamonds from loved ones• Your loved one’s ashes under extreme

temperature and pressure can be changed into a colored diamonds pendant or ring

Carbon…

• Allotropes (draw or describe each)–graphite

–diamonds

–buckeyball

Graphite

Diamonds

Buckyballs

25

Conduction

• Transfer of heat between substances that are in direct contact with each other.

26

•Good conductors?•Poor conductors?

27

Convection

• Up and downward movement of gases and liquid caused by heat transfer

28

Radiation

• Electromagnetic waves come in contact with an object and the waves transfer heat

Pressure

• The ratio of force per unit area.

• Standard Pressure is defined as air pressure at sea level.– As altitude increases, pressure decreases

http://www.sciencemuseum.org.uk/collections/exhiblets/weather/baromdiagram2.asp

Standard Pressures

• Pressure at Sea Level in 7 different units– 14.7 Psi– 30.00 inches Hg– 760 mm Hg– 760 torr– 1.00 atmospheres (atm)– 1013 Millibars – 101.3 kilopascals (kPa)

Standard Pressure Uses• psi – tire pressure/ paint ball• inches Hg – US weather reports• mm Hg- same as torr - medical–Normal blood pressure is 110 to 150

mmHg when heart beats and 60 to 80 mmHg when heart relaxes

• Torr – another name for mmHg (named after scientists Torricelli)

More pressures

• mb – meteorologist • kPa – pascals is SI unit • atm – pressure at earth’s surface

(1 atm)

Temperature

• The hotness or coldness of an object corresponding to its molecular activity• A measure of the average kinetic energy of

the particles in an object.

Temperature Effects

• As temp increases, average KE (kinetic energy) increases

• As temp decrease, average KE decreases

How low can you go?

• Absolute Zero–Particles have zero KE–All particle motion stops–0 Kelvin = -273.15 Celsius

Record Low Temperatures• Prospect Creek, Alaska

– Jan. 23, 1971 -80ºF• Rogers Pass, Montana

– Jan. 20, 1954, -70 F• Michigan

– Feb 9, 1934, -51 FWhat is the only state to never have a below zero temperature?(Hawaii, 12 F is lowest)

Record High Temperatures

• Death Valley, California– July 10, 1913, 134 F

• Michigan – July 13, 1936, 112 F

Temperature scales

•K F C•0 K•-40 °C/ -40 °F

Converting Temperature

• K = C + 273• F = (1.80*C) + 32• Solve this equation for C.

Try these...

• 3 °C to F• 432 K to °C • 212 F to K• 25.7 psi to mmHg• 1.5 atm to kPa• 2000 mbar to torr

http://www.elsevier.com/locate/issn/00112275

C4.3A

C5.4A Changes of State involving Solids

• Solid Liquid–Melting• Examples- other than water

• Solid Vapor (gas)– Sublimation• Example: dry ice, air fresheners, freeze

dried food

Behavior of Liquids

• Viscosity : the measure of a liquid’s resistance to flow

• Surface Tension: Inward forces that must be overcome in order to expand the surface area

Cohesion: molecules sticking to each otherAdhesion: forces that bind liquid to surface

• Capillary Action: rise of liquid up very narrow tubes

Changes of State w/ Liquids

• Liquid --> solid – freezing

• Liquid --> gas– Vaporization – Evaporation: occurs are the surface of the liquid only

• Vapor --> liquid– Condensation

• Gas - - > solid ?– Deposition

SOLID

LIQUID

GAS

Equilibrium

• equilibrium - no net change in a system (usually closed)

• static - no net change because nothing is happening

• dynamic - no net change because two opposite processes are occurring at the same rate

C5.4d/e Freezing and Melting Points

• Freezing point – Temp at which solid and liquid forms of a substance exist in equilibrium

• Melting point – Same point as f.p.• These are not affected significantly by

changing air pressure

Liquid gas

• Vapor pressure - the pressure exerted by those particles that have escaped from the liquid into the vapor (temp dependent)• Volatile - liquids having a significant

vapor pressure under ordinary conditions

Boiling

• Boiling - occurs when the vapor pressure of the liquid equals the external pressure above the liquid• boiling point - temp at which

boiling occurs, depends on external pressure• normal bp - boiling point at 1 atm

Boiling Points

• In Detroit, bp = 100 C• In Denver bp = 86 C–Food is being cooked at lower

temperature so although water boiled faster it needs to be cooked longer

C2.2c Phase diagrams

• http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_10&folder=phase_diagrams

GasLaws

Behavior of Gases

• Compressibility• Diffusion• Low density• Ability to mix• Exert uniform pressure

Gases are described by...• Pressure, P– kPa, atm, mmHg, torr, inHg, mbars, psi

• Volume, V– liter, mL, cm3

• Temperature, T (Use equations to convert)– KFC

• Number of moles, n– mole

Ideal Gas Model• Gases consist of molecular particles

moving in a straight line at any given time.• Molecules collide with each other

and the container of the walls without losing energy.

Ideal Gases ….

• Gas molecules behave as independent particles; attractive forces don’t exist.

UNITS of PRESSURE

• psi – tire pressure/ paint ball• inches Hg – US weather reports• mm Hg- same as torr - medical– Normal blood pressure is 110 to 150 mmHg

when heart beats and 60 to 80 mmHg when heart relaxes

• Torr – another name for mmHg (named after scientists Torricelli)

More pressures• mb – meteorologist

(H and L pressures)• kPa – pascals is SI unit

• atm – pressure at earth’s surface (1 atm)

Boyle’s Law

• For a sample of gas with V1 at some pressure P1 then P1 • V1 = constant.

• The same sample having a different P2 will have a V2 so that P2 • V2 = constant.

• So if constant = constant, then P1 • V1 = P2 • V2

Boyle’s law

• For a fixed quantity of gas ( n is constant ) at constant temperature, the pressure of the gas is inversely proportional to the volume of the gas.

P1 • V1 = P2 • V2

Charles’ Law

• For a sample of gas with V1 at some temperature T1 then V1 / T1 = constant.

• The same sample having a different V2 will have a T2 so that V2 / T2 = constant.

• So if constant = constant, then V1 / T1 = V2 / T2

Charles’ law

• For a fixed quantity of gas ( n is constant ) at constant pressure, the volume of the gas is directly proportional to the temperature of the gas.

V1 / T1= V2

/ T2

Ideal gas law

• PV = nRT–Standard Temperature and

Pressure?–What is R?