UNIT 1BAUGHMAN

KINETIC THEORY

WARM-UP 8/28

MAKE SURE NOTEBOOK IS SETUP

ON THE FIRST LEFT-SIDE PAGE (AFTER YOU TABLE OF CONTENTS), ANSWER THE FOLLOWING:

1.WHAT’S YOUR OPINION OF THE SIMULATION AS A SAFETY REVIEW? WAS IT GOOD/BAD…UGLY? WHY?

2. REVIEWING YOUR SAFETY CONTRACT, LIST 5 THINGS THE SIMULATION DID NOT COVER.

3.IN COMPLETE SENTENCES, TELL ME WHY YOU THINK THE CREATORS DECIDED TO LEAVE THOSE POINTS OF.

WOULD YOU?

HEADS UP FOR FRIDAY:HEADS UP FOR FRIDAY:SAFETY QUIZ!!!

FRIDAY LAB SAFETY CERTIFICATE DUE!

KINETIC THEORY

Kinetic Theory states that the tiny particles in all forms of matter are in constant motion. Kinetic refers to motion Helps you understand the behavior of solid, liquid, and

gas atoms/molecules as well as the physical properties Provides a model behavior based off three principals

3 Principles of Kinetic Theory All matter is made of tiny particles (atoms) These particles are in constant motion When particles collide with each other or the container,

the collisions are perfectly elastic (no energy is lost)

STATES OF MATTER

What is matter? Anything that has mass

& takes up space

5 States of Matter Solid Liquid Gas Plasma Bose-Einstein Condensates

http://www.plasmas.org/E-4phases2.jpg

SOLIDS

Particles are tightly packed and close together

Particles do move but not very muchDefinite shape and definite volume (because

particles are packed closely and do not move)

Most solids are crystalsCrystals are made of unit cells (repeating

patterns) The shape of a crystal reflects the arrangement of

the particles within the solid

SOLIDS

Unit cells put together make a crystal lattice (skeleton for the crystal)

Crystals are classified into seven crystal systems: cubic, tetragonal, orthorhombic, monoclinic, triclinic, hexagonal, rhombohedral

Unit cell crystal lattice solid

SOLIDS

Amorphous Solid: A solid with no defined shape (not a crystal) A solid that lacks an ordered internal structure Examples: Clay, PlayDoh, Rubber, Glass, Plastic,

Asphalt

Allotropes: Solids that appear in more than one form 2 or more different molecular forms of the same

element in the same physical state (have different properties)

Example: Carbon Powder = Graphite Pencil “lead” = graphite Hard solid = diamond

SOLIDS

www.ohsu.edu/research/sbh/resultsimages/crystalvsglass.gif

SOLIDS

Allotropes of Carbon:

a) diamond

b) Graphite

c) lonsdaleite,

d)buckminsterfullerene (buckyball)

e) C540

f) C70

g) amorphous carbon

h) single-walled (buckytube)

www.wikipedia.org

LIQUIDS

Particles are spread apartParticles move slowly through a containerNo definite shape but do have a definite

volumeFlow from one container to anotherViscosity – resistance of a liquid to flowing

Honey – high viscosity Water – low viscosity

chemed.chem.purdue.edu/.../graphics

Ex. Cats!

GASES

Particles are very far apartParticles move very fastNo definite shape and No definite volume

http://www.phy.cuhk.edu.hk/contextual/heat/tep/trans/kinetic_theory.gif

PLASMA

Particles are extremely far apartParticles move extremely fastOnly exists above 3000 degrees CelsiusBasically, plasma is a hot gasWhen particles collide, they break apart into

protons, neutrons, and electronsOccurs naturally on the sun and stars

BOSE-EINSTEIN CONDENSATE

Particles extremely close togetherParticles barely moveOnly found at extremely cold temperaturesBasically Bose-Einstein is a cold solidLowest energy of the 5 states/phases of

matter

GASES AND PRESSURE

Gas pressure is the force exerted by a gas per unit surface area of an object Force and number of collisions When there are no particles present, no collisions

= no pressure = vacuum Atmospheric Pressure is caused by a mixture of

gases (i.e. the air) Results from gravity holding air molecules downward

in/on the Earth’s atmosphere; atmospheric pressure decreases with altitude, increases with depth

Barometers are devices used to measure atmospheric pressure (contains mercury)

Standard Pressure is average normal pressure at sea level As you go ABOVE sea level, pressure is less As you go BELOW sea level, pressure is greater

GASES AND PRESSURE

Standard Pressure Values At sea level the pressure can be recorded as:

14.7 psi (pounds per square inch) 29.9 inHg (inches of Mercury) 760 mmHg (millimeters of Mercury) 760 torr 1 atm (atmosphere) 101.325 kPa (kilopascals)

All of these values are EQUAL to each other: 29.9 inHg = 101.325 kPa 760 torr = 760 mmHg 1 atm = 14.7 psi and so on……….

Say hello to Factor Label Method & Dimensional Analysis!!!!!!!!!!!!

GASES AND PRESSURE

STP Standard Temperature and Pressure Standard Pressure values are the values listed

on the previous slides Standard Temperature is 0°C or 273 K

If given in Fahrenheit, you must convert first! °F = (9/5)°C + 32 °C = (5(°F-32)) / 9 Remember order of operation

rules K = 273 + °C °C = K – 273

What questions have we answered?

Using complete sentences, answer each of the following essential questions in your notebook. (You do NOT need to rewrite the question, but I should be able to tell what the question was by your answer.)

1.What is the kinetic theory of matter?

2.What are the characteristics of matter?

3.What are the 3 types of matter found extensively on Earth?

4.How do particles move in the different states of matter?

Friday 8/29

Standards of Measurement (p.19-25)Unit

(name)Unit

(symbol)What does it

measure?

If units measure the same thing, what makes each

unique?

Keep adding rows as needed… You WILL have more than this!

1. After quiz- Turn in ‘test’ & scantron (face-down) on front desk.• There will be NO TALKING/PHONES until EVERYONE is done

with the quiz!

2. Get a textbook

3. Using p.19-25, create a table like the one below with the data you find there.

4. Below your table, define the following terms:

• heat of vaporization• heat of fusion• freezing• melting • vaporization• condensation• evaporation• sublimation• deposition

Warm-up Tues 9/2

Pick up a set of ‘States of Matter’ cards. Match the properties to each state

Before we can go on… Friday’s work needs to be completed.

You have 15min!

Standards of Measurement (p.19-25)Unit

(name)Unit

(symbol)What does it

measure?

If units measure the same thing, what makes each

unique?

Keep adding rows as needed… You WILL have more than this!

3. Using p.19-25, create a table like the one below with the data you find there.

4. Below your table, define the following terms:

• heat of vaporization• heat of fusion• freezing• melting • vaporization• condensation• evaporation• sublimation• deposition

Warm-up Wed 9/4

Within 5min after the bell:1. Pick up Matter states ‘cards’ (If you haven’t already.)

2. Get your notebook & find your new ASSIGNED seat3. Cut up cards, mix, & practice putting them back in order4. Review our previous notes

Keep in mind… Failure to do these tasks in a QUIET AND PROFESSIONAL

MANNER will result in a Teacher Detention. THIS IS YOUR WARNING!!!

Behave in a way that EARNS you the respect you feel you deserve!

Pop Quiz!

Put your notes away, but keep out something to write

with.On your answer sheet,

choose the correct response.We will exchange, grade,

and discuss after.

Lab DEMO Instructions

Review lab instructions as a class

In the meantime: Changes of States diagram & Temperature Conversions RECALL: Standard Temperature is 0°C or 273 K

If given in Fahrenheit, you must convert first! °F = (9/5)°C + 32 °C = (5(°F-32)) / 9 Remember order of operation rules K = 273 + °C °C = K – 273

Temperature Conversion Examples

What is the Celsius value for 65° Fahrenheit?200°C is the same temperature as what value on

the Fahrenheit scale?Water boils at a temperature of 100°C. What

would be the corresponding temperature for the Kelvin scale?

A substance has a melting point of 625 K. At what Celsius temperature would this substance melt?

Conversions from K to °F, or F to °K are rare, but possible. You can combine 2 formulas or use 2 steps.

Changes of States

Property Changesfrom liquid to gas

2 Examples

Changes of States Key

Property Changesfrom liquid to gas

2 Examples

solid liquid gas

boiling

evaporation

condensationfreezing

vaporizationmelting

Heat of vaporization

Heat of fusion

SublimationEx. Dry ice

Decreased viscosity

Thermal expansion

Phase Change Diagram for Water

Warm-up Fri.: Where should our phase change terms go?