Make sure notebook is setup Friday Lab safety certificate due! KINETIC THEORY Unit 1 Baughman Warm-up 8/28 Make sure notebook is setup on the first left-side page (after you table of contents), answer the following: What’s your opinion of the simulation as a safety review? Was it good/bad…ugly? Why? reviewing your safety contract, list 5 things the simulation did not cover. In complete sentences, tell me why you think the creators decided to leave those points of. Would you? 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? 5 States of 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 much Definite shape and definite volume (because particles are packed closely and do not move) Most solids are crystals Crystals 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 www.wikipedia.org 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 apart Particles move slowly through a container No definite shape but do have a definite volume Flow from one container to another Viscosity – resistance of a liquid to flowing Honey – high viscosity Water – low viscosity Ex. Cats! chemed.chem.purdue.edu/.../graphics

GASES Particles are very far apart Particles move very fast No definite shape and No definite volume http://www.phy.cuhk.edu.hk/contextual/heat/tep/trans/kinetic_theory.gif

PLASMA Particles are extremely far apart Particles move extremely fast Only exists above 3000 degrees Celsius Basically, plasma is a hot gas When particles collide, they break apart into protons, neutrons, and electrons Occurs naturally on the sun and stars

BOSE-EINSTEIN CONDENSATE Particles extremely close together Particles barely move Only found at extremely cold temperatures Basically Bose-Einstein is a cold solid Lowest 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.) What is the kinetic theory of matter? What are the characteristics of matter? What are the 3 types of matter found extensively on Earth? How do particles move in the different states of matter?

Friday 8/29 Standards of Measurement (p.19-25) After quiz- Turn in ‘test’ & scantron (face-down) on front desk. There will be NO TALKING/PHONES until EVERYONE is done with the quiz! Get a textbook Using p.19-25, create a table like the one below with the data you find there. Below your table, define the following terms: heat of vaporization heat of fusion freezing melting  vaporization condensation evaporation sublimation deposition 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!

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! Below your table, define the following terms: heat of vaporization heat of fusion freezing melting  vaporization condensation evaporation sublimation deposition 3. Using p.19-25, create a table like the one below with the data you find there. 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!

Warm-up Wed 9/4 Within 5min after the bell: Keep in mind… Pick up Matter states ‘cards’ (If you haven’t already.) Get your notebook & find your new ASSIGNED seat Cut up cards, mix, & practice putting them back in order 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!

keep out something to write with. 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 2 Examples Property Changes from liquid to gas

Changes of States Key boiling solid liquid gas Property Changes 2 Examples Heat of fusion Heat of vaporization boiling evaporation melting vaporization solid liquid gas freezing condensation Sublimation Ex. Dry ice Property Changes from liquid to gas Decreased viscosity Thermal expansion

Phase Change Diagram for Water Warm-up Fri.: Where should our phase change terms go?