States of Matter Chapter 3 Section 1 states of matter Section 2 behavior of gases Section 3 changes of state

The Four States of Matter Your textbook states that there are three states of matter but you will be responsible for learning about four states of matter…I am throwing in the 5th state just so you can dazzle your high school science teacher! Solids Liquids Gases Plasma

STATES OF MATTER Based upon particle arrangement Based upon energy of particles Based upon distance between particles

Matter Matter is made of tiny particles. Atoms - single element Molecules -more than 1 type of element Atoms and molecules are always in a state of motion (much like the St. Ann students) and are always bumping into each other

STATES OF MATTER SOLIDS Particles of solids are tightly packed, vibrating about a fixed position. Solids have a definite shape and a definite volume. Heat

Solids Solids Definite Shape Definite Volume Particles vibrate in fixed positions Particles have low kinetic energy

Two Types of Solid Matter Crystalline Solids Long-range order Repeating patterns Think back to the 6 different crystalline structures you learned in the 6th grade Ex. Iron, diamond, ice Amorphous Solids No long range order Polymers, glass Ex. Glass, rubber, wax Sodium Chloride

STATES OF MATTER LIQUID Particles of liquids are tightly packed, but are far enough apart to slide over one another. Liquids have an indefinite shape and a definite volume. Heat

Liquids Variable shape (takes the shape of the container) Definite Volume Particles can move around each other Particles have medium Kinetic Energy

Unique characteristics of liquids Surface tension- a force that acts on particles at the surface of a liquid Remember the penny lab at the beginning of the year Water has a high surface tension so forms droplets. Gas has a low surface tension and forms flat drops Viscosity- liquid’s resistance to flow Higher the attraction between the molecules, the more viscous the liquid Think about pouring water vs honey

STATES OF MATTER GAS Particles of gases are very far apart and move freely. Gases have an indefinite shape and an indefinite volume. Heat

Gases Variable shape Variable volume (fills all space in a container) Particles move about freely Particles have high Kinetic Energy

Classifying Matter According to its State: Solid, Liquid, Gas Water can exist as a solid, liquid or gas

Will everything just be a gas? But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ? Will everything just be a gas?

PLASMA NO! The 4th state of matter: If the gas is made up of particles which carry an electric charge (“ionized particles”), but the entire gas as a whole has no electric charge, and if the density is not too high, then we can get The 4th state of matter: PLASMA

STATES OF MATTER PLASMA A plasma is an ionized gas. A plasma is a very good conductor of electricity and is affected by magnetic fields. Plasmas, like gases have an indefinite shape and an indefinite volume. Plasma is the common state of matter

Some places where plasmas are found… 1. Flames

2. Lightning

3. Aurora (Northern Lights)

4. Neon lights

5. Stars Stars make up 99% of the total matter in the Universe. Therefore, 99% of everything that exists in the entire Universe is in the plasma state.

The Sun is an example of a star in its plasma state

6. Clouds of gas and dust around stars

STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

Will everything just be a frozen solid? But now what happens if you lower the temperature way, way, down to 100 nano degrees above “Absolute Zero” (-273°C) Will everything just be a frozen solid?

Not Necessarily! In 1924 (82 years ago), two scientists, Albert Einstein and Satyendra Bose predicted a 5th state of matter which would occur at very very low temperatures. Einstein Bose +

Ketterle and his students Finally, in 1995 (only 12 years ago!), Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time. Ketterle and his students The 5th state of matter: Bose-Einstein Condensate This 5th state of matter will not be on any St. Ann test but you will dazzle your high school science teacher if you know that a 5th state has been discovered!

To really understand Bose-Einstein condensate you need to know Quantum Physics

In 2002, Ketterle and two other scientists received the highest award in science for discovering Bose-Einstein condensate: The Nobel Prize

The five states of matter: PLASMAS (only for low density ionized gases) BOSE-EINSTEIN CONDENSATE LIQUIDS SOLIDS GASES Lower Temperature Higher Temperature

Kinetic Theory Kinetic energy = energy an object has due to its motion The faster an object is moving; the greater its kinetic energy. Kinetic theory states that all particles of matter are in constant motion.

Classifying Matter According to its State: Kinetic Theory

3-2 Behavior of Gases What's the Matter? The three main states of matter that we meet daily are: gas, liquid, and solid. Gases can be compressed, they expand to fill their containers. The volume of a gas is variable

In this room right now are millions of gas molecules and atoms colliding with the walls, the floor, your face and each other. Can you feel it?

Pressure One property of gases is that they exert pressure. The pressure exerted by the gas mixture we call air is called atmospheric pressure. The atmosphere that surrounds Earth is a sea of air. It exerts a force on the surface of the planet. Above you is a column of air that is exerting a force on you. This pressure can be measured. But why is air exerting pressure?

Pressure Pressure = the result of force distributed over an area In a closed container, gases exert pressure when the particles of the gas collide with the walls of the container.

Compressibility Solids are incompressible Gases are compressible Liquids are very slightly compressible – usually considered incompressible

Factors That Affect Gas Pressure Temperature – raising temp. will increase pressure if volume of gas and # of particles are kept constant Inc. in temp.  part. move faster  part. collide with walls more frequently  increased pressure

Volume – Decreasing volume of a gas causes an increase in pressure if the temp. and # of part. are constant Decrease in vol.  less space  particles collide with walls more often  inc. pressure

Number of particles – increasing the number of particles of a gas will increase pressure if temp. and volume are constant Inc. # of particles  particles collide with container more often  inc. pressure

Why is air pressure important? Feel the pressure!! Why is air pressure important? It causes wind Creates clouds and clear skies Allows us to predict the weather

P1V1 = P2V2 Pressure and Volume Boyles Law The volume of a gas is inversely proportional to its pressure P1V1 = P2V2

Pressure and Volume: Boyles Law Irish scientist Robert Boyle experimented with the relationship between pressure and volume of gases. He set-up a J-shaped tube and added mercury to see what it did to the volume of a trapped gas. As pressure increased volume decreases.

Pressure and Volume Boyles Law If the volume is increased the gas particles collide with the walls of the container less often and the pressure is reduced.

Boyle’s Law

Boyle’s Law (temp constant) A decrease in the volume of gas will result in an increase in pressure An increase in the volume of gas will result in a decrease in pressure V1P1 = V2P2

Volume and Temperature: Charles's Law French physicist Jacques Charles was the first to fill a balloon with hydrogen gas and make a solo flight. He showed that the volume of a gas increases when the temperature increases (at a constant pressure)

Volume and Temperature Charles’s Law The volume of a gas is directly proportional to its Kelvin temperature at constant pressure V2 V1 = T1 T2

Charles’ Law

Charles’s Law pressure constant Volume of a gas increases with increasing temperature Volume of a gas decreases with decreasing temperature V1 = V2 T1 T2

Principle- Use Boyles (temperature constant) Squeezing a balloon Charles (pressure constant) Why balloons decrease in size when kept in a cold room Reason for statement on hair spray: “keep away from heat, contents under pressure”

Websites for additional help http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/gasesv6.swf http://www.grc.nasa.gov/WWW/K-12/airplane/aboyle.html http://www.virtlab.com/main.aspx

3-3 Changes of State What would it take for matter to move from one state to another?

Melting and Freezing Melting Solid changes to liquid Particles absorb energy (endothermic) Particles become less orderly

Freezing Liquid changes to solid Particles release energy (exothermic) Particles become more orderly

Vaporization and Condensation Liquid changes into a gas Particles absorb energy (endothermic) Particles become LESS orderly and more free to move 2 types of vaporization Evaporation – takes place at the surface of a liquid Boiling – occurs when a liquid is heated to its boiling point

Condensation Gas changes to a liquid Particles release or lose energy (exothermic) Particles become MORE orderly

Sublimation and Deposition Changing from a solid directly to a gas Energy is absorbed (endothermic) Deposition Changing from a gas directly to a solid Energy is released (exothermic)

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Solid to liquid Melting Heat goes into the solid as it melts. Liquid to solid Freezing Heat leaves the liquid as it freezes.

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Liquid to gas Vaporization, which includes boiling and evaporation Heat goes into the liquid as it vaporizes. Gas to liquid Condensation Heat leaves the gas as it condenses. Solid to gas Sublimation Heat goes into the solid as it sublimates.

Phase Changes Melting Going from Solid to Liquid Freezing Going from Liquid to Solid Vaporization Going from Liquid to Gas Condensation Going from Gas to Liquid Sublimation Going from Solid to Gas

Phase Change Diagram