TABLE OF CONTENTS States of Matter 2 – 10 Changes in state 11 – 12 Heating Curve & Heat equations 13 – 18 Practice Problems 17 Review questions 19 - 20

4th state: Plasma - formed at high temperatures; ionized phase of matter as found in the sun (gases stripped of electrons).

SOLID, LIQUID AND GAS http://www.footprints-science.co.uk/states.htm Click on the link and watch the animations below The Three States of Matter2.rm Note the change in how the particles are arranged in each state.

COPPER PHASE - SOLID

LIQUID PHASE - COPPER

GAS PHASE - COPPER

Some Properties of Solids, Liquids, and Gases Property Solid Liquid Gas Shape Has definite shape Takes the shape of Takes the shape the container of its container Volume Has a definite volume Has a definite volume Fills the volume of the container Arrangement of Fixed, very close Random, close Random, far apart Particles Interactions between Very strong Strong Essentially none particles

YOU NEED TO KNOW UNDERSTAND THE INFORMATION IN THIS CHART!!! WEAK STRONG VERY STRONG Particle Attraction FREE TO MOVE ABOUT NO NO Gas CLOSE, SLIDE PAST EACH OTHER YES NO Liquid CLOSE, VIBRATE IN PLACE YES YES Solid Particle Arrangement Volume Def volume (Y/N) Shape Def Shape? (Y/N) State of matter

CHANGES OF STATE Adding or taking away energy causes substances to change state. Most of these changes in state are familiar. http://eanes.tx.schoolwebpages.com/education/components/docmgr/default.php?sectiondetailid=6107&fileitem=8730&catfilter=1594 Solid Liquid Gas Melt Evaporate Condense Freeze

Click on the link below to watch how the particles of ice change as heat is added. You are not responsible for any questions on this animation. http://www.bgfl.org/bgfl/custom/resources_ftp/client_ftp/ks3/science/changing_matter/index.htm CHANGES OF STATE Some changes in state are not so familiar. An important change in state is sublimation. Sublimation is the change of a substance as it goes from a solid directly to a gas. The most common example being dry ice. Dry ice is frozen carbon dioxide gas.

HEATING CURVE BIG TEST CONCEPT

A NOTE ON SPECIFIC HEAT Description: One paper cup is filled with water; the other is empty. When the cups are placed above a lit Bunsen burner, the empty cup burns, whereas the water-filled one doesn't. This is because the water absorbs most of the heat of the flame due to its high specific heat. Specific Heat Capacity - The ability of materials to "hold" a certain amount of thermal energy at a given temperature. Consider a day at your favorite Carolina beach. On a typical summer day the sand is so hot it will burn your feet, yet the water feels much cooler and quite comfortable. The same holds true if you consider the parking lot. Each material experiences the same summer sun, but each heats up differently. Later that night the sand and parking lot would feel quite cool to the feet, and the water temperature will not have changed. Each material “holds” a certain amount of specific heat, and each will gain and lose that heat at different rates. The sand loses its heat really fast (low specific heat) the water loses heat slowly (high specific heat). The reverse is true, water must gain a lot of heat to change temperature, sand needs only a little to warm up quickly. Not as bad as it looks…read on 140 °C 70 °C Foosium 140 °C 40 °C Unobtainium 100 °C 20 °C Bolognium Boiling point Melting point Substance

Q = m x C x Δ T Determine the energy needed (in Joules) when 55.6 grams of water at 43.2 °C is heated to 78.1 °C. Q = ? m = 55.6 g Δ T = T f – T i (final temp – initial temp) 78.1 o – 43.2 o = 34.9 o C C = specific heat of water 4.18J (found on your reference table) Q = 55.6g x 4.18J x 34.9 o C = 8111 J of energy needed