2. EnergyMatter  The capacity to do work or produce heat  Anything that occupies space and has mass

3.  A joule is @ how much energy it takes to lift an apple 1 meter.  4.184 Joules = 1 calorie  A calorie is the mount of heat needed to heat 1 gram of Water 1⁰ C  1 Calorie = 1 gram H2O x 1 ⁰ C  How many calories to heat 5 grams of water 2 ⁰ C?  Calories = 5 grams x 2 ⁰ C = 10 calories  1 ml of distilled water = 1 gram distilled water.

4. Potential Positional Energy Stored Energy Kinetic Energy of Motion ENERGY Thermal Total energy of all the particles in a substance

5.  The energy carried by moving things.  A train moving down the tracks has a lot of energy (it is doing a lot of work, producing a lot of heat). The engine is pulling the rest of the train against the resistance due to friction of the tracks, the surrounding air, and grinding of moving parts in the engine.

6.  The energy of position ( or stored energy).  If you collect rain water in a barrel, and then channel it down a pipe, so that it turns a wheel, and the moving wheel performs some sort of work – then the water in the barrel has potential energy (it has the ability to perform work due to it’s position above the wheel.)

7.  A form of potential and kinetic energy due to the internal motion of particles of matter.  A small pot of boiling water vs. a large pot of boiling water. The large pot could probably do more work, and therefore has more thermal energy due to more movement of particles within the water.

9. Temperature is the average of the kinetic energy of the particles of a substance.  In Chemistry, we measure temperature in Kelvin and Degrees Celsius (°C)

10. The kinetic molecular theory explains that all matter is made up of tiny particles.  These atoms and molecules are constantly in motion.  Kinetic energy is energy due to motion.

11. HEAT!! The more heat you add to a system – the more the particles spread out and move faster. If you take away heat – the particles move closer together and slow down. The faster molecules are moving, the greater their kinetic energy and therefore the greater their temperature

12. Celsius Kelvin (SI unit)  Based on the boiling and freezing points of pure water  Has the same gradations as the Celsius scale  Is based around ABSOLUTE ZERO (-273⁰ C)  This is the temperature where all molecular motion stops… we think ;) N.B. You can’t ever have a temperature lower than zero K... This should help you remember this equation!!!

13. Why is absolute zero impossible to get to? What is the coldest place in our solar system?  Practically… the work needed to remove heat from a gas increases the colder you get, and an infinite amount of work would be needed to cool something to absolute zero (where it doesn’t move b/c no heat).  The lowest temperature ever measured in the solar system was on the Moon. NASA's Lunar Orbiter measured temperatures as low as −240°C in permanently shadowed craters near the lunar south pole.

14.  Energy can be neither created or destroyed in any process (where energy is transferred).  James Prescott Joule, a physicist.

15. 1) What point on the Kelvin scale corresponds to -273 ⁰ C? 2) Convert 50 ⁰ C to Kelvin 3) Convert 50 ⁰ K to Celsius 4) What happens at absolute zero? 5) You are baking a lasagna for your mommy because you are so sweet! BUT… the recipe says to bake at 453 ⁰K, and your oven is in Fahrenheit!! What ⁰F would you need to set the oven at ? (this equation might help… F = (1.8 )(C) + 32)

16. 1) What point on the Kelvin scale corresponds to -273 ⁰ C? O ⁰ K 2) Convert 50 ⁰ C to Kelvin 323 ⁰ K 3) Convert 50 ⁰ K to Celsius -223 ⁰ C 4) What happens at absolute zero? All particle motion stops!! 5) You are baking a lasagna for your mommy because you are so sweet! BUT… the recipe says to bake at 453 ⁰K, and your oven is in Fahrenheit!! What ⁰F would you need to set the oven at ? (this equation might help… F = (1.8 )(C) + 32) 453 ⁰K = 180 ⁰C = 356 ⁰F

17. Summary of Matter Pure Substance Has a unique set of properties and always maintains the same element to element ratio Element 1 type of atom present (Ca) Compound More than 1 type of atom present (H2O) Mixture A blend of 2 or more pure substances Homo- genious Mixture (No visibly different parts) (Sea water) Hetero- genious Mixture (Visibly different parts) Each component has it’s own unique properties (Milk)

18. 3 states/phases of matter = Solid, liquid, gas. Solid – very little particle movement (little space between particles). A definite shape and volume. Very Dense!! Liquid = more particle movement, and more space between particles. No definite shape, but a definite volume. Gas = Lots of particle movement,and lots of space between particles. No definite shape or volume. Very Low density!! Also Plasma!!

19. Eg. Mercury Freezes to a solid at -39 degrees (it’s freezing point and melting point), and it boils and becomes a gas at 357 degrees (it’s boiling point and condensing point). Between these 2 temperatures, Mercury is a shiny slippery liquid.

20. What did the Ice cube say to the Bunsen Burner? Ice Cube: Oh Bunsen, I melt every time I see you! Bunsen: You’ll get over it it’s just a phase you’re going through.

22. Define: Melting point Freezing point Boiling Point Condensation point Question: Why does the temperature remain constant at the moments of phase change, but continue to rise once a phase is established?

23. Physical Changes - A change in phase so that NO new substances are formed. Eg. Change in size, changing from liquid to solid, change in color, density, malleability, etc… Chemical Changes – A change in which a new substance is created Eg. Metal rusting, something burning, a chemical reaction to create a new compound, etc..

24.  Matter can neither be created or destroyed in a process (where matter is being transferred)  From Antoine Lavoisier  Guillotined during the “Reign of terror” in France  “ It only took an instant to cut off that head, and a hundred years may not produce another like it” ~ Lagrange (mathematician)

25.  # 33, 34, 35, 36, 39, 41, 44