1. Phases of Matter Chapter 3 1

2. Matter and Energy Section 1 2

3. Let’s Review! Matter is… –Anything that has mass and takes up space –Can be a pure substance… Element or compound – Or a mixture… Homogeneous or heterogeneous –Made of… Atoms and molecules 3

4. Kinetic Theory Kinetic Theory of Matter: –Matter is made of atoms and molecules –These atoms and molecules act like tiny particles that are always in motion 4

5. Kinetic Theory The higher the temperature, the faster the particles move. At the same temperature, more massive particles move slower than less massive ones 5

6. Phases of Matter Matter can be classified as a solid, liquid, or gas This is determined by whether or not the shape and volume are definite or variable 6

7. Solid Solid: atoms/molecules can only vibrate in one place, occasionally slide by one another. –students in a detention fidgeting in their seats Shape: definite Volume: definite Energy: low Crystalline Solid: atoms arranged in a regular repeating pattern –Salt, diamonds Amorphous Solid: No repeating pattern –Wax, glass 7

8. Liquid Liquid: atoms/molecules can move about freely –students in the cafeteria Shape: variable Volume: definite Energy: mid-level Surface Tension: Attraction of molecules at the surface of a liquid –this causes liquids to form spherical drops Viscosity: resistance to the flow of a liquid –low = runny –high = thicker, like honey 8

9. Gas Gas: atoms/molecules move around wildly constantly running into each other. –football practice Shape: variable Volume: variable Energy: High Because the particles in liquids and gases can move past each other they are considered “fluids” 9

10. Plasma 4 th and most common phase of matter in the universe Shape: variable Volume: variable Energy: highest (the particles are electrically charged) Affected by magnetic fields 10

11. Plasma They act like gases but have some differences –plasma can conduct electric current while gases do not Commonly found in stars, can be created naturally by lightning on Earth and in the hottest part of a very hot flame. 11

12. Energy Energy: the ability to change or move matter, or to do work. –Kinetic: energy of motion –Potential: stored energy or energy of position 12

13. Energy Because all particles of matter are in motion, they all have kinetic energy All energy can be converted from potential energy to kinetic energy 13

14. Temperature Particles of matter are constantly moving, but they don’t all move at the same speed, therefore, some have more kinetic energy than others Temperature: a measure of the average kinetic energy of the particles in an object. 14

15. Thermal Energy Thermal energy: total kinetic energy of the particles that make up a substance Temperature versus thermal energy –Temperature is average kinetic energy –Thermal energy is determined by the amount of a substance 15

16. Changes of State Section 2 16

17. Changes of State Change of state or a phase change is a conversion of a substance from one phase (solid, liquid, or gas) to another. The identity of the substance does not change, but the amount of energy does. 17

18. Phase Changes Adding energy, in the form of heat, causes particles to move FASTER –Solid  Liquid  Gas Removing energy causes particles to move SLOWER –Gas  Liquid  Solid 18

19. Phase Changes Some phase changes require energy –Melting, evaporation, sublimation Some phase changes release energy –Boiling, condensation, deposition A change in energy often means a change in temperature also 19

20. Melting Solid  Liquid Melting Point: the temperature at which a substance changes from solid to liquid. Melting point depends on the pressure. 20

21. Evaporation Liquid  Gas Boiling Point: the temperature at which a liquid turns into a gas When humans sweat (a liquid), heat from the body or surroundings causes evaporation When the water evaporates, the molecules take their heat energy with them, which creates a cooling effect on the body! 21

22. Sublimation Solid  Gas –Solid carbon dioxide (dry ice) goes from solid to gas –Ice cubes can go from ice to gas while still in the freezer 22

23. Condensation Gas  Liquid Condensation Point: the temperature at which a gas becomes a liquid Fog is caused by condensation, the water gas particles clump, energy is released from the particles, and their movement slows down 23

24. Freezing Liquid  Solid Freezing Point: temperature at which a liquid becomes a solid 24

25. Temperature During a change of state, temperat ure is constant 25

26. Law of Conservation of Mass Mass cannot be created or destroyed, it is conserved for all physical and chemical changes The total mass of the reactants is the same as the total mass of the products 26

27. Law of Conservation of Energy Energy cannot be created or destroyed Energy may be changed to another form during a physical or chemical change, but the total amount of energy present before and after the change is the same –IF energy of a substance changes it is because it came from another source! 27