1. Chapter 16 & 15 Properties and classification of matter

2. Kinetic Theory Kinetic Theory—an explanation of how particles in matter behave. There are 3 assumptions of kinetic theory: 1.All matter is made of small particles 2.These particles are in constant motion 3.The particles collide with each other and the walls of their container.

3. Solid State The particles of a solid are closely packed together. Most solids have a specific geometric arrangement. You can tell the chemical and physical properties of a solid based on the type of arrangement that a solid forms. Solids have a definite shape and volume.

4. Liquid State Liquids form at a melting point—the temp. that a solid begins to liquefy. Particles in a liquid have more kinetic energy than in a solid—they are moving faster. These particles can slide past each other allowing liquids to flow and take the shape of their container. Liquids have a definite volume, but no definite shape.

5. Gas State Particles in a gas have more kinetic energy than in a liquid. A liquid becomes a gas through evaporation or boiling. Gas particles have enough kinetic energy to overcome the attractions between them. Gases have no definite shape or volume. They can spread apart to fill the container they are in. Diffusion—the spreading out of particles throughout a volume until they are uniformly distributed.

6. States of Matter

7. Plasma State Plasma is the most common state of matter in the universe. Plasma—matter consisting of positive and negative particles at very high temperatures. When gases get very hot their particles move faster, these fast moving particles collide with greater force. These collisions can pull off electrons, creating a charged particles All stars (including the sun) consist of plasma. Plasma is also found in lightning, neon light tubes, and auroras.

8. Expansion of Matter As the temperature of particles increases, the particles move faster and separate. The separation of particles causes the whole object to expand. Thermal Expansion—an increase in the size of a substance when temperature increases. Examples: Examples: Solid: Expansion joints in sidewalks Liquid: Thermometer Gas: Hot air balloon

9. Water: The Exception Water is an exception to thermal expansion because liquid water is most dense at 4 ° C. Water molecules are unusual because they have highly positive areas and highly negative areas. As the molecules move closer, the unlike charges are attracted. This causes some empty spaces in the structure. This empty space makes solid ice less dense than liquid water.

10. Solid or Liquid? Some substances have unusual behavior. They have properties of both solids and liquids. Amorphous solids—solids that lack the ordered structure found in crystals. Examples: Glass and plastic Examples: Glass and plastic Liquid Crystals—start to flow as they melt, but do not lose their ordered arrangement completely Examples: Liquid Crystal Displays (LCD) in watches, calculators, computers, and TVs. Examples: Liquid Crystal Displays (LCD) in watches, calculators, computers, and TVs.

11. Sec. 2: Properties of Fluids Buoyancy—the ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it. This is what causes ships to float. This is what causes ships to float. Archimedes’ Principle—the buoyant force on an object is equal to the weight of the fluid displaced by the object. An object will float if its density is less than the density of the fluid it is placed in.

12. Pascal’s Principle Pressure—force exerted per unit area Pressure = Force/Area P = F/A Pressure = Force/Area P = F/A Pascal’s Principle—pressure applied to a fluid is transmitted throughout the fluid. Example: you squeeze 1 end of a toothpaste tube, toothpaste comes out the other end. Example: you squeeze 1 end of a toothpaste tube, toothpaste comes out the other end.

13. Bernoulli’s Principle Bernoulli’s principle describes how people were able to build a machine that can fly. Bernoulli’s Principle—as the velocity of a fluid increases, the pressure exerted by the fluid decreases. Airplane wings were designed to reduce pressure above the wings.

14. Sec 3: Behavior of Gases Boyle’s Law—when volume is decreased, pressure is increased (and vice versa) as long as temperature is constant. The equation for Boyle’s Law is P 1 V 1 = P 2 V 2 P 1 V 1 = P 2 V 2 The subscript 1 represents initial pressure and volume, and the 2 represents final P & V. The subscript 1 represents initial pressure and volume, and the 2 represents final P & V. The unit for pressure is pascals & the unit for volume is liters.

15. Charles’s Law Charles’s Law—the volume of a gas increases with increasing temperature (and vice versa) The equation for Charles’s Law is V 1 = V 2 V 1 = V 2 T 1 T 2 T 1 T 2 Again, 1 is initial, and 2 is final. Again, 1 is initial, and 2 is final. Volume is in liters and temp. must be in Kelvin Volume is in liters and temp. must be in Kelvin

16. The Pressure-Temperature Law As temperature increases, the pressure increases too (and vice versa) This is why you should keep pressurized spray canisters away from heat.

17. Classification of Matter

18. Sec. 1 Composition of Matter All materials are either made of pure substances or mixtures. Substance—an element or compound, definite composition Element—a substance with atoms that are all alike Ex. Carbon (C) & Magnesium (Mg) Ex. Carbon (C) & Magnesium (Mg) You can find them on the periodic table!! You can find them on the periodic table!! Compound—a substance that contains 2 or more elements combined chemically. Ex. Table salt (NaCl) & Hydrogen peroxide (H 2 O 2 ) Ex. Table salt (NaCl) & Hydrogen peroxide (H 2 O 2 )

20. Mixtures Mixture—a material made of 2 or more substances that can be separated physically. There are 2 types of mixtures: heterogeneous and homogeneous. Heterogeneous Mixture—different materials can be distinguished easily. Ex. Pizza, salad, chocolate chip cookies (mmm) Ex. Pizza, salad, chocolate chip cookies (mmm) Suspension—a heterogeneous mixture containing a liquid in which visible particles settle. Ex. Mud in a pond & river deltas Ex. Mud in a pond & river deltas

21. Mixtures Homogeneous Mixture—substances are blended evenly throughout. Solution – homogenous mixture that remains constantly and uniformly mixed and has extremely small particles Ex. Pop, vinegar Ex. Pop, vinegar

22. How to Classify Matter ElementSubstanceCompoundMatterHeterogeneousMixtureHomogeneous

23. Sec. 2: Properties of Matter Physical Properties—any characteristic of a material that you observe without changing its substances. Ex. Color, shape, size, density, melting & boiling point Ex. Color, shape, size, density, melting & boiling point Some physical properties describe behavior. Magnetism, conduct electricity, viscosity, dissolving. Magnetism, conduct electricity, viscosity, dissolving. You can separate mixtures using physical properties. Size, color, magnetism, boiling point, etc. Size, color, magnetism, boiling point, etc.

24. Chemical Properties Chemical Property—a characteristic of a substance that tells if it can undergo a certain chemical change. Ex. Flammability, reaction to light Ex. Flammability, reaction to light

25. Physical Changes Physical change—a change in size, shape, or state of matter (solid, liquid, gas) The identity of the substance doesn’t change. The identity of the substance doesn’t change. Ex. Freezing, ripping, folding, dissolving. Ex. Freezing, ripping, folding, dissolving.

26. Physical Changes Physical changes DO NOT alter the identity of the original substance A change in size, shape or state of matter is a physical change “3S”

27. Chemical Changes Chemical Change—a change of 1 substance to another. Ex. Rotten eggs, rust, burning. Ex. Rotten eggs, rust, burning. Detecting Chemical Changes: Odor, heat, light, sound, release gas (bubbles), color change Odor, heat, light, sound, release gas (bubbles), color change Separating Substances: Ex. Cleaning tarnished silver, purifying metals. Ex. Cleaning tarnished silver, purifying metals. A chemical change will change the substances, so it cannot be used to separate a mixture. A chemical change will change the substances, so it cannot be used to separate a mixture.

28. Chemical Change The change of one substance to another is a chemical change 6 Clues that a chemical change has occurred Color change Color change Bubbles (not boiling) Bubbles (not boiling) New odor New odor Heat or Cooling Heat or Cooling Light Light Sound Sound

29. Chemical Reaction Chemical change happens during a chemical reaction Never a change in the number of elements Energy is always taken in or given off

30. Weathering Weathering is how Earth’s surface changes. Weathering is a result of both physical & chemical changes. Physical: ice wedging (ice in cracks expands & breaks the rocks), & streams cut through softer rock. Chemical: limestone dissolves in acidic ground water (canyons & caves are formed this way)

31. Caves are formed through chemical weathering. Ice wedging or the freeze/thaw cycle breaks rocks into pieces

32. Conservation of Mass Law of Conservation of Mass—the mass of all substances before a chemical or physical change equals the mass of all substances after the change. In other words: mass is neither created nor destroyed during any chemical or physical change.