2. Chapter Menu Matter—Properties and Change Section 3.1Section 3.1Properties of Matter Section 3.2Section 3.2 Changes in Matter Section 3.3Section 3.3 Mixtures of Matter Section 3.4Section 3.4 Elements and Compounds Exit Click a hyperlink or folder tab to view the corresponding slides.

3. Section 3-1 Section 3.1 Properties of Matter Identify the characteristics of a substance. density: a ratio that compares the mass of an object to its volume Distinguish between physical and chemical properties. Differentiate among the physical states of matter.

4. Section 3-1 Section 3.1 Properties of Matter (cont.) states of matter solid liquid gas Vapor Plasma Most common substances exist as solids, liquids, and gases, which have diverse physical and chemical properties. physical property extensive property intensive property chemical property

5. Section 3-1 Substances Matter is anything that has mass and takes up space. Matter is everything around us. Matter with a uniform and unchanging composition is a pure substance. Particles of matter are always in motion. The kinetic energy (speed) of these particles increases as temperature increases.

6. Section 3-1 States of Matter The physical forms of matter, either solid, liquid, or gas, are called the states of matter.states of matter Solids are a form of matter that have their own definite shape and volume. Very Low Kinetic EnergySolids Liquids are a form of matter that have a definite volume but take the shape of the container. Low Kinetic EnergyLiquids

7. Section 3-1 States of Matter (cont.) Gases have no definite shape or volume. They expand to fill their container. Very High Kinetic EnergyGases Vapor refers to the gaseous state of a substance that is normally a solid or liquid at room temperature.Vapor Plasma very high kinetic energy- particles collide with enough energy to break into charged particles (+/-). gas-like, variable shape & volume

8. Section 3-1 Physical Properties of Matter A physical property is a characteristic that can be observed or measured without changing the sample’s composition.physical property

9. Section 3-1 Physical Properties of Matter (cont.) Extensive properties are dependent on the amount of substance present, such as…Extensive properties Intensive properties are independent of the amount of substance present, such as…Intensive properties

10. A. Extensive vs. Intensive Examples: –boiling point –volume –mass –density –conductivity intensive extensive intensive Extensive vs. Intensive

11. Section 3-1 Chemical Properties of Matter The ability of a substance to combine with or change into one or more other substances is called a chemical property.chemical property describes the ability of a substance to undergo changes in identity –Examples:

12. Section 3-1 Observing Properties of Matter A substance can change Chemical properties can change with specific environmental conditions, such as temperature and pressure.

13. B. Physical vs. Chemical Examples: –melting point –flammable –density –magnetic –tarnishes in air physical chemical physical chemical Physical vs. Chemical

14. Section 3-2 Section 3.2 Changes in Matter Define physical change and list several common physical changes. observation: orderly, direct information gathering about a phenomenon Define chemical change and list several indications that a chemical change has taken place. Apply the law of conservation of mass to chemical reactions.

15. Section 3-2 Section 3.2 Changes in Matter (cont.) Matter can undergo physical and chemical changes. physical change phase change chemical change law of conservation of mass

16. Section 3-2 Physical Changes A change that alters a substance without changing its composition is known as a physical change. physical change A phase change is a transition of matter from one state to another.phase change Examples:

17. SOLID  LIQUID Melting LIQUID  GAS Boiling or Evaporation GAS  LIQUID Condensing SOLID  GAS Sublimation GAS  SOLID Reverse Sublimation or Deposition LIQUID  SOLID Freezing, Solidifying or Crystallizing

18. Section 3-2 Chemical Changes A change that involves one or more substances turning into new substances is called a chemical change.chemical change changes the identity of a substance products have different properties Examples:

19. B. Physical vs. Chemical Signs of a Chemical Change –change in color or odor –formation of a gas –formation of a precipitate (solid) –change in light or heat http://www.youtube.com/watch?v=QL7V3 L3dfDM

20. B. Physical vs. Chemical Examples: –rusting iron –dissolving in water –burning a log –melting ice –grinding spices chemical physical chemical physical Physical vs. Chemical

21. B. Physical vs. Chemical Reaction occurs when one or more substances are changed into new substances. Reactants- stuff you start with; elements or compounds Products- What you make products have NEW PROPERTIES Yields Arrow separates reactants and products

22. Section 3-2 Conservation of Mass The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.law of conservation of mass The mass of the reactants equals the mass of the products. mass reactants = mass products

23. Section 3-3 Section 3.3 Mixtures of Matter Contrast mixtures and substances. substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance Classify mixtures as homogeneous or heterogeneous. List and describe several techniques used to separate mixtures.

24. All mixtures can be separated though some type of physical process. Yes, I agree with this statement because… No, I disagree with this statement because… YES – NO – WHY?

25. Section 3-3 Mixtures A mixture is a physical combination of two or more pure substances in which each pure substance retains its individual chemical properties.mixture A homogenous mixture is a mixture where the composition is constant throughout.homogenous mixture Homogeneous mixtures are also called solutions.solutions Examples…

26. C. Mixtures Solution –homogeneous –very small particles –no Tyndall effect Tyndall Effect –particles don’t settle –EX: rubbing alcohol

27. Section 3-3 Mixtures (cont.)

28. Section 3-3 Mixtures (cont.) A heterogeneous mixture is a mixture where the individual substances remain distinct.heterogeneous mixture mixture is not uniform in composition Examples…

29. C. Mixtures Colloid –heterogeneous –medium-sized particles –Tyndall effect –particles don’t settle –EX: milk

30. C. Mixtures Suspension –heterogeneous –large particles –Tyndall effect –particles settle –EX: fresh-squeezed lemonade

31. C. Mixtures Examples: –mayonnaise –muddy water –fog –saltwater –Italian salad dressing colloid suspension colloid solution suspension

32. Section 3-3 Separating Mixtures Filtration is a technique that uses a porous barrier to separate a solid from a liquid in a heterogeneous mixture.Filtration Distillation is a separation technique for homogeneous mixtures that is based on the differences in boiling points of substances.Distillation Crystallization is a separation technique for homogenous mixtures that results in the formation of pure solid particles from a solution containing the dissolved substance.Crystallization

33. Section 3-3 Separating Mixtures (cont.) Sublimation is the process of a solid changing directly to a gas, which can be used to separate mixtures of solids when one sublimates and the other does not.Sublimation Chromatography is a technique that separates the components of a mixture on the basis of tendency of each to travel across the surface of another material.Chromatography

34. Section 3-4 Section 3.4 Elements and Compounds Distinguish between elements and compounds. proportion: the relation of one part to another or to the whole with respect to quantity Describe the organization of elements in the periodic table. Explain how all compounds obey the laws of definite and multiple proportions.

35. Section 3-4 Elements An element is a pure substance that cannot be separated into simpler substances by physical or chemical means.element 92 elements occur naturally on Earth. Each element has a unique name and a one, two, or three-letter symbol. The periodic table organizes the elements into a grid of horizontal rows called periods and vertical columns called groups.periodic table

36. Section 3-4 Compounds A compound is a made up of two or more elements combined chemically.compound Most of the matter in the universe exists as compounds. Table salt, NaCl, and water, H 2 O, are compounds.

37. Section 3-4 Compounds (cont.) Elements can never be separated. Compounds can be broken into components by chemical means.

38. A. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous Mixture CompoundElement MIXTUREPURE SUBSTANCE yes no Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions

39. Section 3-4 Law of Definite Proportions The law of definite proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample.law of definite proportions

40. Section 3-4 Law of Definite Proportions (cont.) The relative amounts are expressed as percent by mass, the ratio of the mass of each element to the total mass of the compound expressed as a percentage. percent by mass

41. Section 3-4 Law of Definite Proportions (cont.) This table demonstrates that the percentages of elements in sucrose remain the same despite differences in sample amount.

42. Section 3-4 Law of Multiple Proportions The law of multiple proportions states that when different compounds are formed by a combination of the same elements, different masses of one element combine with the same relative mass of the other element in whole number ratios.law of multiple proportions –H 2 O 2 and H 2 O –Copper(I) chloride and copper(II) chloride

43. Section 3-4 Law of Multiple Proportions (cont.)