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Section 1: Classifying Matter

Section 1: Classifying Matter. Preview Key Ideas Bellringer What is Matter? Elements Elements in the Human Body Compounds Pure Substances and Mixtures Types of Mixtures. Key Ideas. How can matter be classified? Why are carbon and copper classified as elements?

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Section 1: Classifying Matter

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  1. Section 1:Classifying Matter Preview • Key Ideas • Bellringer • What is Matter? • Elements • Elements in the Human Body • Compounds • Pure Substances and Mixtures • Types of Mixtures

  2. Key Ideas • How can matter be classified? • Why are carbon and copper classified as elements? • How are elements related to compounds? • What is the difference between a pure substance and a mixture?

  3. What is Matter? • How can matter be classified? • Every sample of matter is either an element, a compound, or a mixture. • matter:anything that has mass and takes up space

  4. Visual Concept: Matter

  5. Elements • Why are carbon and copper classified as elements? • Each element is made of one kind of atom. • element:a substance that cannot be separated or broken down into simpler substances by chemical means • atom:the smallest unit of an element that maintains the properties of that element

  6. Elements in the Human Body

  7. Elements, continued • Elements are represented by symbols. • Atoms that make up a molecule act as a unit. • molecule:a group of atoms that are held together by chemical forces; a molecule is the smallest unit of matter that can exist by itself and retain all of a substance’s chemical properties.

  8. Visual Concept: Elements

  9. Compounds • How are elements related to compounds? • Each molecule of a compound contains two or more elements that are chemically combined. Elements combine chemically to form a compound. • compound:a substance made up of atoms of two or more different elements joined by chemical bonds

  10. Visual Concept:Compounds

  11. Compounds,continued • Compounds have unique properties. • Chemical formulas represent compounds. • The following chemical formula represents the compound for indigo:

  12. Visual Concept:Chemical Formula

  13. Pure Substances and Mixtures • What is the difference between a pure substance and a mixture? • Elements and compounds are pure substances, but mixtures are not. • pure substance:a sample of matter, either a single element or a single compound, that has definite chemical and physical properties • mixture:a combination of two or more substances that are not chemically combined

  14. Pure Substances and Mixtures, continued • Mixtures are classified by how thoroughly the substances mix. • heterogeneous mixture:substances aren’t mixed uniformly and are not evenly distributed • homogeneous mixture:substances are evenly distributed, and the mixture is the same throughout • miscible:substances that can be mixed • immiscible:substances that cannot be mixed • Gases can mix with liquids.

  15. Types of Mixtures

  16. Visual Concept:Comparing Miscible and Immiscible Liquids

  17. Understanding Concepts, continued • Which of the following terms most accurately describes carbon dioxide? F. element G. compound H. mixture I. solution

  18. Understanding Concepts, continued • Which of the following terms most accurately describes carbon dioxide? F. element G. compound H. mixture I. solution

  19. Interpreting Graphics, continued 9. Which of the following substances is classified as a compound? F. water G. ozone H. hydrogen gas I. solid sulfur

  20. Interpreting Graphics, continued 9. Which of the following substances is classified as a compound? F. water G. ozone H. hydrogen gas I. solid sulfur

  21. Interpreting Graphics, continued 10. A mixture contains 100 molecules of table salt, 30 molecules of baking soda, 20 molecules of ethanol, and 10 molecules of water. Atoms from which of the following elements make up most of the mixture? A. sodium, Na C. hydrogen, H B. oxygen, O D. carbon, C

  22. Interpreting Graphics, continued 10. A mixture contains 100 molecules of table salt, 30 molecules of baking soda, 20 molecules of ethanol, and 10 molecules of water. Atoms from which of the following elements make up most of the mixture? A. sodium, Na C. hydrogen, H B. oxygen, O D. carbon, C

  23. Interpreting Graphics, continued 11. A scientist discovers a way to easily combine molecules of ozone and molecules of hydrogen gas to make molecules of water. To create 300 molecules of water, how many molecules of ozone and how many molecules of hydrogen gas would the scientist need?

  24. Interpreting Graphics, continued 11. A scientist discovers a way to easily combine molecules of ozone and molecules of hydrogen gas to make molecules of water. To create 300 molecules of water, how many molecules of ozone and how many molecules of hydrogen gas would the scientist need? Answer: 100 molecules of ozone and 300 molecules of hydrogen gas

  25. Section2:Properties of Matter Preview • Key Ideas • Bellringer • Physical Properties • Math Skills • Chemical Properties

  26. Key Ideas • Why are color, volume, and density classified as physical properties? • Why are flammability and reactivity classified as chemical properties?

  27. Physical Properties • Why are color, volume, and density classified as physical properties? • Physical properties are characteristics that can be observed without changing the identity of the substance.

  28. Physical Properties, continued • Physical properties can help identify substances. • Physical properties can be observed or measured. • Examples: shape, color, odor, texture, state, melting point, boiling point, strength, hardness, magnetism, the ability to conduct electricity or heat • melting point:the temperature and pressure at which a solid becomes a liquid • boiling point:the temperature and pressure at which a liquid becomes a gas • Physical properties help determine uses.

  29. Visual Concept:Solid, Liquid and Gas

  30. Physical Properties, continued • Density is a physical property. • density:the ratio of the mass of a substance to the volume of the substance • common unit of density is g/cm3 • Density is different from weight.

  31. Visual Concept:Equation for Density

  32. Math Skills Density If 10.0 cm3 of ice has a mass of 9.17 g, what is the density of ice? 1. List the given and unknown values. Given: mass, m = 9.17 g volume, V = 10.0 cm3 Unknown:density, D = ? g/cm3

  33. Math Skills, continued 2. Write the equation for density. density = mass/volume, or D = m/V 3. Insert the known values into the equation, and solve. D = 0.917 g/cm3

  34. Understanding Concepts, continued 4. At 4 °C, the volume of 15 g of water was 15 cm3. At 20 °C, the volume of the same 15 g of water was 15.03 cm3. What effect did the increase in temperature have on the water’s density?

  35. Understanding Concepts, continued • At 4 °C, the volume of 15 g of water was 15 cm3. At 20 °C, the volume of the same 15 g of water was 15.03 cm3. What effect did the increase in temperature have on the water’s density? Answer: The density decreased.

  36. Understanding Concepts, continued 5. If the density of water changes because the temperature of the water changes, is this change a physical change or a chemical change?

  37. Understanding Concepts, continued • If the density of water changes because the temperature of the water changes, is this change a physical change or a chemical change? Answer: The change in density is a physical change.

  38. Understanding Concepts, continued • Study the graph below. Which has a greater density: water or gasoline?

  39. Understanding Concepts, continued • Study the graph below. Which has a greater density: water or gasoline? Answer: Water has a greater density than gasoline.

  40. Interpreting Graphics, continued 12. Which rock or rocks have the greatest density?

  41. Interpreting Graphics, continued 12. Which rock or rocks have the greatest density? Answer: Rock B

  42. Interpreting Graphics, continued 13. Which rock or rocks will float to the surface of the water in the cylinder? Why?

  43. Interpreting Graphics, continued 13. Which rock or rocks will float to the surface of the water in the cylinder? Why? Answer: Rock C, because its density is less than water’s.

  44. Chemical Properties • Why are flammability and reactivity classified as chemical properties? • A chemical property describes how a substance changes into a new substance, either by combining with other elements or by breaking apart into new substances.

  45. Chemical Properties, continued • Flammability is a chemical property. • flammability:the ability to burn • Reactivity is a chemical property. • reactivity:the capacity of a substance to combine chemically with another substance

  46. Chemical Properties, continued • Physical and chemical properties are different. • Physical properties can be observed without changing the identity of a substance. • Chemical properties can be observed only in situations in which the identity of the substance changes.

  47. Visual Concept:Comparing Physical and Chemical Properties

  48. Section 3: Changes of Matter Preview • Key Ideas • Bellringer • Physical Changes • Chemical Changes • Breaking Down Mixtures and Compounds

  49. Key Ideas • Why is getting a haircut an example of a physical change? • Why is baking bread an example of a chemical change? • How can mixtures and compounds be broken down?

  50. Physical Changes • Why is getting a haircut an example of a physical change? • A physical change affects one or more properties of a substance without changing the identity of the substance. • physical change:a change of matter from one form to another without a change in chemical properties

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