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The Puzzle of Matter: Classification and Properties

Explore the classification of matter and learn about its properties. Understand the differences between elements, compounds, homogeneous mixtures, and heterogeneous mixtures. Discover how the structure of matter influences its behavior. Learn about physical changes, physical properties, and solutions.

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The Puzzle of Matter: Classification and Properties

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  1. Chapter Menu Section 1.1The Puzzle of Matter Section 1.2 Properties and Changes of Matter Click a hyperlink to view the corresponding slides. Chapter Menu

  2. The Puzzle of Matter Classify matter according to its composition. Distinguish between elements, compounds, homogeneous mixtures, and heterogeneous mixtures. Relate the properties of matter to structure. Section 1.1

  3. The Puzzle of Matter chemistry matter mass property scientific model qualitative quantitative substance mixture physical change physical property solution alloy solute solvent aqueous solution element compound formula Most everyday matter occurs as mixtures—combinations of two or more substances. Section 1.1

  4. A Picture of Matter Chemistry is the science that investigates and explains the structure and properties of matter. Matter is anything that takes up space and has mass. • The paper and ink of a book • The air you breathe Section 1.1

  5. A Picture of Matter (cont.) Mass is the measure of the amount of matter that an object contains. The propertiesof matter describe the characteristics and behavior of matter, including the changes that matter undergoes. • Macroscopic level of matter—based on behavior and observed composition of matter • Submicroscopic level of matter—used to determine how the hidden structure of matter influences its behavior Section 1.1

  6. Using Models in Chemistry A model of the submicroscopic structure of a piece of matter must be able to explain and predict the observed macroscopic behavior. Section 1.1

  7. Using Models in Chemistry (cont.) Scientific models are built on investigation and observation and explain macroscopic observations. Section 1.1

  8. Classifying Matter A qualitativeobservation is one that is made without measurement. A quantitative observation is one that is made with measurement. Section 1.1

  9. Classifying Matter (cont.) A substance is matter with the same fixed composition and properties. • Pure means that every bit of the matter being examined is the same substance. A mixture is a combination of two or more substances in which the basic identity of each substance is not changed. • Can be separated by physical processes Section 1.1

  10. Classifying Matter (cont.) A physical change is a change in matter that does not involve a change in the identity of the substance. • Includes boiling, freezing, melting, evaporating, dissolving, and crystallizing Section 1.1

  11. Classifying Matter (cont.) Physical properties are characteristics of a sample of matter that can be observed or measured without any change to its identity. • Includes solubility, melting point, boiling point, color, density, electrical conductivity, and physical state Section 1.1

  12. Classifying Matter (cont.) A heterogeneous mixture does not have a uniform composition and its individual substances remain distinct. A homogeneous mixture, or solution, always has a uniform composition and is the same throughout. An alloy is a solid solution that contains different metals and sometimes nonmetallic substances. Section 1.1

  13. Classifying Matter (cont.) Section 1.1

  14. Classifying Matter (cont.) The solute is the substance being dissolved. The solvent is the substance that dissolves the solute. When the solvent is water, the solution is called an aqueous solution. Section 1.1

  15. Substances: Pure Matter There are two types of pure substances—compounds and elements. Section 1.1

  16. Substances: Pure Matter (cont.) An element is the simplest form of matter. There are 117 elements—only 90 occur naturally on Earth. The periodic table organizes elements and uses chemical symbols that are universally understood. Section 1.1

  17. Substances: Pure Matter (cont.) Section 1.1

  18. Substances: Pure Matter (cont.) A compound is a chemical combination of two or more different elements joined together in a fixed proportion Section 1.1

  19. Substances: Pure Matter (cont.) Section 1.1

  20. Substances: Pure Matter (cont.) A chemical formula is a combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element. C12H22O11→ Section 1.1

  21. Section Assessment Scientific models explain ___ observations. A.macroscopic B.submicroscopic C.qualitative D.quantitative Section 1.1

  22. Section Assessment Which of the following is not a solution? A.gasoline B.steel C.air D.orange juice Section 1.1

  23. End of Section 1.1

  24. Properties and Changes of Matter Distinguish between physical and chemical properties. Contrast chemical and physical changes. Apply the law of conservation of matter to chemical changes. Section 1.2

  25. Properties and Changes of Matter matter: anything that takes up space and has mass Section 1.2

  26. Properties and Changes of Matter volatile density chemical property chemical change chemical reaction law of conservation of mass energy exothermic endothermic Matter can undergo physical and chemical changes. Section 1.2

  27. Physical Properties Physical properties are those that do not involve changes in composition. Physical properties can be either quantitative or qualitative. When salt is dropped into water, the particles in the salt crystal separate and are surrounded by water. Section 1.2

  28. Physical Properties (cont.) Most matter on Earth exists in one of three physical states: solid, liquid, or gas. Changes in state are examples of physical changes because there is no change in the identity of the substance. Some substances are volatile, or change to a gas easily at room temperature. Section 1.2

  29. Physical Properties (cont.) Density is the amount of matter (mass) contained in a unit of volume. Section 1.2

  30. Chemical Properties and Changes A chemical property can be observed only when there is a change in the composition of the substance. Chemical change, otherwise known as a chemical reaction, is the change of one or more substances into other substances. Section 1.2

  31. Chemical Properties and Changes (cont.) According to the law of conservation of mass, matter is neither created nor destroyed in a chemical change. Section 1.2

  32. Chemical Properties and Changes (cont.) Energy, which is the capacity to do work, is either absorbed or released during a chemical change. Exothermic reactions are chemical reactions that give off heat energy. • Combustion of ammonium nitrate Section 1.2

  33. Chemical Properties and Changes (cont.) Endothermic reactions are chemical reactions that absorb heat energy. • Photosynthesis Section 1.2

  34. Section Assessment Which substance is considered volatile? A.alcohol B.naphthalene C.gasoline D.all of the above Section 1.2

  35. Section Assessment Photosynthesis is the most important ___ process on Earth. A.exothermic B.endothermic C.physical D.qualitative Section 1.2

  36. End of Section 1.2

  37. Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion Resources Menu

  38. Key Concepts Chemists study matter. Macroscopic observations reflect the submicroscopic structure of matter. Mixtures are heterogeneous or homogeneous (solutions). Substances are classified as elements or compounds. Elements are the building blocks of all matter. Study Guide 1

  39. Key Concepts Every substance has a unique set of physical and chemical properties. The density of a sample of matter is the amount of matter (mass in grams) in a unit volume (usually a milliliter). Chemical changes—also called chemical reactions—involve substances forming different substances. In a chemical reaction, atoms are never created or destroyed. Physical and chemical changes absorb or release energy. Study Guide 2

  40. Which of the following items is not matter? A.clouds B.radio waves C.oxygen D.precipitation Chapter Assessment 1

  41. To determine what chemicals make up sucrose, what kind of analysis would one use? A.qualitative B.quantitative Chapter Assessment 2

  42. Which of the following is a substance? A.solder B.soil C.blood D.pure sucrose Chapter Assessment 3

  43. Which of the following can be separated by a physical process? A.submicroscopic matter B.pure substance C.mixture D.element Chapter Assessment 4

  44. The melting point of a sample of matter is a characteristic of its ___. A.physical change B.physical property C.mass D.volume Chapter Assessment 5

  45. Which of the following is an aqueous solution? A.gasoline B.orange juice C.soft drink D.kerosene STP 1

  46. Most of the processes of life occur in aqueous solutions. A.true B.false STP 2

  47. Which of the following is not an element? A.ammonia B.carbon C.hydrogen D.gold STP 3

  48. The physical state of a substance depends on its ___. A.mass B.composition C.temperature D.volume STP 4

  49. To determine density, it is necessary to measure its ___. A.mass B.temperature C.volume D.A and C STP 5

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