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Matter and Changes: Physical vs. Chemical Properties and Reactions

Learn about the properties of matter, physical changes, chemical properties, phases of matter, mixtures, pure substances, and practice classifying elements, compounds, and mixtures in this detailed chapter.

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Matter and Changes: Physical vs. Chemical Properties and Reactions

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  1. Chapter 2 Matter and Change

  2. Physical Properties Density Mass Volume Texture Temperature Color Odor Taste Conductivity Boiling Point Melting Point Physical Changes – does not change the chemical make-up. Change in state Melting Boiling Freezing Evaporating Condensing Dissolving Tearing/Ripping/Cutting Properties of Matter - All matter has mass and takes up space.

  3. Chemical Properties Oxidizes Rusts Decomposes Explodes Burns Corrodes Reacts with … Chemical Change Evidence New substance forms New color New texture New odor Bubbles of gas are produced Energy is produced Heat Light Electricity Properties of Matter

  4. Extensive and Intensive Properties • Extensive – a property that is dependent on the amount of matter present. • Examples • Mass • Volume • Intensive – a property that is independent on the amount of matter present. • Examples • Color • density

  5. Practice • Which of the following are chemical changes (C) and which of the following are physical changes (P)? • Making caramel from sugar • Carving a wooden figurine • Freezing mercury metal • Cake batter being baked into a cake • Dissolving salt into water C P P C P

  6. Phases of Matter • Solid – definite shape and volume • Liquid – indefinite shape and definite volume • Gas – indefinite shape and volume

  7. Mixtures • Combination of two or more substances where each substance retains it properties. • Substances are not chemically bonded. • Most mixtures can be separated by physical means.

  8. Heterogeneous Mixture • A mixture that does not have uniform composition. • Examples • Salad • Orange juice • Sand

  9. Homogeneous Mixture • A mixture that does have uniform composition. • Examples • Salt Water • Air • Bronze • Know also as solutions.

  10. Separating Mixtures • Salad • By hand • Iron filings and sand • Magnet • Sugar and water • Evaporation • Water and metal ions • Distillation • Water and cornstarch • Filtering or centrifuging

  11. Pure Substances • Made of only one type of matter. • Have a uniform and definite composition. • Cannot be broken down by physical means. • Examples • Elements • Compounds

  12. Elements • Made of one type of atom • Examples • Iron • Oxygen • Sodium • Symbols • Consist of a capital letter and if a second letter, it must be lowercase.

  13. Compounds • Made of one type of molecule • Examples • Sugar • Rubbing alcohol • Salt • Symbols • Consist of element symbols and subscripts • Subscript – small number that appears to the right of the element it multiplies. • Example: H2O • 1- oxygen 2 - hydrogen

  14. Practice • Classify each substance as a pure substance or a mixture. • Silver • Alphabet soup • Soda pop • Carbon dioxide Pure substance Mixture Mixture Pure Substance

  15. Practice • Classify each pure substance as an element or compound. And classify each mixture as hetero- or homogeneous. • Silver • Alphabet soup • Soda pop • Carbon dioxide Element Heterogeneous Mixture Homogeneous Mixture Compound

  16. Practice • A clear liquid was left in an open container and is allowed to evaporate. A white residue is left after three days. Was the original liquid an element, compound, or a mixture? How do you know?

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