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Substances

Unit 1 Lessons 4-6 -Elements, Compounds, and Mixtures -Solids, Liquids and Gases -Change of State. Substances. Elements: Pure substance in its simplest form can’t be broken down physically or chemically Examples: Hydrogen, Oxygen, Gold. Pure Substances:

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Substances

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  1. Unit 1 Lessons 4-6-Elements, Compounds, and Mixtures-Solids, Liquids and Gases-Change of State

  2. Substances Elements: Pure substance in its simplest form can’t be broken down physically or chemically Examples: Hydrogen, Oxygen, Gold Pure Substances: Made of only one type of particle

  3. Characteristic Properties: Physical and chemical properties that help identify elements Examples: Boiling/Melting Points, Density, Color, Reactivity, Flammability Elements Categories of Elements: -Metals -Nonmetals -Metalloids

  4. Metals: shiny, conducts heat electricity well Copper, Tin, Lead Nonmetals: Dull, conduct heat and electricity poorly, solids tend to be brittle Metals and Nonmetals

  5. Metalloids • Have properties of both metals and nonmetals • Some conduct heat and electricity well, shiny or dull • Smallest portion on the periodic table

  6. Combination of two or more types of matter that are not chemically joined Parts retain their properties Can be separated by physical means (magnets, filtering) Made of atoms of two or more elements chemically joined Has properties like elements (density, b.p) Compounds properties differ than those of the individual elements Compounds Mixtures

  7. Do not react to form a compound Pizza: Tomato sauce, cheese, pepperoni Mixtures

  8. Homogeneous(evenly mixed) mixture of two or more substances dispersed through a single phase Same appearance and properties throughout the mixture Salt water solution: Solute (salt): substance that dissolves in the solvent Solvent (water): substance in which the solute dissolves Solutions

  9. Concentration: the amount of solute dissolved in a solvent (g/ml) What is the concentration of a solution if it has 100 g of sugar dissolved in 200 milliliters of water? 100 g of sugar/ 200 ml of water .5 g/ml Concentration of Solutions

  10. States of Matter Solids Liquids Gases No Yes Farther than solid Weaker than solid Flow freely No No Very far apart Very weak Rapidly in straight lines Yes Yes Very Close together Very strong Vibrate back and forth

  11. Measure of how hot or cold something is Temperature

  12. Amount of space that an object takes up Volume

  13. Amount of force exerted on an area Pressure

  14. Boyle’s Law: Volume of a gas is inversely proportional to the pressure of a gas when temperature is constant “Boyle The Pickle Vines… opposite” Gas Laws

  15. Charles Law: Volume of a gas is directly proportional to the temperature when pressure is constant “Charles Pumped The Volume….up” Gas Laws

  16. Change of a substance from one state to another Change of State

  17. Change of State • Melting Point: the temperature at which a solid changes to a liquid • Freezing Point: the temperature at which a liquid changes to a solid • Evaporation Point: the temperature at which a liquid changes to a gas (Boiling Point of water is 212) • Condensation Point: the temperature at which a gas changes to a liquid • Sublimation: process in which a solid changes directly to a gas • Deposition: process in which a gas changes directly into a solid

  18. Change of State Diagram of Water Temperature C 100 Blue = solid Red = liquid Green = gas 0 Time (s)

  19. Water Change of State Diagram Be neat, colorful, creative and neat! Requirements: Title Labels and descriptions for: melting/freezing points, boiling/condensing points, solids, liquids, gases X and Y axis labels and units Color coded key

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