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Matter

Matter. Chapter 3. What is Matter?. Anything that has mass and takes up space. 2. Basic Building Blocks of Matter. Elements: Pure substances that cannot be separated into simpler substances Where can we find information about elements? Dmitri Mendeleev created the first periodic table.

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Matter

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  1. Matter • Chapter 3

  2. What is Matter? • Anything that has mass and takes up space. 2

  3. Basic Building Blocks of Matter • Elements: Pure substances that cannot be separated into simpler substances • Where can we find information about elements? • Dmitri Mendeleev created the first periodic table.

  4. Classifications of Matter • Substances: matter that has uniform and unchanging composition. • Ex. Table salt, water, hydrogen, oxygen

  5. Classifications of Matter • Mixture: combination of two or more substances in which the substances retain their individual chemical properties • Heterogeneous: does NOT blend, can distinguish parts • Homogeneous: does blend, CANNOT distinguish parts • Called solutions

  6. Compounds • Combination of two or more elements. • Ex. Table salt (Sodium Chloride), Water

  7. Physical Properties of Matter • A characteristic that can be observed without changing the composition • Ex. Density, color, odor, taste, hardness, melting point, and boiling point, state of matter

  8. Chemical Properties of Matter • The ability of a substance to combine with or change into one or more other substances. • Ex. Flammability, change into a new substance, rust

  9. Physical vs Chemical Change • Physical change: altering a substance appearance, but not its composition • Chemical change: altering a substance’s composition • Be careful…this also changes its appearance!!!

  10. Indicators of Chemical Change • Change of color (can also be physical change indicator) • Change heat (exothermic/endothermic) • Produces light • Produces gas (bubbles) • Forms precipitate (solid) • Change in smell

  11. Liquids • Takes the shape of its container • Volume is constant • viscosity – how easily it’s poured • Fluidity – ability to flow • Compression – compressed very little, gases have a greater ability to be compressed • Surface tension – overfilled glass of water • capillary action – meniscus, paper towels

  12. Solids • Definite shape • Definite volume • Tightly packed particles • Crystalline – salt • Molecular – sugar – weak forces • Amorphous – glass, rubber

  13. Gases • Do not have a definite shape • Do not have a definite volume • Can diffuse and effuse • Can be compressed and expanded • Have fluidity

  14. States of Matter

  15. States of Matter

  16. Liquids Gases Solids Phase Changes Sublimation Condensation Deposition Vaporization Melting Freezing

  17. Melting • Endothermic –heat is absorbed • Solid to a liquid • Melting point – temperature at which the forces holding the molecules together are broken • Example – Ice to water

  18. Vaporization • Endothermic • Liquid to a gas • Evaporation is vaporization on the surface • Boiling point – temperature at which the vapor pressure of a liquid equals the external pressure • Example: Water to steam

  19. Sublimation • Endothermic • Solid goes directly to a gas, not entering the liquid state • Example: Dry Ice

  20. Condensation • Exothermic – releases heat • Opposite of vaporization – gas to liquid • Dew in the morning • “sweat” on a glass

  21. Deposition • Exothermic • Gas to a solid without going through the liquid phase • Example: Snow

  22. Freezing • Exothermic • Liquid to a solid • Freezing point – temperature when a liquid is turned into a crystalline solid • Example: water to ice

  23. Which is which? • Endo-all the “ hot” changes • Exo – all the “cold” changes

  24. Phase Diagrams • Phase diagram – graph of pressure versus temperature that shows the condition required for a specific substance to undergo a phase change • Triple point – represents the temperature and pressure at which three phases of a substance can coexist • Critical point- max pressure and temperature the substance can exist as a liquid

  25. Phase Diagrams Con’t • Line that goes between liquid and solid – whichever phase the line is leaning towards, that phase is less dense than the other • Lines between all phases on a phase diagram indicate that both states of matter exist simultaneously (in equilibrium)

  26. Phase Diagrams - Water Which is more dense? Solid water or liquid water? Critical Point 217.75 Liquids Pressure (atm) Boiling point Solids Gas 1.00 Triple point 100.00 373.99 Temperature (°C)

  27. Worksheet • Answer the questions about the phase diagram.

  28. Conservation of Mass • According to the Law of Conservation of Mass states that matter can neither be created nor destroyed in a chemical change (reaction) • Mass reactants = Mass products

  29. Example Problem 3-1 • In an experiment, 10.00 g of red mercury (II) oxide powder is placed in an open flask and heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What is the mass of oxygen formed in the reaction?

  30. Analyze the Problem • What is/are the reactant(s)? • Mercury (II) oxide • What is/are the product(s)? • Oxygen and mercury

  31. Solve for Unknown • Mass reactants = Mass products • Mass Mercury (II) oxide= Mass oxygen + Mass of Mercury • 10.00g = x + 9.26g • Mass of oxygen (x) = 10.00g -9.26g • Mass of oxygen = 0.74g

  32. Percent by Mass • Is used to determine if compounds made of the same elements are the same… • Mass of element x 100 • Mass of compound

  33. Example Problem • A 78.0g sample of an unknown compound contains 12.4g of hydrogen. What is the percent by mass of hydrogen in the compound? • % =mass of hydrogen x 100 • mass of compound • Answer: 15.9%

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