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Physical Property

This guide explains the fundamental concepts of physical and chemical properties of matter. Learn about color, luster, malleability, and conductivity as physical properties, and reactivity, chemical change, and synthesis as chemical properties. Understand the difference between physical and chemical changes, elements, compounds, and mixtures. Discover methods of separating mixtures, such as distillation, filtration, and sorting, and learn about homogeneous and heterogeneous mixtures. Explore the phases of matter, the characteristics of compounds and elements, and the importance of physical constants in understanding matter.

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Physical Property

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  1. Physical Property Describes form or behavior of matter

  2. Color Luster Malleability Conductivity Hardness Cleavage Phase at room temp. Vapor pressure Melting point Boiling point Heat of fusion Heat of vaporization Density Specific Heat Capacity Physical Properties Physical constants!

  3. Chemical Property Describes how matter interacts with other matter: reactivity

  4. Chemical Change Identity Change

  5. Examples of Chemical Change Synthesis, Decomposition, Single Replacement, Double Replacement, Combustion, Polymerization, Esterification, etc.

  6. Monatomic One-atom Molecule

  7. 1 uppercase letter in formula Element

  8. 2 or more uppercase letters in formula Compound

  9. Physical Change Identity stays the same

  10. H2O(l)  H2O(g) Phase changes are physical changes. Identity stays the same.

  11. 2H2O(l)  2H2 + O2(g) Identity changes. Chemical change.

  12. Diatomic 2-Atom Molecule

  13. Gases Take the shape & volume of their container

  14. Physical Constant Physical property expressed with a # & unit. Independent of sample size.

  15. Liquids Definite volume but no definite shape

  16. Solids Definite volume & definite shape

  17. Compound 2 or more elements chemically combined

  18. Element Cannot be broken down into anything simpler by ordinary chemical or physical methods

  19. Mixture Physical combination of 2 or more pure substances.

  20. Pure Substances Elements & Compounds

  21. Mixtures Heterogeneous or Homogeneous

  22. Distillation Physical method of separating mixture of 2 or more liquids based on differences in boiling points.

  23. Solution Homogeneous Mixture. Liquid & gas phase solutions transmit light. Look translucent. Do not separate on standing.

  24. Suspension Heterogeneous Mixture. Scatter light. Look cloudy. Need to be shaken or stirred. Separate on standing.

  25. NaCl(aq) Homogeneous Mixture. NaCl dissolved in water.

  26. NaCl(s) Pure substance. NaCl in the solid phase.

  27. Variable Composition Mixture

  28. NaCl(l) Pure substance. NaCl in the liquid phase.

  29. NaCl(g) Pure substance. NaCl in the gas phase.

  30. Homogeneous Uniform, constant, the same throughout.

  31. Heterogeneous Non-uniform composition. May see regions that look different. May be more than 1 phase present.

  32. Always Homogeneous Pure substance: Element or Compound

  33. Filtration Physical separation technique used to separate heterogeneous mixtures. Based on differences in particle size.

  34. Sorting Physical separation technique used to separate heterogeneous mixtures. Based on differences in appearance.

  35. Definite & Unique Properties Pure substance. Element or Compound.

  36. Broken into components by chemical decomposition reaction Compound

  37. Definite Composition Pure substance. Element or Compound.

  38. Separated by physical technique Mixture

  39. Triatomic 3-atom Molecule

  40. May be homogeneous or heterogeneous Mixture

  41. Density, melting point, boiling point Examples of physical constants

  42. Law of conservation of matter Mass Before = Mass After

  43. The equation is a distractor. 44 + 128 – 32 = grams Z = 140 g. Given: X + 2Y  Q + 3Z Mass Before = Mass After When 44 grams of X react completely with 128 grams of Y, 32 grams of Q are produced. How much Z will be made?

  44. No new properties. Properties are a mix of properties of components. Mixture

  45. C6H12O6(s)  C6H12O6(aq) Equation represents dissolving. Dissolving is a physical change.

  46. Physical Properties Used to identify substances.

  47. Atoms can vibrate back & forth about a fixed position. Solid state

  48. Phys. M. Chem. (suspensions) (solutions) Mixtures  Separated by physical methods. Compounds  Separated by chemical methods.

  49. Sorting Filtration Crystallization Evaporation Distillation Chromatography Differences in density Differences in magnetic properties Differences in solubility Ways to separate heterogeneous mixtures

  50. Evaporation = Freezing = Melting = Condensation = Boiling = Deposition = Fusion = Vaporization = Sublimation = Change of phase terms Liquid to gas Liquid to solid Solid to liquid Gas to liquid Liquid to gas Gas to solid Solid to liquid Liquid to gas Solid to gas

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