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Physical Property

This article explores the various properties of matter, including physical and chemical properties, changes, and the differences between pure substances and mixtures. It also discusses the concepts of density, melting point, boiling point, and the law of conservation of mass.

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Physical Property

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  1. Physical Property Describes form or behavior of matter

  2. Independent of sample size(density, melting point, boiling point, etc.) Intensive Properties

  3. Depend on how much stuff!(Mass & Volume) Extensive Properties

  4. Chemical Property Describes how matter interacts with other matter

  5. Chemical Change Identity Change A new substance is formed.

  6. Chemical ChangeIdentities change! Note: particle diagram shows conservation of mass: same # of each type of atom on reactant and product sides.

  7. Monatomic One-atom Molecule

  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. Smallest particle of an element that retains the properties of the element and that can participate in a chemical reaction. Atom

  14. Gases Take the shape & volume of their container

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

  16. Liquids Definite volume but no definite shape

  17. Solids Definite volume & definite shape

  18. Compound 2 or more elements chemically combined

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

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

  21. Pure Substances Elements & Compounds

  22. Pure Substances The particles in each case are identical to each other. Type of Matter?

  23. Mixtures Heterogeneous or Homogeneous

  24. Heterogeneous Mixtures Type of Mixtures?

  25. Homogeneous Mixtures! Type of Mixtures?

  26. Pure Substance! Mixture or Pure Substance?

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

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

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

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

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

  32. Variable Composition Mixture

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

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

  35. Homogeneous Uniform, constant, the same throughout.

  36. Always Homogeneous Pure substance: Element or Compound

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

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

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

  40. Broken into components by chemical decomposition reaction Compound

  41. Definite Composition Pure substance. Element or Compound.

  42. Separated by physical technique Mixture

  43. Triatomic 3-atom Molecule

  44. May be homogeneous or heterogeneous Mixture

  45. Compare pure substances & mixtures

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

  47. Law of conservation of mass (lab scale) Total Mass of Reactants = Total Mass of Products

  48. Total # of atoms of each type on reactant side = • Total # of atoms of each type on product side Law of conservation of mass (microscale)

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

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

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