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States of Matter

States of Matter. Chapter 13. Matter. Remember all matter is made up of tiny particles – either atoms, ions or molecules depending on what matter you are talking about The particles are in constant motion. Kinetic-Molecular Theory. Describes the motion of individual molecules

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States of Matter

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  1. States of Matter Chapter 13

  2. Matter • Remember all matter is made up of tiny particles – either atoms, ions or molecules depending on what matter you are talking about • The particles are in constant motion

  3. Kinetic-Molecular Theory • Describes the motion of individual molecules • Kinetic = “to move” • Also called Kinetic Theory

  4. Forces of Attraction Affect on States of Matter • At room temperature (20oC-25oC, 68oF-77oF) all particles of matter have the same kinetic energy • So why do we have different states of matter for these materials? • There are different strengths of INTERMOLECULAR FORCES

  5. 13.2 Forces of Attraction Intermolecular Forces What holds molecules together

  6. Properties of Molecules • Most have LOW melting & boiling points • tend to be gases and liquids at room temperature • Ex: CO2, NH3, H2O • Polar and Nonpolar molecules have a little bit different properties due to the partial charges.

  7. - + d+ H - F d+ H - F d- d- d- H - F d+ d+ d- H - F H - F d+ d- d- H - F d+ d+ d+ H - F H - F d- d-

  8. Intermolecular Forces • They are what make solid and liquid molecular compounds possible. • The weakest are called van der Waal’s forces - there are two kinds • Dispersion forces (London forces) • Dipole Interactions

  9. Dispersion Force • Depends only on the number of electrons in the molecule • Bigger molecules more electrons • More electrons stronger forces • F2 is a gas • Br2 is a liquid • I2 is a solid All are nonpolar but why are they different states of matter?

  10. d- d- d+ d+ d- d+ H H H H H H H H H H H H Dispersion force

  11. Dispersion Force • Occurs between all molecules • Depends only on the number of electrons in the molecule • Result from a temporary shift in density of electrons in electron clouds • Causes nonpolar molecule to become polar • Happens quickly and temporarily for nonpolar molecules

  12. Dipole interactions • Occur when polar molecules are attracted to each other. • Slightly stronger than dispersion forces. • Opposites attract but not completely hooked like in ionic solids.

  13. d+d- d+d- H F H F Dipole interactions • Occur when polar molecules are attracted to each other. • Slightly stronger than dispersion forces. • Opposites attract but not completely hooked like in ionic solids.

  14. Hydrogen bonding • Are the attractive force caused by hydrogen bonded to F, O, or N. • F, O, and N are very electronegative so it is a very strong dipole. • Causes hydrogen to have a large partial positive charge on it • The molecules are small, so they can get close together • The hydrogen partially share with the lone pair of electrons on an atom in a neighboring molecule • The strongest of the intermolecular forces.

  15. d- d+ O d+ H d+ d- H H O H d+ Hydrogen Bonding

  16. H O O H H O H H H H O H H H H O O O H H H Hydrogen bonding

  17. Hydrogen bonding is the reason why water has unique properties compared to other molecules its same size • Properties: • It is a liquid at room temp. • It is a good solvent • It is less dense as a solid (ice floats) • Just remember Water is not the only molecule that has hydrogen bonds.

  18. Examples: • What type of intermolecular forces do the following molecules have? • NH3 • O2 • CO2 • HBr • Which of the following compounds can form dipole-dipole forces: Cl2, CO, NO, CH4 Hydrogen bonding Dispersion forces Dispersion forces Dipole-dipole forces

  19. 13.4 Phase Changes • What is a phase? • The distinct states of matter when they are in mixtures • How is this different from just states of matter? • Occur due to changes in temperature.

  20. Phase changes that need energy • Melting • Heat of Fusion • Melting Point • KMT?

  21. Vaporization • Heat of Vaporization • How is this different from evaporation? • KMT?

  22. Boiling Point • Normal Boiling Point • KMT?

  23. Sublimation – • Dry Ice • Ice in the Freezer • KMT?

  24. Phase Changes that Release Energy • Condensation • What is this the reverse of? • KMT?

  25. Freezing • Freezing Point • How do the melting point & freezing points of a substance compare? • KMT?

  26. Deposition • What is this the reverse of? • KMT?

  27. Liquids • Flow • Fluidity • Viscosity • Density • Compression

  28. Surface tension • Cohesion vs. Adhesion • Capillary action

  29. Solids • Density

  30. Types • Crystalline • Amorphous

  31. Properties of Solid Molecules • Molecular solids – molecules held together by attractive forces • Ex: BI3, Dry Ice, sugar • Network solids- atoms held together by bonds • One big molecule (diamond, graphite) • High melting & boiling points, brittle, extremely hard • Metallic solids – positive ions surrounded by sea of e-

  32. Graphite Diamond

  33. Heating Curve

  34. Vapor Pressure Graphs

  35. Phase Diagram For Water

  36. Phase Diagram For CO2

  37. Video lesson Water, a polar molecule, on YouTube: http://www.youtube.com/watch?v=DVCYlST6mYQ

  38. Review Ionic and Covalent Compounds Practice Quiz and Graphics: http://www.elmhurst.edu/~chm/vchembook/145Areview.html

  39. Internet resources • Molecular polarity: http://www.elmhurst.edu/~chm/vchembook/210polarity.html • Polar covalent compounds: http://www.elmhurst.edu/~chm/vchembook/152Apolar.html • Nonpolar covalent compounds: http://www.elmhurst.edu/~chm/vchembook/150Anpcovalent.html • Ionic compounds: http://www.elmhurst.edu/~chm/vchembook/143Aioniccpds.html • Compare Ionic, Polar, and Nonpolar Bonds: http://www.elmhurst.edu/~chm/vchembook/153Acompare.html

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