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Chapter 10 Notes

Chapter 10 Notes. Kinetic Theory: Particles in all states of matter are in constant motion . constant motion. Particles in solid state. Motion is a vibration about a fixed point. Kinetic Theory: . Particles in solid state. Heat makes particles move faster . Kinetic Theory: .

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Chapter 10 Notes

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  1. Chapter 10 Notes Kinetic Theory: Particles in all states of matter are in constant motion. constant motion

  2. Particles in solid state Motion is avibrationabout a fixed point Kinetic Theory:

  3. Particles in solid state Heat makes particles movefaster. Kinetic Theory:

  4. Particles in solid state More energy = faster particles Kinetic Theory:

  5. Particles in solid state Temperature measures averagekineticenergyKEave. Kinetic Theory:

  6. Melting: (solidliquid) Particles move out of fixed positions Kinetic Theory:

  7. Particles in liquid state Particles can flow. Kinetic Theory:

  8. Gasesare composed of particles that are very small, hard spheres that are relatively farapart.

  9. There is lots of emptyspace between the gas particles.

  10. There is no significant attractive or repulsive force between the gas particles.

  11. The gas particles move rapidly in constant random motion in a straight line.This is called a random walk.

  12. Gas particles only change direction if they collide with another gas particle or the wall of the container.

  13. All collisions are perfectly elastic. In other words,Kinetic energy is transferred without any loss in the collision.

  14. The Nature of Gases • Gases expand to fill their containers • Gases are fluid – they flow • Gases have low density (1/1000 the density of the equivalent liquid or solid) • Gases are compressible • Gases effuse and diffuse

  15. Diffusion Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.

  16. Uncontained gases can diffuse into space without limit.

  17. Effusion Effusion: describes the passage of gas into an evacuated chamber.

  18. Pressure • is equal to force/unit area • SI units = Newton/meter2 = 1 Pascal (Pa)

  19. Pressure • Is caused by the collisions of molecules with the walls of a container • is equal to force/unit area • SI units = Newton/meter2 = 1 Pascal (Pa) • 1 standard atmosphere = 101,325 Pa • 1 standard atmosphere = 1 atm = 101.3 kPa =760 mm Hg Note: 760 mm Hg = 760 Torr

  20. Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli during the 17th century. The device was called a “barometer” • Baro = weight • meter = measure

  21. An Early Barometer The normal pressure due to the atmosphere at sea level can support a column of mercury that is 760 mm high.

  22. The Aneroid Barometer

  23. The Digital Barometer

  24. Standard Temperature and Pressure“STP” • P = 1 atm. = 101.3 kPa = 760 mm Hg • T = 0°C, 273 Kelvin • 1 mole of an ideal gas = 22.4 L @ STP

  25. Converting Pressure Units.1 atmosphere (atm) = 760 mm Hg (Torr) = 101.3 kiloPascals (kPa) Convert 2.5 atm to kPa 101.3 kPa 253.25 1 atm

  26. Converting Pressure Units.1 atmosphere (atm) = 760 mm Hg (Torr) = 101.3 kiloPascals (kPa) Convert 2.5 atm to mm Hg 760 mm Hg 1900 1 atm

  27. Converting Pressure Units.1 atmosphere (atm) = 760 mm Hg (Torr) = 101.3 kiloPascals (kPa) Convert 732 mm Hg to kPa 101.3 kPa 97.6 760 mm Hg

  28. Converting Pressure Units.1 atmosphere (atm) = 760 mm Hg (Torr) = 101.3 kiloPascals (kPa) Convert 120 kPa to mm Hg 760 mm Hg 900.3 101.3 kPa

  29. Electronegativity The ability of an atom in a molecule to attract shared electrons to itself. Linus Pauling 1901 - 1994

  30. Table of Electronegativities

  31. Covalent Bonds(Nonmetals with Nonmetals) Nonpolar-Covalent bonds • Electrons are equally shared • Electronegativity difference of 0 to 0.4 • All diatomic molecules are nonpolar: H2, F2, etc… Polar-Covalent bonds • Electrons are unequally shared • Electronegativity difference between .4 and 1.7

  32. Polarity A molecule, such as FCl, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment. Unequal sharing of electrons Cl Difference in Electronegativity: - F + • 4.0 • 3.0 • 1.0 Electronegativity: (From periodic table) 4.0 3.0 A Dipole forms with a partial (+) and partial (-) side The electronegativity difference is 1.0 So the molecule is Polar with a permanent (+) and (-) side

  33. Table of Electronegativities

  34. Ionic compounds: (metals w/ nonmetals) Starts with a metal or ammonium, NH4+ Molecular compounds: (all nonmetals) Starts with a nonmetal Location of metals, metalloids, and nonmetals

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