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States of Matter: Kinetic-Molecular Theory Explained

This lesson explores the Kinetic-Molecular Theory of Matter, which describes the characteristics and behavior of different states of matter. It discusses the properties of gases, liquids, and solids, including their intermolecular forces, particle arrangement, and motion. The lesson also covers measurable properties of gases and introduces the fourth state of matter, plasma.

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States of Matter: Kinetic-Molecular Theory Explained

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  1. THE STORY CONTINUES…

  2. …STATES OF MATTER Unit 1 (LESSON 5)

  3. Unit 1 – LESSON 5 “STATES of MATTER”

  4. MATTER: • all matter is composed of small particles (atoms ormolecules) • Kinetic-Molecular Theory of Matter states: (1) the DISTANCE between particles determines the state of the substance (2)particles are in constant motion (3)theMOTION of particles is different for each state of matter

  5. MATTER: Kinetic-Molecular Theory of Matter … • describes the characteristics of the states of matter • explains the behavior of matter by examining the molecular forces between particles and their energy • matter maintains the same chemical composition regardless of the state matter in which it exists (e.g.) water is H2O whether it’s a solid, liquid or gas

  6. MATTER: Kinetic-Molecular Theory of Matter … • particles of substances at a given temperature have the SAME average KINETIC ENERGY… • … this is due to the strength of the intermolecular attraction between particles • (e.g.) ROOM TEMPERATURE (20o C): some substances are solids, some liquids and others gases

  7. GASES: Kinetic-Molecular Theory of Matter … • have the WEAKEST intermolecular forces • particles are FAR APART moving freely in all directions in a translational (straight line/linear) motion • when particles “COLLIDE” energy is transferred between the particles, but is NOT LOST

  8. GASES: Kinetic-Molecular Theory of Matter

  9. LIQUID: Kinetic-Molecular Theory of Matter … • have STRONGER intermolecular forces than gases • particles are still CLOSE TOGETHER, but are now in partial disorder as they move about • particles are FLUID (able to flow from place to place)

  10. LIQUID: Kinetic-Molecular Theory of Matter

  11. SOLID: Kinetic-Molecular Theory of Matter … • have the STRONGEST intermolecular force between the particles • particles are CLOSE TOGETHER arranged in an ordered pattern • particles have kinetic energy and are ALWAYS VIBRATING

  12. SOLID: Kinetic-Molecular Theory of Matter

  13. Summary: Kinetic-Molecular Theory of Matter

  14. “3” Principle States of Matter: • Solid (definite shape & volume;atoms held tightly together w/ a vibrational motion) • Liquid(definite volume;shape of container;atoms loosely held together,atoms sliding over one another) • Gas (shape & volume of container; atoms NOT held together and moving in ALL directions)

  15. “3” Principle States/Phases of Matter: • Solid • Liquid • Gas

  16. TYPESof SOLIDS: • CRYSTALLINE (true):regular, orderly, repeating, crystalline lattice pattern • ALLOTROPES  same element, same state of matter, different atomic form (e.g.) Carbon [C]: graphite, diamond, nanotubes and buckyballs • AMORPHOUS:long, intertwiningchains or strands of atoms

  17. TYPESSOLIDS: CRYSTALLINE and AMORPHOUS CRYSTALandAMORPHOUS ALLOTROPES

  18. PROPERTIESof LIQUIDS: • ADHESION: a force that attracts particles of different substances to each other • COHESION:a force that attracts particles of the SAME substance to each other • SURFACE TENSION  the attraction of water molecules to each other at the surface • VISCOSITY:the resistance of a liquid to flow

  19. PROPERTIES of LIQUIDS: ADHESION,COHESION&SURFACE TENSION and VISCOSITY ADHESIONandCOHESION VISCOSITY

  20. PROPERTIES of LIQUIDS: ADHESION,COHESION&SURFACE TENSION and VISCOSITY http://apod.nasa.gov/apod/ap130424.html SURFACE TENSION

  21. PROPERTIESof GASES: • EXPANSION: the spreading out of molecules filling a container regardless of its size due to the spacing between gas molecules • COMPRESSION:the compactionof same amount of gas molecules in a smaller containerdue to the spacing between molecules • DIFFUSION: the process where one gas mixes with another [SOLIDS and LIQUIDS can also diffuse] • EFFUSION:the process where gas escapes through a very small holes in a container

  22. PROPERTIES of GASES: DIFFUSION andEFFUSION state the HEAVIER the gas’s molecular MASS, the SLOWER the diffusion (mixing) and effusion (escaping) of the gas molecules

  23. MEASUREABLE PROPERTIES of GASES: • PRESSURE and VOLUME (Boyle’s Law): as VOLUMEincreasesPRESSUREdecreases [when TEMPERATURE remains CONSTANT] • PRESSURE and TEMPERATURE:as TEMPERATUREincreases PRESSUREincreases [when VOLUME remains CONSTANT] • VOLUME and TEMPERATURE (Charles’s Law):as TEMPERATURE increases a “flexible”VOLUMEincreases [when PRESSURE remains CONSTANT]

  24. MEASURABLE PROPERTIES of GASES: PRESSURE andVOLUME (Boyle’s Law) as the VOLUME INCREASESPRESSURE DECREASES when TEMPERATURE is kept CONSTANT

  25. MEASURABLE PROPERTIES of GASES: PRESSURE andTEMPERATUREas the TEMPERATURE INCREASESPRESSURE also INCREASES when VOLUME is kept CONSTANT

  26. MEASURABLE PROPERTIES of GASES: VOLUME andTEMPERATURE (Charles’s Law) as the TEMPERATURE INCREASESVOLUME alsoINCREASES when PRESSURE is kept CONSTANT

  27. “4th” State/Phase of Matter: PLASMA • ionized atoms stripped of their electrons(negatively charged subatomic particles of an atom) leaving positively charged nuclei tightly packed together • the state of matter of the starsand stellar nebulae • makes up 99% of the matter in our universe • also found in the outer-most layer of earth’s atmosphere = ionosphere • ionized gases are found in fluorescentand neonsigns and lightning

  28. “4th” State of Matter: PLASMA

  29. THE END FOR NOW… UNIT 1 (LESSON 5)

  30. COMING SOON “CHANGES of STATE” UNIT 1 (Lesson 6)

  31. THE STORY CONTINUES…

  32. …CHANGING STATES OF MATTER Unit 1 (LESSON 6)

  33. Unit 1 – LESSON 6 “CHANGING STATES of MATTER”

  34. STATE OF MATTER depends on the BALANCE between TEMPERATURE and ENERGY • changing temperature causes a gain or loss in energy • changing the amount of energy causes a change in the motion of the particles • changing motion of the particles changes the distance and attraction of the particles to each other

  35. What DOES CHANGE when changing States of Matter: • the energy of the particles (gainorlose) • the motion of the particles (fast or slow) • the attraction of the particles (more, less or none) • the distanceof the particles (close or farther apart) • without a change in temperature and energy (outside forces) , matter would remain in its current state due to INERTIA

  36. MELTING occurs when: • temperature of a SOLID is raised • the SOLID’S particles gain energy • the particles of the SOLID movefaster • the attraction of the SOLID’S particles weakens • the distanceof the particles become farther apart  turns into a LIQUID

  37. VAPORIZATION occurs when: • temperature of a LIQUID is raised • the LIQUID’S particles gain energy • particles of the LIQUID movefaster • the attraction of the LIQUID’S particles weakens • the distanceof the particles become farther apart  turns into a GAS

  38. FORMS of VAPORIZATION: EVAPORATION = changing of the SURFACE molecules only of a liquid into a GAS BEFOREreaching the boiling point temperature BOILING= changing of ALL the liquid’s molecules throughout the liquid into aGAS AFTERreaching the boiling point temperature

  39. MELTINGandVAPORIZATION:

  40. SUBLIMATION occurs when: • temperature of a SOLID is raised • the SOLID’S particles gain energy • particles of the SOLID movefaster • the attraction of the SOLID’S particles weakens • the distanceof the particles become farther apart  turns DIRECTLY into a GAS

  41. BOILING; MELTINGandSUBLIMATION:

  42. CONDENSATION occurs when: • temperature of a GAS is lowered • the GAS’S particles lose energy • the particles of the GAS moveslower • the attraction of the GAS’S particles strengthens • the distanceof the particles become closer  turns into a LIQUID

  43. FREEZING occurs when: • temperature of LIQUID is lowered • the LIQUID’S particles lose energy • particles of the LIQUID moveslower • the attraction of the LIQUID’S particles strengthens • the distanceof the particles become closer  turns into a SOLID

  44. DEPOSITION occurs when: • temperature of a GAS is lowered • the GAS’S particles lose energy • particles of the GAS moveslower • the attraction of the GAS’S particles strengthens • the distanceof the particles become closer  turns DIRECTLY into a SOLID

  45. CONDENSATIONandFREEZING:

  46. LATENT HEAT: • “hidden heat” providing the energy for the molecules to be “rearranged” without making them move faster, which allows for continued melting/freezing or boiling/condensation without the overall temperature of the substance changing • HEAT of FUSION going from a solid to a liquid and a liquid to a solid • HEAT of VAPORIZATION going from a liquid to a gas and gas to a liquid

  47. LATENT HEAT:

  48. LATENT HEAT(hidden heat of physical changes): • the heat that is absorbed or releasedwhen a substance undergoes a physical phase change but does NOT makethe substance change temperature • the heat of the water in our atmospherethat creates weather patterns and provides the powerful energyof lightningand thunderstorms

  49. Law of Conservation of Energy: • the TOTAL amount of ENERGY ALWAYS STAYS THE SAME regardless of how many times it undergoes a physical or chemical change • ENERGY can change FORM, but it can NEVERbe CREATED or DESTROYED

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