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Understanding the Four States of Matter

Learn about the four states of matter - solid, liquid, gas, and plasma - and how they are formed based on particle arrangement, energy, and distance. Explore phase changes and the concept of plasma as the common state of matter.

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Understanding the Four States of Matter

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  1. STATES OF MATTER

  2. STATES OF MATTER • The Four States of Matter • Four States • Solid • Liquid • Gas • Plasma

  3. STATES OF MATTER • Based upon particle arrangement • Based upon energy of particles • Based upon distance between particles

  4. Kinetic Theory of Matter • Matter is made up of particles which are in continual random motion.

  5. STATES OF MATTERSOLIDS • Particles of solids are tightly packed, vibrating about a fixed position. • Solids have a defiite shape and a definite volume. Heat

  6. STATES OF MATTERLIQUID • Particles of liquids are tightly packed, but are far enough apart to slide over one another. • Liquids have an indefinite shape and a definite volume. Heat

  7. STATES OF MATTERGAS • Particles of gases are very far apart and move freely. • Gases have an indefinite shape and an indefinite volume. Heat

  8. F. Phase Changes – Physical Liquid -> Gas Gas -> Liquid Solid -> Liquid Liquid -> Solid Solid -> Gas • Evaporation = • Condensation = • Melting = • Freezing = • Sublimation =

  9. PHASE CHANGES

  10. PHASE CHANGES

  11. But what happens if you raise the temperature to super-high levels…between 1000°C and 1,000,000,000°C ? Will everything just be a gas?

  12. STATES OF MATTERPLASMA • A plasma is an ionized gas. • A plasma is a very good conductor of electricity and is affected by magnetic fields. • Plasmas, like gases have an indefinite shape and an indefinite volume. • Plasma is the • common state • of matter

  13. STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

  14. Some places where plasmas are found… 1.Flames

  15. 2. Lightning

  16. 3. Aurora (Northern Lights)

  17. The Sun is an example of a star in its plasma state

  18. G. Chemical Changes • Signs of a Chemical Change • change in color or odor • formation of a gas • formation of a precipitate (solid) • change in light or heat

  19. H. Physical vs. Chemical Changes chemical physical chemical physical physical • Examples: • rusting iron • dissolving in water • burning a log • melting ice • grinding spices

  20. Learning Check S1 • Match: (1) solid, (2) liquid, or (3) gas. • ____ A. Has a definite volume, but shape • of the container. • ____ B. Its particles are moving rapidly. • ____ C. Fills the volume of a container. • ____ D. Particles are in a fixed structure. • ____ E. Particles are close together, but mobile.

  21. Heat Calculation for Fusion • Heat = g water x 80. cal • g water • = g water x 334 J • g water • How much heat in calories is needed to melt 15.0 g of water? • 15.0 g water x 80. cal = 1200 cal • 1 g water

  22. Learning Check CS2 A. Why does the temperature of ice stay at 0°C while the ice melts? • B. How much heat in joules is needed to melt 1.00 g of ice of 0°C? • 1) 1.00 J 2) 100 J 3) 334 J • C. How many joules of heat are released when 100.0 g of water at 0°C freezes (0°C)? • 1) 3.34 J 2) 3340 J 3) 33,400 J

  23. Solution CS2 A. Why does the temperature of ice stay at 0°C while the ice melts? Energy goes into the change of state. • B. How much heat in joules is needed to melt 1.00 g of ice of 0°C? • 3) 334 J • C. How many joules of heat are released when 100.0 g of water at 0°C freezes (0°C)? • 3) 33,400 J

  24. Heat of Vaporization • Amount of heat needed to change 1 gram of liquid to gas at its boiling point • Boiling (Condensing) Point of Water = 100°C • Heat of Vaporization (water) = 2260 J/g

  25. Learning Check CS4 • A. Ice cubes in a warm drink will • 1) melt 2) freeze 3) not change • B. The liquid drink _________ energy. • 1) loses 2) gains 3) does not change • C. The ice ___________energy. • 1) loses 2) gains 3) does not change • D. The final temperature of the ice and liquid is • 1) the same 2) different

  26. Solution CS4 • A. Ice cubes in a warm drink will 1) melt • B. The liquid drink 1) losesenergy. • C. The ice 2) gains energy. • D. The final temperature of the ice and liquid is 1) the same

  27. I. Law of Conservation of Mass Review from balancing CR ch. 11 • Although chemical changes occur, mass is neither created nor destroyed in a chemical reaction • Mass of reactants equals mass of products massreactants = massproductsts A + B C

  28. I. Conservation of Mass • In an experiment, 10.00 g of red mercury (II) oxide powder is placed in an open flask and heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What is the mass of the oxygen formed in the reaction? GIVEN: Mercury (II) oxide  mercury + oxygen Mmercury(II) oxide = 10.00 g Mmercury = 9.86 g Moxygen = ? WORK: 10.00 g = 9.86 g + moxygen Moxygen = (10.00 g – 9.86 g) Moxygen = 0.14 g Mercury (II) oxide  mercury + oxygen Mmercury(II) oxide = 10.00 g Mmercury = 9.26 Moxygen = ? massreactants = massproducts

  29. PURE SUBSTANCE MIXTURE yes no yes no Is the composition uniform? Can it be chemically decomposed? A. Matter Flowchart MATTER yes no Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

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