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Matter

Learn about the diverse properties of matter, its physical and chemical aspects, different states like solid, liquid, gas, and plasma, the kinetic theory, pressure, laws like Boyle's and Charles's, how temperature affects matter, changes in states, and energy interactions.

jeanineyoung
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Matter

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  1. Matter Anything that has mass and takes up space (volume)

  2. MATTER FACT Water can be found naturally on earth as a solid, liquid, and a gas. MATTER is anything that has mass and takes up space can be can be can be freezes to condenses to solid liquid gas melts to evaporates to

  3. Properties of Matter Physical Property • Any property of matter that can be observed or measured without changing the identity of the matter • Examples color shape taste density state/phase D = M V

  4. Properties of Matter Chemical Property • Any property of matter that describes a substance based on its ability to change into a new substance • Examples flammability reactivity with vinegar reactivity with oxygen Iron + Oxygen  Iron oxide (rust) 2Fe + 3O2  Fe2O3

  5. 5 Physical States of Matter • Bose-Einstein • Solid • Liquid • Gas • Plasma (Newest State)

  6. Kinetic Theory • All particles of matter are in constant motion

  7. Temperature • a measure of the average kinetic energy of the particles of matter

  8. Exist at extremely cold temperatures (around absolute zero or -460 oF) Particles are super unexcited Particles lock or “clump” together so firmly that they move as a single unit Definite shape and volume (?) Bose-Einstein Condensate

  9. Particles are tightly compact Particles vibrate without the ability to move freely Definite shape and volume Solid Animation Solid

  10. Particles are tightly compact, but able to move around close to each other No definite shape, but definite volume Liquid Animation Liquid

  11. Particles can easily spread out or move close together Particle move freely and with a lot of energy No definite shape or volume Gas Simulation Gas

  12. Exist at extremely high temperatures (several million degrees Celsius) Particles are broken apart Particles move freely and with extremely high energy This form is not too common on earth, however it is the most common form of matter in the universe No definite shape or volume? Examples: Florescent and neon lights, lightning, aurora borealis Plasma Why do you think this is the most common form/state of matter in the universe?

  13. Pressure • Force distributed over an area • Caused by: Collisions between particles of a gas and the walls of the container • How does the frequency of collisions affect the pressure of the gas?

  14. Pressure Units

  15. Factors that affect pressure: • Temperature – increase temperature = increase in pressure • Volume – reduce volume = increase in pressure • Number of particles – increase number of particles = increase in pressure

  16. Atmospheric Pressure • The gas molecules closest to Earth’s surface are packed together very closely. • This means pressure is lower the higher up you go into the atmosphere.

  17. Atmospheric Pressure

  18. Describe what is happening using what we just learned.

  19. Charles’s Law

  20. Charles’s Law • A hot-air balloon floats because the air inside is less dense than the air outside. • Volume decreases with decreasing temperature. • The volume of a gas increases with increasing temperature.

  21. Boyle’s Law

  22. Boyle’s Law • When you squeeze a fixed quantity of gas into a smaller volume the pressure goes up. • Volume is inversely proportional to pressure

  23. Combined Gas Law • Relates temperature, volume and pressure

  24. Practice Problem 1: • A kit used to fix flat tires consists of an aerosol can containing compressed air and a patch to seal the hole in the tire. Suppose 5 liters of air at atmospheric pressure (1 atm) is compressed into a 0.5 liter aerosol can. What is the pressure of the compressed air in the can? Assume no change in temperature or mass.

  25. Practice Problem 2: • Gas stored in a tank at 273 K has a pressure of 388 kPa. The safe limit for the pressure is 825 kPa. At what temperature will the gas reach this pressure?

  26. Changes in States(Physical Changes) Plasma Deposition Vaporization (Evaporation/Boiling) Gas Liquid Condensation Melting Solid Freezing Sublimation Bose-Einstein All changes in state require a change in energy

  27. States of Matter Continuum

  28. Energy and the States of Matter • The physical states of matter result from the amount of energy the particles composing the matter have. Basically, more energy means more movement for the particles and less energy means less movement. • Energy/Temperature and Matter If you were to compare an ice cube and the steam created from boiling water, which would you think has more energy?

  29. States of Matter Simulation Simulation 1 Simulation 2 This is what happens when energy is added and taken away

  30. Endothermic Reactions • Absorbs energyfrom surroundings

  31. Endothermic Reactions • Energy must be absorbed as the products form. • The container in which an endothermic reaction is taking place will feel cold .

  32. Exothermic Reactions • Releaseenergy to its surroundings • Energy must be released as the products form. The container in which an exothermic reaction is taking place will feel hot.

  33. Endothermic or Exothermic?

  34. Endothermic or exothermic?

  35. Heat of Fusion • Heat of Fusion: Amount of energy absorbed • Measured in joules (J) • One gram of ice absorbs 334 joules as it melts

  36. Joules • A joule is the energy used by one watt going for 1 second. The penlight is about 1 watt. So turn it on for one second and you consume one joule of energy. So one joule isn't much, but 90,000,000,000,000,000 (90 quadrillion) joules is.

  37. Heat of Vaporization • The amount of energy a substance must absorb to change from a liquid to a gas

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