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Solids, Liquids and Gases

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Presentation on theme: "Solids, Liquids and Gases"— Presentation transcript:

1 Solids, Liquids and Gases
Chapter 16

2 Section 1 – Kinetic Theory
States of matter you saw at lunch? Kinetic Theory – explanation of how particles in matter behave All matter is composed of small particles (atoms, molecules, ions)

3 Kinetic Theory Particles in constant, random motion Particles are colliding Energy that particles lose from collisions is negligible

4 Average Kinetic Energy
Temperature is measure of average kinetic energy. Warmer – particles have MORE energy  Move faster Cooler – particles have LESS energy  Move slower

5 Solid State – H2O Particles in fixed position

6 Liquid State Particles in solid gain energy and move faster  break out of fixed position Melting point: temperature where solid begins to liquefy Heat of fusion: amount of energy needed to change a solid to liquid

7 Liquids Flow Particles have energy to break SOME attraction and flow

8 Gas State Particles have energy to escape ALL attraction

9 Vaporization Liquid particles gain enough energy to escape to gas phase Evaporation: vaporization at the surface of liquid, spontaneously Boiling point: applying heat, temperature at which pressure of vapor is equal to external pressure, liquid to gas Heat of vaporization: amount of energy needed for liquid to be a gas

10 Gases fill their Container
Diffusion: spreading of particles throughout until they are mixed

11 Heating Curve of a Liquid

12 Heating Curve of a Liquid
a and c – increasing in energy b and d – energy used to break attraction between particles

13 Plasma Def: consists of positive and negative particles
Very HIGH temperature Particles moving so fast  e- are stripped off Lightning, sun, neon lights

14 Thermal Expansion

15 Thermal Expansion Spaces are expansion joints Prevent cracks
Absorbs heat – expands Cools – shrinks

16 Expansion of Matter Thermal Expansion: increase in the size of a substance when the temperature is increased Warmer = less attraction b/ particles = move freer Cooler = more attraction = closer together

17 Expansion of Matter

18 Expansion of Matter

19 Strange Water Ice is less dense than liquid water
(+) and (-) ends arrange themselves next to each other Create empty spaces

20 Strange Water

21 Solid or Liquid? Amorphous Solids: “without” form, change to liquid over range of temperatures Ex: glass, plastic Liquid turned to solid too quickly

22 Solid or Liquid Liquid crystals: change to liquid but don’t lose their ordered form Ex: liquid crystal display (LCD)  calculators, etc.

23 Properties of Fluids Section 2

24 How do ships float? Buoyancy: ability of fluid to exert upward force on object. If force equal to weight = float

25 Archimedes’ Principle
Def: buoyant force on an object is equal to the weight of the fluid displaced by the object

26 Density Same size blocks - wood and steel
Displace same amount of water BUT, wood block floats and steel block sinks Different densities – object has less density than density of fluid to float

27 Archimedes’ Principle

28 Pascal’s Principle Pressure: force exerted per unit area
Pressure applied to fluid is exerted throughout the fluid Used in hydraulic lifts – use your weight to lift something much heavier

29 Bernoulli’s Principle
Def: as velocity of fluid increases  pressure of fluid decreases

30 Fluid Flow Viscosity: the resistance of a fluid to flow
Syrup – high viscosity Water – low viscosity

31 Behavior of Gases Section 3

32 Pressure Result of gas particle collisions with the container
More collisions = More pressure Pressure unit = Pascal (Pa) How do we get high pressure?

33 Boyle’s Law Relationship between pressure and volume
 volume, size of container, what will pressure do? Pressure  Inversely related: as one goes  the other goes  , or vice versa

34 Charles’s Law Relationship between volume and temperature
“Keep away from heat” on pressurized can  temperature what will volume do?  volume Directly related: as one goes  the other goes , or vice versa

35 Kelvin Scale All (+) numbers
0K = absolute zero – all particle motion stops 0K = -273oC K = oC + 273


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