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Chapter 3-1 Matter and Energy
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Kinetic Theory Kinetic theory - an explanation of how particles in matter behave. 3 requirements
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Kinetic Theory All matter is composed of small particles (atoms, molecules, and ions).
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Kinetic Theory Particles are in constant, random motion.
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Kinetic Theory Particles are colliding with each other and the walls of their container.
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Solids Definite shape and volume
Crystalline – orderly arrangement of atoms Amorphous – atoms in no particular pattern
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Crystalline Solid
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Amorphous Solid
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Liquids Change shape but not volume
Surface tension – force acting on the surface of a liquid
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Surface Tension
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Thermal Energy Atoms in solids – tightly packed together
Thermal energy in the particles causes them to vibrate in place
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Gas Particles are free to move in all directions
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Plasma Plasma – state of matter that starts as a gas and then becomes ionized 99% of know matter in universe Electrons stripped off
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Plasma Stars Lightning Fire Fluorescent Lights
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Energy Energy – the capacity to do work
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Thermal Energy Thermal Energy – Kinetic energy of a substance’s atoms
Kinetic energy – energy of motion
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Average Kinetic Energy
Temperature - average kinetic energy of particles in the substance How fast the particles are moving.
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Average Kinetic Energy
On average, molecules of frozen water at 0°C will move slower.
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Average Kinetic Energy
On average, molecules of water at 90°C will move faster.
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Change of state Endothermic change Exothermic change Requires energy
Melting Sweating Exothermic change Energy released from change Freezing
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Evaporation vs Boiling
Boiling - occurs throughout a liquid Evaporation - occurs at the surface of a liquid
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Sublimation Sublimation – process where a solid turns directly to a gas Ex. old ice cubes or dry ice
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Condensation Condensation – change of a substance from a gas to a liquid Gas comes in contact with a cool surface
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Conservation of Mass and Energy
Mass can not be created or destroyed Amount mass and energy stays the same before and after the change
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States of Matter Clip
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