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Label each picture as the correct state of matter.
A B C
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3.1: Solids, Liquids and
Gases
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What are the three common states of matter and how do they differ?
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• Three states of matter are:1. Solid2. Liquid3. Gas
• Classified based on whether their shapes and volumes are definite or variable.
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• What do these four objects have in common?– Pencil, cell phone, book, and a quarter
• They all have a recognizable shape and they all take up a certain amount of space.
• They are classified as SOLIDS.– state of matter in which materials have a definite
shape and a definite volume.
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Solids• State of matter in which materials
have a definite shape and a definite volume.• Almost all solids have some type
of orderly arrangement of particles at the atomic level.
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Liquids• State of matter in which a
material has a definite volume but not a definite shape.
• liquid always has the same shape as its container and can be poured from one container to another.
• Atoms arranged close together but more random than those in a solid.
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Gases• State of matter in which a
material has neither a definite shape nor a definite volume. • Takes the shape and volume of
its container.• Random arrangement of atoms• Example: Air-mixture of gases
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Gases• Helium filled balloons, a
colorless gas that is less dense than air. The “shape” of the helium in a balloon is the same as the shape of the balloon itself. The volume of the helium in a balloon is equal to the volume of the balloon.
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Plasma• State of matter in which atoms have
been stripped of their electrons• Found in stars, solar wind, lightning
and other EXTREMELY hot places.
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Phase Changes• Occurs when a substance changes from one state of
matter to another• Six common phase changes:– Melting– Freezing– Vaporization– Condensation– Sublimation– Deposition
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What change is taking place?• Melting = solid to liquid *• Freezing = liquid to solid• Vaporization= liquid to gas *• Condensation = gas to liquid• Sublimation = solid to gas *• Deposition = gas changes to solid
without changing to liquid first
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Phase Change Flow Chart
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Endothermic vs. Exothermic
• Endothermic-absorbs energy in the form of heat– Melting– Vaporization– Sublimation
• Exothermic-releases energy in the form of heat– Freezing– Condensation– Deposition
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Temperature and Energy• All phase changes share characteristics
related to energy and temperature.• The temperature of the substance does
not change during a phase change.• Energy is either absorbed (endothermic)
or released (exothermic) during the phase change.
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Phase Change Diagram
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Endothermic Processes• Heat of Fusion = the
energy a substance must absorb in order to change from SOLID to LIQUID– “Fusion” is another term
for melting– Varies depending on
substance– Ex: I g of ice absorbs 334
J of energy as it melts
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Endothermic Processes
• Heat of Vaporization = the energy a substance must absorb in order to change from LIQUID to GAS– Varies depending on
substance– Ex: I g of water absorbs
2258 J of energy when it vapors at 100 ° C.
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Kinetic Theory• Word kinetic comes from the Greek word
meaning “to move”• Kinetic Theory of Matter says that all
particles of matter are in constant motion.– Gas-particles in CONSTANT, RANDOM motion– Liquid-particles “flow” to new locations– Solid-particles vibrate around a fixed location
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Thermal Expansion • Occurs when particles of matter move
farther apart as the temperature increases– Gases expand more than liquids– Liquids expand more than solids
• Thermal expansion is used in glass thermometers– As the temperature increases, the alcohol in the
tube expands and its height increases so you can read the temperature.