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The Characteristics of
Matter
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States of Matter
• Solid:
• Liquid:
• Gas:
• Plasma:
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States of Matter
• Solid: definite volume & shape, hard to compress, dense
• Liquid:
• Gas:
• Plasma:
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States of Matter
• Solid: definite volume & shape, hard to compress, dense
• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense
• Gas:
• Plasma:
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States of Matter
• Solid: definite volume & shape, hard to compress, dense
• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense
• Gas: indefinite volume, fills container, easy to compress, not dense
• Plasma:
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States of Matter
• Solid: definite volume & shape, hard to compress, dense
• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense
• Gas: indefinite volume, fills container, easy to compress, not dense
• Plasma: like gas but ionized (with + or – charge)
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Phase Changes (Changes of State) • Solid liquid: • Liquid solid:• Liquid gas: • Gas liquid:• Solid gas: • Gas solid: • Gas plasma: • Plasma gas:
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Phase Changes (Changes of State) • Solid liquid: melting• Liquid solid: freezing (solidification)• Liquid gas: boiling (evaporation) • Gas liquid: condensation • Solid gas: sublimation• Gas solid: deposition • Gas plasma: ionization• Plasma gas: recombination
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Phase Changes (Changes of State)
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Phase Changes in Water
• Boiling point of water =
• Melting point of water =
• Freezing point of water =
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Phase Changes in Water
• Boiling point of water = 373.15K
• Melting point of water = 273.15K
• Freezing point of water = 273.15K
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Phase Changes in Water
• Boiling point of water = 373.15K
• Melting point of water = 273.15K
• Freezing point of water = 273.15K
• Notice that these are the same? They are interchangeable
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The Kinetic Molecular Theory• Particles are always moving
• The more energy they have, the faster they move
• Heat is the measure of total kinetic energy
• Temperature is the average kinetic energy of all the molecules
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The Kinetic Molecular Theory• Solid particles: closely packed (dense), low energy
and little space to move so they vibrate in place
• Liquids particles: more space and more energetic so they can flow (slide past each other)
• Gas particles: lots of space, most energetic and move freely within a container
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Physical and Chemical Changes in
Matter
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Physical Properties vs. Chemical Properties
• Properties that can be found without a chemical reaction (without creating a new substance)
• E.g. density, colour, hardness, malleability, ductility, lustre, viscosity, melting point, boiling point
• Describe the ability of a substance to undergo chemical reactions and change into new substances
• E.g. H2 can burn in air to produce H2O; H2 combines with Cl2 to form HCl
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Physical Change
• Change in the shape or state of a substance
• No new substances formed (same chemicals)
• Reactants are the same as products
• Generally possible and easy to reverse
• E.g. changes in state (liquid water ice), changes in shape or volume
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Physical Change
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Chemical Change
• A change where new substances are formed
• Reactants are different from the products
• Difficult or impossible to reverse
• Often include changes in physical properties
• E.g. cooking an egg, burning a match
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Chemical Change
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Homework
• Read Hebden p.44-52• HW check on p.44 #13 and p.52 #33, 35-41, 44