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Properties and States of Matter Chapters 2 and 3
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Classifying Matter Matter Anything that has mass and takes up space Either a pure substance or a mixture end
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Classifying Matter-Pure Substance Pure Substance Matter that always has exactly the same make-up Either an element or a compound Salt, table sugar, water, gold, aluminum end
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Classifying Matter- Pure Substance Element Something that cannot be broken down into simpler things Given a 1 or 2 letter symbol on the Periodic Table (C, N, O, Au, Fe) Carbon, iodine, gold, iron end
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Classifying Matter- Pure Substance Compound Made from 2 or more things and can be broken down into those things 2 or more elements joined in a fixed proportion Water, table salt, sugar end
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Classifying Matter- Mixture Mixtures Contains 2 or more elements with no fixed make-up Heterogeneous Mixtures Can identify different parts of the mixture Does not look the same all the way through Salad dressing, sand/dirt Homogeneous Mixtures Substances cannot be distinguished Looks the same all over Tap water, Fruit Punch, stainless steel end
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Classifying Matter- Mixtures Solutions When something dissolves and forms a homogeneous mixture Salt water, Kool-Aid, Sweet Tea Suspension A heterogeneous mixture that separates into layers over time Salad dressing, paint, liquid medicines “Shake well before using” end
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Physical Properties Physical property Something that can be observed or measured without changing the material 7 physical properties you need to know end
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Physical Properties Viscosity Liquid’s resistance to flowing Honey = high water = low Conductivity Ability to allow heat/electricity to flow Iron = good rubber = bad Malleability Solid’s ability to be hammered without shattering Gold = very glass = not end
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Physical Properties Hardness Ability of something to cut something else Diamond is the hardest substance on Earth Melting Point Temp. where a substance goes from a solid to a liquid Boiling Point Temp. where a substance gores form a liquid to a gas end
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Physical Properties Density (D) A substances’ mass divided by its volume Measured in either g/mL or g/cm 3 Remember: 1 mL = 1 cm 3 !!! Things that are more dense will sink, Things that are less dense will float Density (g/mL or g/cm 3 ) mass (g) Volume (mL or cm 3 ) end
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Physical Properties A rock has a mass of 12 g. If it has a volume of 50 mL, what is the rock’s density? A block has a density of 0.005 g/cm 3. If the block has a volume of 56 mL, what is the block’s mass? A graduated cylinder has 13.4 mL of water. When a marble, with a density of 6.2 g/mL, is dropped in the cylinder the water level rises to 34 mL. What is the marble’s mass? end
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Using Physical Properties Physical properties are used for: Identifying a material Choosing a material for a specific purpose To separate the substances in a mixture end
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Separating Mixtures Filtration Separates materials based on the size of their particles Using a coffee filter Distillation Separates things in solution based on boiling points Making moonshine end
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Chemical Properties Chemical property A property that produces a change in something’s composition Something is changing into something else end
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Chemical Properties Flammability Ability to burn in the presence of oxygen Different elements burn different colors Think fireworks!!! Reactivity How quickly something combines with other things end
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Physical vs. Chemical Changes Physical Change Some properties of a substance change, but the substance is still the same Shredding paper, breaking glass, ice cube melting end
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Physical vs. Chemical Changes Chemical Change When a substance reacts and forms one or more new substances The composition of the matter changes end
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Physical vs. Chemical Changes Evidence of a chemical change: Change in color Copper roof -> green Production of a gas See bubbles forming Formation of a precipitate Forms a solid Temperature change Production of light end
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States of Matter There are 5 states of matter (phases of matter) We only care about 3 of them Solid Liquid Gas end
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States of Matter- Solids Solid Something with a fixed shape and a fixed volume Particles are very close together and vibrate end
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States of Matter- Liquid Liquid Something with no fixed shape but a fixed volume Particles are free to move around Also called a fluid end
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States of Matter- Gas Gas Something with no fixed shape and no fixed volume Particles spread apart to fill the space available end
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States of Matter- Other Plasma Exists at high temperatures and high pressure Stars Bose-Einstein Condensate (BEC) Exists near absolute zero at very low pressures Solid acts as a single particle end
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Behavior of Matter Kinetic Theory of Matter All particles of matter are in constant motion The state of matter depends on the amount of motion Originally developed to describe gases Kinetic Energy The energy an object has due to motion More Speed = More Kinetic Energy end
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Behavior of Matter- Gases Particles move so fast that they are not attracted to each other Particles move in a straight line until they hit something Act like billiard balls end
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Behavior of Matter- Gases Kinetic Theory of Gases The motion of a gas allows it to fill a container of any shape or size 3 main points Particles in a gas are in constant, random motion The motion of 1 particle is not affected by the motion of other particles, unless the particles hit each other Forces of attraction between particles are ignored end
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Behavior of Matter- Liquids Particles move slower than gases Each particle is attracted to the others Fight between a particle’s constant motion and the attraction to the other particles end
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Behavior of Matter- Solids Particles are extremely attracted to each other They move very little Vibrate back and forth in the same spot end
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Changes of State (Phase Changes) Phase Change A reversible physical change A substance goes from 1 state of matter to another 6 common phase changes Melting and Freezing Vaporization and Condensation Sublimation and Deposition end
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Changes of State (Phase Changes) Gas Solid Liquid Sublimation Deposition Melting Freezing Vaporization Condensation end
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Changes of State- Energy When you heat something up you give it energy And the temperature goes up UNTIL it changes to another state! When something goes through a phase change, the temperature stays the same. The heat you add is breaking the attraction between particles and pushing them away from each other end
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Changes of State- Energy Solid- Temperature is going up Melting- Temperature is staying the same Liquid- Temperature is going up
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Changes of State- Energy Temperature is not changing during melting, but heat is added Temperature is not changing during boiling, but heat is added
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Changes of State- Energy If you have to add energy, the phase change was endothermic Melting, Vaporization, Sublimation If you have to take away energy, the phase change was exothermic Freezing, Condensation, Deposition end
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Changes of State- Melting and Freezing Melting Some molecules in a solid, gain energy to overcome attractive forces to become a liquid Freezing Some molecules in a liquid, start to slow down and become attracted to each other as a solid end
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Changes of State- Vaporization and Condensation Vaporization Some molecules in a liquid, gain energy to overcome attractive forces to become a gas Heat of Vaporization The amount of energy needed to move from a liquid to a gas Evaporation Changing a liquid to a gas at temperatures below the boiling point Spilled water “disappears” after a few hours end
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Changes of State- Vaporization and Condensation Condensation Some molecules in a gas, start to slow down and become attracted to each other as a liquid The outside of your cold drink, on a hot day end
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Changes of State- Sublimation and Deposition Sublimation Some molecules in a solid, gain energy to overcome attractive forces to go to a gas Dry Ice (carbon dioxide) Deposition Some molecules in a gas, start to slow down and become attracted to each other as a solid Frost on cold windows end
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