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Published byTeresa Carter Modified over 9 years ago
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What is Matter? Anything that takes up space (volume) and has mass. Anything on EARTH.
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Types of Matter Homogeneous Matter that is made up of the same or alike particles. SAME THROUGHOUT Can’t see the particle Heterogeneous Matter that is made up of different types of particles. DIFFERENT THROUGHOUT Can see the particles
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Homogeneous Materials Kool aid Tea Clear sodas Rubbing alcohol Water Elements Compounds Acids
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Heterogeneous Materials Cereal Salad Snack mix Kabobs Italian dressings Uncooked pizza M & M’s Skittles Vegetable soup Milk
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Now it is your turn… you tell me: Homogeneous or Heterogeneous Flat soda pop Cherry vanilla ice cream Sugar (C 2 H 3 O 2 ) Salt (NaCl) City Air Iron (Fe) Beach Sand Spaghetti Sauce
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Mixtures vs. Pure Substances MIXTURES Heterogeneous or Homogeneous Easily separated EXAMPLES Any Heterogeneous or homogeneous examples PURE SUBSTANCES Homogeneous Hard to separate In it simplest form EXAMPLES Elements and compounds
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Types of Pure Substances Elements: Purest substance known that can’t be broken down Neon: Ne Compounds: 2 or more elements chemically combined Water: H 2 O
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Atoms are the counting units or quantity of the element.
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Properties of Mixtures Easily separated Physically combined to easily separate. Amounts vary when mixed Changes only in physical appearance when dissolved.
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Types of Mixtures Heterogeneous Mixtures Suspensions Colloids Homogeneous Mixtures Solutions
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Solution Homogeneous Mixture: Same throughout Examples: Ice tea Sugar water Kool aid Sprite
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Solutions and Its Properties Particles are individual atoms, molecules, or ions (charged particles) Clear Can’t be filtered Particles are evenly spread out Can’t see the particles Homogeneous
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Parts of a Solution Solute – Part being dissolved in the solvent. ex: Sugar, Hot Chocolate, Salt Solvent – Part that does the dissolving. ex: Water – universal solvent
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Aqueous vs. Tincture Solution Aqueous – water is the solvent Tincture – alcohol is the solvent
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Combinations of Solutions SOLUTES 1. Solid 2. Solid 3. Solid SOLVENT Solid Liquid Gas EXAMPLES Alloy (pots) Sea water Soot in air 4. Liquid 5. Liquid 6. Liquid Solid Liquid gas Dental fillings Antifreeze Humid air 7. Gas 8. Gas 9. Gas Solid Liquid Gas Gas mask Sodas Air
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Special Activities of Solutions Dissociation – splitting ions to form charges Ionization – gaining or losing electrons to form ions Electrolyte – Solution that produce electricity (Salt and Water) Non-electrolyte – solution that does not produce electricity (Sugar and Water)
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Special Solutions Miscible – when a liquid is dissolved into a liquid Example: Antifreeze, alcohol and water Alloy – when a solid is dissolved into a solid Examples: Stainless steel pots and pans, bronze, brass, jewelry
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Rates of Solutions (how to speed up a solution) Stirring Heating Powdering- increasing the surface area
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Solubility and Its Factors Solubility – ability of a solute to dissolve into a solvent. Factors that affect solubility of a gas in a solution Temperature – decreasing temperature Pressure – increasing pressure
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Dilute vs. Concentrated Dilute – weak solution “watered down” Concentrated Strong solution
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Levels of Solutions Saturated – Holding as much solute at a given temperature Supersaturated – UNSTABLE – more solute in the solvent at a high temp.
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Colloid Properties Heterogeneous Mixture Can’t see particles Particle size is larger than those in solutions Scatters light – Tyndall Effect
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Examples of Colloids Fog- clouds Smoke- smoke Foam- whipped cream Emulsion- mayonnaise Sol- paints Gel- butter
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Suspension Properties Heterogeneous Mixture Can see the particles Easily separated EXAMPLES waste oil and water trail mix eggs cereals
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Ways to Separate Mixtures Filtering – Suspensions Evaporation – Solution, Colloids, Suspensions Distillation – Solutions, Colloids, Suspensions Chromatography - Solutions
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Physical Properties and Changes Physical Properties Characteristic you can observe without changing the substance Examples: ○ Appearance: color, shape, … ○ Measurements: mass, length, volume… ○ Behavior: attracted by magnet, soluble… ○ Changes of State: melting point, boiling point… Physical Changes Change made to material that does not change the substances Usually, the change can be reversed Examples: ○ Tearing, shredding crushing… ○ Boiling, melting, freezing… ○ Dissolving
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Chemical Properties Characteristic of a substance that undergoes a certain chemical change Examples: ○ Flammability or combustibility ○ Reactivity
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Chemical Change Change of one substance in a material to a different substance Usually the change can’t be reversed Signs of a chemical change: Smell Color Foaming or gas production Precipitate – solid forming when two items are mixed together Light or explosion (release of energy) Examples: rusting, burning, …
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Law of Conservation of Mass Matter is neither created nor destroyed during a chemical change or physical change original mass = final mass
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