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MATTER UNIT

MATTER UNIT. Physical Science. What is Matter. Anything that takes up space (volume) and has mass 2 Types 2 Classifications 4 States. Types of Matter. HOMOGENEOUS Matter that is made up of the same or alike particles Can’t see what makes it up Looks uniform. HETEROGENEOUS

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MATTER UNIT

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  1. MATTER UNIT Physical Science

  2. What is Matter • Anything that takes up space (volume) and has mass • 2 Types • 2 Classifications • 4 States

  3. Types of Matter • HOMOGENEOUS • Matter that is made up of the same or alike particles • Can’t see what makes it up • Looks uniform • HETEROGENEOUS • Matter that is made up of different types of particles • Can see what makes it up

  4. Examples of Homogeneous Materials • Kool Aid • Tea • Rubbing Alcohol • Water (H20) • Element (Ne, H, S) • Compounds (NaCl, KF)

  5. Example of Heterogeneous Materials • Cereal • Salad • Snake Mix • Skittles • Kabobs • Italian Dressing • M~n~M • Milk

  6. Is it Homogeneous or Heterogeneous? • Soda Pop (flat) • Cherry Vanilla Ice Cream • Soda Pop (carbonated) • Sugar (C2H3O2) • Salt (NaCl) • City Air • Iron (Fe) • Beach Sand

  7. Classification of Matter • Mixture • A material made up of two or more substances that can be easily separated • Either Heterogeneous or Homogeneous • Ex: Salsa, Cake batter, pizza, soda • Pure Substance • Classification of matter with a fixed composition • Only Homogeneous • Either Element or Compound • Ex: Neon, Gold, Water, Alcohol

  8. Types of Pure Substance • ELEMENT • Is a substance that cannot be broken into simpler substance • Ex: Neon, Gold, Helium • Compound • Is a substance with 2 or more elements chemically combine • Ex: Water (H20) • Salt (NaCl) • Sugar (C2H3O2)

  9. END DAY ONE

  10. Types of Mixture • Based on the size of its largest particle a mixture can be classified as: • Suspension heterogeneous • Colloids heterogeneous • Solutions homogeneous

  11. Suspension Mixture • Mixture that separates into layers over time • Heterogeneous Mixture • Large particles • Will scatter light • Ex: oil & water, muddy water

  12. Colloid Mixture • A mixture with intermediate size particles • Will NOT settle out • Heterogeneous • Experiences THE TYNDALL EFFECT • Ex: Milk, Paint, fog, smoke, foam, butter, mayo

  13. The Tyndall Effect • Light scatters by particles in colloids • Created by John Tyndall

  14. Solution Mixture • Where one substance dissolve in another • Homogeneous materials • Will NOT settle out • Will NOT scatter light • Ex: salt water, sugar water, kool aid, sprite

  15. Ways to Separate Mixture • Filtering Suspensions only • Evaporation all three types • Distillation • Separate mixtures based on their boiling point • All three types • Chromatography Solutions only

  16. END DAY TWO

  17. Parts of a Solution • SOLUTE • Part being dissolving • Ex: sugar, salt • SOLVENT • Part doing the dissolving • Water is the universal solvent • Ex: water, alcohol

  18. Solubility • Ability of a solute to dissolve in a solvent • Determined by attraction between solute and solvent

  19. Factors Affecting Solubility • Polarity • Substances are polar (have north & south) or nonpolar • Likes will dissolve likes • Temperature • Increase solvent temperature increase solubility

  20. 3 Level of Solution • Saturated • Contains as much solute as the solvent at a given temperature • Unsaturated • Holding little solute in much solvent • Supersaturated • Containing more solute than it normally hold at a given temperature

  21. Electricity & Solutions • Electrolyte • Solution that can conduct electricity • Ex: Salt and Water • Nonelectrolyte • Solution that cannot conduct electricity • Ex: Sugar and Water

  22. Concentrated vs. Diluted • Concentrated • Strong solutions • Diluted • Weak solutions • “Watered Down”

  23. Solubility Curve • Shows how temperatures affect solubility of solutes

  24. Solubility Curve

  25. Using the Solubility Curve • What compounds shows a decrease in solubility from 0ºC to 100ºC? • Which salt is most soluble at 10ºC? • Which salt is least soluble at 20ºC? • Which salt show the least change in solubility from 0ºC to 100ºC? • How many grams of potassium chloride (KCl) can be dissolved at 80ºC? • At 50ºC, how much potassium chlorate (KClO3) can be dissolved in 300 grams of water? • At 30ºC, 90 grams of sodium nitrate (NaNO3) is dissolved in 100 g of water. Is this solution saturated, unsaturated or supersaturated?

  26. END DAY THREE

  27. Physical Property • Any characteristic of a material that can be observed or measured without changing the composition • EX: • Viscosity: liquids resistance to flow (oil, syrup, honey) • Appearance • Hardness • Conductivity • Malleability • Melting Point • Boiling Point

  28. Physical Change • Change made to material that does not change the composition of the substance. • Ex: • Boiling • Melting • Dissolving • Shredding

  29. Chemical Property • A characteristic of a substance that will undergo a certain chemical change • Ex: • Flammability materials that can burn • Combustibility materials that can explode • Reactivity how readily substances will chemically combine with another

  30. Chemical Change • Change of one substance into a NEW & DIFFERENT substance • Signs of Chemical Change • Color Change • Production of Gas Fizzing/Bubbling • Formation of Precipitate insoluble solid • Release of Energy light or Explosion

  31. Law of Conservation of Matter • Matter is not created nor destroyed but changed • Start = Finish

  32. SOLID • Definite Shape • Definite Volume 4 States of Matter • LIQUID • Indefinite Shape • Definite Volume • GAS • Indefinite Shape • Indefinite Volume • PLASMA • Matter made of positively and negatively charged particles • Most of universe

  33. END DAY FOUR

  34. Phase Change • The reversible change that occurs when a substance changes from one state of matter to another

  35. What are the Phase Change? • Melting • Solid to Liquid • Freezing • Liquid to Solid • Vaporization • Liquid to Gas • Condensation • Gas to Liquid • Deposition • Gas to Solid • Sublimation • Solid to Gas

  36. Temperature & Phase Change • As a phase change occurs, temperature remains the same

  37. Phase Change Diagram • Solid State • Phase Change • Liquid State • Phase Change • Gas State

  38. Endothermic vs. Exothermic • Endothermic • System that absorbs energy/heat from its surrounding • Phase Changes: melting, sublimation, vaporization • Exothermic • System that releases energy/heat to its surrounding • Phase Changes: freezing, condensation, deposition

  39. Temperature Indicators • Boiling Point • When liquid goes to a gas • 100ºC for water • Freezing Point • When liquid goes to a solid • 0ºC for water

  40. Evaporation or Boiling--Vaporization can be evaporation or boiling Evaporation Boiling Liquid to gas At temperatures above the boiling point At the bottom • Liquid to gas • At temperatures below the boiling point • At the surface

  41. END THE UNIT

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