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Mixtures! Let’s Review

Mixtures! Let’s Review

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Mixtures! Let’s Review

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  1. Mixtures! Let’s Review

  2. What were our solutes and solvents yesterday? Remember these are only for solutions!

  3. Particle Size…

  4. The Tyndall Effect

  5. Let’s relate this to our lab yesterday… • Which substances DID NOT scatter the light? • Which substances DID scatter the light? • DID NOT: water, sugar water, copper sulfate • DID: Milk, Oil • Light did not go through….but still scattered light • Soil

  6. Solutions • A solution is a homogeneous mixture of two or more components. The dissolving agent is the solvent. The substance which is dissolved is the solute. The components of a solution are atoms, ions, or molecules, which makes them 10-9 m or smaller in diameter. • Example: Sugar and Water • Colloids • Particles intermediate in size between those found in solutions and suspensions can be mixed such that they remain evenly distributed without settling out. These particles range in size from 10-8 to 10-6 m in size and are termed colloidal particles or colloids. The mixture they form is called a colloidal dispersion. A colloidal dispersion consists of colloids in a dispersing medium. • Example: Milk • Suspensions • The particles in suspensions are larger than those found in solutions. Components of a suspension can be evenly distributed by a mechanical means, like by shaking the contents, but the components will settle out. • Example: Oil and Water

  7. SOLUTIONS • Do not settle out • Pass unchanged through ordinary filter paper • Do not scatter light • SUSPENSIONS • Settle out on standing • Separated by ordinary filter paper • Scatter light • COLLOIDS • Do not settle out • Pass unchanged through ordinary filter paper • Scatter light

  8. Examples…. SOLUTIONS Salt water Syrup (sugar in water) Vinegar (acetic acid in water) Paper glue (usually polyvinylacetate dissolved in water) Shampoo (various soaps and surfactants dissolved in water) Bronze (copper dissolved into tin and then cooled) Fizzy water (carbon dioxide in water) COLLOIDS Milk Mayonnaise hand cream whipped cream shaving cream Fog Mist hair sprays Gelatin Jelly Smoke Cloud Blood SUSPENSIONS sand in water dust in air Dirt in water Oil in water

  9. The bigger picture… What is a mixture? How does that differ from a pure substance?

  10. Let’s think…

  11. Pure substances • A pure substance has a definite and constant composition — like salt or sugar. A pure substance can be either an element or a compound, but the composition of a pure substance doesn’t vary. • Elements • An element is composed of a single kind of atom. An atom is the smallest particle of an element that still has all the properties of the element. • Here’s an example: Gold is an element. If you slice and slice a chunk of gold until only one tiny particle is left that can’t be chopped any more without losing the properties that make gold gold, then you’ve got an atom. • Compounds • A compound is composed of two or more elements in a specific ratio. For example, water is a compound made up of two elements, hydrogen (H) and oxygen (O). These elements are combined in a very specific way — in a ratio of two hydrogen atoms to one oxygen atom, known as:H2O • Many compounds contain hydrogen and oxygen, but only one has that special 2 to 1 ratio we call water. The compound water has physical and chemical properties different from both hydrogen and oxygen — water’s properties are a unique combination of the two elements. • Chemists can’t easily separate the components of a compound: They have to resort to some type of chemical reaction.

  12. Mixtures • Mixtures are physical combinations of pure substances that have no definite or constant composition — the composition of a mixture varies according to who prepares the mixture. • Although chemists have a difficult time separating compounds into their specific elements, the different parts of a mixture can be easily separated by physical means, such as filtration. • For example, suppose you have a mixture of salt and sand, and you want to purify the sand by removing the salt. You can do this by adding water, dissolving the salt, and then filtering the mixture. You then end up with pure sand. • Mixtures can be either homogeneous or heterogeneous: • A homogeneous mixture, sometimes called a solution, is relatively uniform in composition; every portion of the mixture is like every other portion. • For example, if you dissolve sugar in water and mix it really well, your mixture is basically the same no matter where you sample it. • A heterogeneousmixture is a mixture whose composition varies from position to position within the sample. • For example, if you put some sugar in a jar, add some sand, and then give the jar a couple of shakes, your mixture doesn’t have the same composition throughout the jar. Because the sand is heavier, there’s probably more sand at the bottom of the jar and more sugar at the top.

  13. molecule

  14. Activity time! • Find a partner • Take one of the CLASS COPIES • DRAW the particle examples in your notes! • Answer the questions on your notes or a separate sheet of paper. • Work on review packet once you are finished.

  15. Sources • • • • •