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What weapon can you make from potassium, nickel, and iron?

What weapon can you make from potassium, nickel, and iron?. A KNiFe !!!. Journal:. Please answer the following questions in your journal What was the most difficult part of the atomic structure unit for you? What is your specific plan to prepare for your test next week?

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What weapon can you make from potassium, nickel, and iron?

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  1. What weapon can you make from potassium, nickel, and iron?

  2. A KNiFe!!!

  3. Journal: • Please answer the following questions in your journal • What was the most difficult part of the atomic structure unit for you? • What is your specific plan to prepare for your test next week? • What is the atomic structure of Potassium? You may write it shorthand or extended form • What happens to the electrons in the gas discharge tubes we looked at? How is light produced?

  4. Unit 2: Aqueous Reactions Write a balanced chemical formula for the reaction of: Lead (II) nitrate + potassium iodide  lead (II) iodide + potassium nitrate http://www.youtube.com/watch?v=DITY2rXYU-I&feature=related Write down the physical characteristics (what color, consistency) of the reaction before and after

  5. Pb(NO3)2 + 2KI  PbI2 + 2KNO3 • When we have a double displacement reaction, there are 2 indicators of chemical change 1. change of colour 2. a precipitate forms

  6. Solutions & Solubility

  7. Heterogeneous Mixtures • Heterogeneous mixtures(not all the same parts)

  8. Homogeneous Mixtures • all parts are evenly distributed on a microscopic level • Cannot see separate parts

  9. Homogeneous Mixtures • Also called solutions • Two or more substances in one state • Solute  substance that is dissolved in solution • ex. Iced tea crystals dissolved in water • Solvent  substance that does the dissolving • ex. The water that dissolves the iced tea crystals

  10. Aqueous Solutions • When water is the solvent we call the solution aqueous (root of the word is aqua = water) • Solutions are clear or transparent (coloured but you can see through it)

  11. Solvation • Soluble: a solute dissolves in a specific solvent • Insoluble/slightly soluble: the solute does not dissolve • The amount of solute that will dissolve in a particular solvent is described by its “solubility”

  12. So which one is the solute? • Whichever reactant changed phases • Ex. Solid to liquid • If there was no state change, then the substance in the GREATEST amount is usually the solvent

  13. Solutions • Are homogeneous • Are stable (nothing settles out or precipitates) • Solute & Solvent will pass through a filter • Are in a single phase • Solutes and solvents may be solid, liquid, or gas

  14. Concentration (moles/L) • Concentrated solution: large amount of solute for solvent present • Ex. Syrup (sugar) • Dilute Solution: small amount of solute for solvent present 1g of NaCl in 100 g of water 30g of NaCl in 100 g of water

  15. What is the concentration of a salt solution that contains 0.90 grams of sodium chloride in 100ml of solution?

  16. What is the concentration of our saline solution if we diluted it with 200 ml of water? [stock] = 0.15 mol/L [dilute] = ? Volume, stock = 100mL volume, dilute = 300ml Moles = ? moles = ?

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