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End of Course Review

End of Course Review. Reporting Category 1: C.4A. A woman goes to her hair dresser to have her hair done. What is the difference between having her hair trimmed and getting her hair colored? Which is a physical change and which is a chemical change? JUSTIFY your answer!.

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End of Course Review

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  1. End of Course Review

  2. Reporting Category 1: C.4A • A woman goes to her hair dresser to have her hair done. What is the difference between having her hair trimmed and getting her hair colored? Which is a physical change and which is a chemical change? JUSTIFY your answer!

  3. Reporting Category 1: 4B • Prove that density is an intensive property using an example that you create/design.

  4. Reporting Category 1: 4C • Create a complex (3+ circle) Venn Diagram highlighting similarities and differences among solids, liquids and gases.

  5. Reporting Category 1: 4D • Describe the process you might take to identify an unknown substance in a laboratory setting.

  6. Reporting Category 1: 5A • Given the time period, JUSTIFY why Mendeleev’s periodic table was organized by atomic mass and not atomic number.

  7. Reporting Category 1: 5B • Make a statement regarding which families on the periodic table naturally like to form bonds with one another. JUSTIFY how you know this to be true.

  8. Reporting Category 1: 5C • Make a correlation between metallic character and electronegativity.

  9. Reporting Category 2: 6A • Explain using historical events as evidence which SPECIFIC parts of Dalton’s Atomic Theory have been modified since it’s publication.

  10. Reporting Category 2: 6B • Define direct and inverse relationships in your own words. Decide how energy & wavelength are related; how energy & frequency are related; how frequency & wavelength are related.

  11. Reporting Category 2: 6C #1 • Calculate the frequency of a 340 nm wavelength.

  12. Reporting Category 2: 6C #2 • Calculate the energy of the 340 nm wavelength.

  13. Reporting Category 2: 6D • Calculate the average atomic mass of oxygen given the following information: • Oxygen-16 (99.76%) • Oxygen-17 (0.037%) • Oxygen-18 (0.204%)

  14. Reporting Category 2: 6E • Give the electron configuration, noble gas configuration and Lewis dot diagram for each of the following: • Calcium • Fluorine • Carbon • Sodium

  15. Reporting Category 2: 12A • Identify the three major types of radioactive decay. What is the relationship between mass of radiation and penetrating power? Which type of decay is the most powerful and thus most difficult to protect against?

  16. Reporting Category 2: 12B • Balance the following nuclear reactions: • Cerium-144  Praseodymium-144+ _________ • Potassium-40  Argon-40 + ______ • Plutonium-239  ______ + 1 alpha particle

  17. Reporting Category 2: 12C • Write a short persuasive essay. Decide whether you are for or against nuclear fission as a means for generating power. Use your knowledge of both fission and fusion to support your argument.

  18. Reporting Category 3: 7A • Name the following compounds: • H3PO4 • H2S • CaCO3 • Cu(NO3) 2 • NaF • P4O10

  19. Reporting Category 3: 7B • Write the formulas for the following: • Lead (IV) sulfate • Iron (III) oxide • Carbon monoxide • Hydroiodic acid • Magnesium fluoride

  20. Reporting Category 3: 7C • Draw Lewis dot diagrams for the following compounds: • Carbon dioxide • Sodium chloride • Ammonia • water

  21. Reporting Category 3: 7D • What defining feature of metals and metallic bonding offers an explanation of the properties of metals such as conductivity of heat & electricity as well as malleability and ductility?

  22. Reporting Category 3: 7E • Give a chemical compound example for each of the following VSEPR shapes: • Bent (2E) • Tetrahedral • Trigonal pyramidal • Trigonal planar

  23. Reporting Category 3: 8A #1 • Calculate the number of moles in 3.54 x 1025 atoms of silver.

  24. Reporting Category 3: 8A #2 • Calculate the number of molecules in 3.5 moles of carbon dioxide.

  25. Reporting Category 3: 8A #3 • Calculate the number of atoms in 4.7 moles of sulphur.

  26. Reporting Category 3: 8B #1 • How many moles are in 14 grams of Ba(OH)2?

  27. Reporting Category 3: 8B #2 • How many atoms of iodine are in a 3.85 g sample of iodine?

  28. Reporting Category 3: 8B #3 • 11.2 g of carbon dioxide contains how many molecules of carbon dioxide?

  29. Reporting Category 3: 8C #1 • Calculate the percent carbon in acetaminophen (C8H9NO3).

  30. Reporting Category 3: 8C #2 • What is the difference between an empirical formula and a molecular formula?

  31. Reporting Category 3: 8C #3 • A compound is 40.0 % carbon, 6.7% hydrogen and 53.5 % oxygen. What is the empirical formula?

  32. Reporting Category 3: 8C #4 • What is the molecular formula of the compound in 8C #3, if the molar mass is 60. g = 1 mol?

  33. Reporting Category 3: 8D • Balance the following reactions: • Mg + O2 MgO • FeO + Al  Al2O2 + Fe • C3H8 + O2  CO2 + H2O

  34. Reporting Category 3: 8E • Consider the combustion of 315 g of butane (C4H10) with an excess of oxygen. If you collect 301 g of water in the lab, what was your percent yield?

  35. Reporting Category 4: 9A #1 • Give the complete version of the combined gas law. Identify within the combined gas law the following laws: • Boyle’s Law • Charles’ Law • Avogadro’s Law

  36. Reporting Category 4: 9A #2 • Describe how you know when to use ideal gas law versus the combined gas law.

  37. Reporting Category 4: 9A #3 • A 2.00L fire extinguisher has an internal pressure of 410 kPaat 20°C. What volume of methyl bromide is needed to fill an empty extinguisher at STP?

  38. Reporting Category 4: 9A #4 • A 3.8 mol sample of gas is placed in a container with a volume of 35 L @ 42°C. What is the pressure exerted by the gas?

  39. Reporting Category 4: 9B • What volume of oxygen gas is needed to form 35 g of nitrogen dioxide from the reaction between nitrogen monoxide and oxygen?

  40. Reporting Category 4: 11A • Compare and contrast potential versus kinetic energy. Give at least two examples of each (forms like light or heat, etc).

  41. Reporting Category 4: 11B • Define the law of conservation of energy. This being true, explain where energy absorbed by endothermic reactions comes from and where energy given off by exothermic reactions goes to.

  42. Reporting Category 4: 11C • Calculate the enthalpy of reaction for the combustion of methane (CH4). Determine if the reaction is endo/exo.

  43. Reporting Category 4: 11D #1 • How much heat is required to raise 50.0g of Al from 10°C to 56°C? Specific heat of aluminum is 0.900 J/g°C.

  44. Reporting Category 4: 11D #2 • To make an 8 cup pot of green tea, you must heat water to boiling at STP. If there are 1.4 kg of water and the temperature at the tap is 23°C, how much heat must be absorbed by the water? Specific heat of water is 4.18 J/g°C.

  45. Reporting Category 5: 10A • Water has a number of unique properties. What factor is the major driving force of water’s uniquness?

  46. Reporting Category 5: 10B • The poison used in a recent murder is either potassium iodide or silver nitrate. You have access to 0.1M solutions of sodium chloride and sodium carbonate. Formulate a process by which you could perform tests on the poison to determine its identity.

  47. Reporting Category 5: 10C • Calculate the molarity of a solution given 3.58 g of calcium hydroxide and enough water to create 500 mL of solution.

  48. Reporting Category 5: 10D • Concentrated nitric acid is 18.0M. What volume is needed to make 1.50L of 0.750M solution?

  49. Reporting Category 5: 10E • Create a complex Venn Diagram contrasting and comparing unsaturated, saturated, and supersaturated solutions.

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