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THIS. IS. ™. JEOPARDY. Jeopardy. ™. Review problems. Colligative properties. Titrations and reactions. Acids and Bases. pH. Electro chemisty. 100. 100. 100. 100. 100. 100. 200. 200. 200. 200. 200. 200. 300. 300. 300. 300. 300. 300. 400. 400. 400. 400. 400. 400.

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  1. THIS IS ™ JEOPARDY

  2. Jeopardy ™ Review problems Colligative properties Titrations and reactions Acids and Bases pH Electro chemisty 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500

  3. Why do elements in a group have similar chemical characteristics A 100

  4. Because they all have the same number of valence electrons A 100

  5. What is the difference between ionic and covalent bonds in terms of electrons? A 200

  6. Covalent Bonds – Electrons are shared between atoms Ionic Bonds – Electrons are transferred from one atom to another. A 200

  7. What is an isotope? A 300

  8. An atom that has different amounts of neutrons. A 300

  9. Define endothermic and exothermic reactions. A 400

  10. Exothermic reactions are reactions where energy is a released, ∆H is negative and reactions generally feel warm. Endothermic reactions are reactions where energy is absorbed, ∆H is positive and reactions generally feel cold. A 400

  11. How many protons and neutrons are in an element of Carbon-14? A 500

  12. 6 Protons; 8 neutrons A 500

  13. What are the three colligative properties? B 100

  14. Vapor Pressure Decreasing Boiling Point Elevation Freezing Point Depression B 100

  15. Which will lower the freezing point the most and why? NaCl or C6H12O6 B 200

  16. NaCl, because it dissociates into two particles and will hold solvent particles in the liquid more effectively that molecular substances that do not dissociate. B 200

  17. Name two instances where colligative properties are used in everyday life. B 300

  18. Road Salt Anti-Freeze in cars Other responses will be judged by Ms. Jensen B 300

  19. What is the freezing point and boiling point of a 0.5 m aqueous MgSO4 solution? B 400

  20. Freezing point: -1.86 degrees Boiling point: 100.5 degrees B 400

  21. What is the boiling point of a solution made from 20.0 g of CO2 in 400 g of water? B 500

  22. Boiling point: 100.5 degrees B 500

  23. Find the pH if [H+] = 1 x 10 -9 M And tell if the solution is acidic or basic C 100

  24. 9; basic C 100

  25. What is the pH if [OH-] = 1 x 10 -6 M and tell if it is acidic or basic C 200

  26. 8; basic C 200

  27. Find the pH of a 2.6 x 10-3 M HCl solution and tell if it is acidic or basic C 300

  28. 2.6 ; acidic C 300

  29. DAILY DOUBLE DAILY DOUBLE Place A Wager C 400

  30. Find the pH a 6.7 x 10-2 Ca(OH)2 solution and tell if it is acidic or basic C 400

  31. 13.1; basic C 400

  32. If a solution has a pH of 6.7, find the hydrogen ion concentration. Is this acidic or basic? C 500

  33. 2 x 10 -7; acidic C 500

  34. What is a titration? D 100

  35. When an acid and a base is added together until they are equivalent to find an unknown concentration D 100

  36. What is the molarity of an HCl solution if 30 mL is needed to neutralize 20 mL of a 0.45 M NaOH solution D 200

  37. 0.3 M D 200

  38. What is the molarity of an H3PO4 solution if 20 mL is completely titrated by 45 mL of a 0.14 M NaOH solution? D 300

  39. 0.105 M D 300

  40. Write a balanced reaction when magnesium hydroxide and nitric acid react D 400

  41. Mg(OH)2 +2HNO3 Mg(NO3)2 + 2H2O D 400

  42. Write a balanced reaction when sodium reacts with hydrobromic acid D 500

  43. 2Na +2 HBr 2NaBr + H2. D 500

  44. Is this reaction a spontaneous redox reaction? Mg + Sn2+  Mg2+ + Sn E 100

  45. Yes, Sn is reduced and is above magnesium and on reduction potential chart E 100

  46. How will electrons flow in a Sr/Sr2+//Zn/Zn 2+ electrochemical cell? E 200

  47. Zinc E 200

  48. What are the oxidation numbers in NO3- E 300

  49. +5, -2 E 300

  50. What is oxidation? E 400

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