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5. 100 200 300 400 500 Atomic History and Model Chemical Bonding Chemical Reactions Kinetics and Equilibrium Solutions Acids and Bases ™

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

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

8. What is the gold foil experiment and why what did it prove. A 200

9. Earnest Rutherford shot particles at gold foil and the particles went through the foil. This experiment demonstrated that atoms are mostly empty space which was a new concept at the time. A 200

10. What is an isotope? A 300

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

12. In general, do metals become more or less reactive as you go down a group? A 400

13. Elements generally get more reactive as you go down a group because there are more electrons shielding the valence electrons from the nucleus. A 400

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

15. 6 Protons; 8 neutrons A 500

16. What are the three major types of Bonding B 100

17. Ionic, Covalent, Metallic B 100

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

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

20. Why do atoms form ions? B 300

21. Because all atoms want to have electron configuration like Noble gases, thus they will gain or lose electrons in order to become like noble gases.

22. What types of elements form ionic bonds, covalent bonds and metallic bonds? B 400

23. Ionic – Metal and Non-metal, or metal and Polyatomic ion Covalent – Non-metal and Non-metal Metallic – Metal and Metal B 400

24. What are characteristics of ionic substances? B 500

25. High melting and boiling points Dissolve readily in water and conduct electricity Brittle Solids B 500

26. What are some signs of a chemical reaction? C 100

27. Bubbling, Color Change, Precipitate, Temperature Change

28. C 200 What is the law of conservation of mass?

29. Matter cannot be created or destroyed. We must have a balanced chemical equation. C 200

30. What is the mole ratio and where is it found? C 300

31. The mole ratio related the amount of one substance to the amount of another substance in the chemical reaction. It can be found in a balanced chemical equation. C 300

32. DAILY DOUBLE C 400 DAILY DOUBLE Place A Wager

33. Solve the stoichiometry problem Ms. Jensen is putting on the board. C 400

34. Ms. Jensen will determine if you are correct. C 400

35. Define endothermic and exothermic reactions. C 500

36. 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. C 500

37. What are the four major factors that effect the rate of a chemical reaction D 100

38. Temperature Surface Area Concentration Catalysts D 100

39. What is an effective collision? D 200

40. A collision where molecules have the right speed and angles in order to create a reaction. D 200

41. What is equilibrium? D 300

42. A state at which a reactions forwards reaction rate equals the reverse reaction rate. Products and reactants are being produced in equal amounts. D 300

43. How does adding more reactants effect the equilibrium in a reaction? D 400

44. If you add more reactant the equilibrium will shift right in order to reestablish equilibrium according to Le Chateliers Principle. D 400

45. Which way will an endothermic reaction shift if we decrease the temperature? D 500

46. The reaction will shift left to reestablish equilibrium. D 500

47. What is the solute? E 100

48. The substance that is dissolved in the solvent. E 100

49. What are the units of Molarity and molality? E 200

50. Molarity – moles of solute/liters of solution Molality – moles of solute/kg of solvent E 200

51. What are the three colligative properties? E 300

52. Vapor Pressure Decreasing Boiling Point Elevation Freezing Point Depression E 300

53. . E 400 Which will lower the freezing point the most and why? NaCl or C 6 H 12 O 6

54. NaCl, because it dissociates into two particles and will hold solvent particles in the liquid more effectively that molecular substances that do not dissociate. E 400

55. Name two instances where colligative properties are used in everyday life. E 500

56. Road Salt Anti-Freeze in cars Other responses will be judged by Ms. Jensen E 500

57. F 100 What makes a substance an acid?

58. The ability to dissociate into H+ ions. F 100

59. What is an acid on the pH scale? F 200

60. Anything lower than 7. F 200

61. What is the [OH - ] in a neutral solution? F 300

62. 1 x10 -7 F 300

63. Calculate the molarity of HCl if 20.0 mL of it are needed to neutralize 34.0 mL of a 0.90 M NaOH solution. F 400

64. 1.53 M F 400

65. What is the most massive type of radiactive decay? F 500

66. Alpha particles F 500

67. The Final Jeopardy Category is: Nuclear Click on screen to begin

68. you have 200 g of Th-234. The half life is 5.0 min. How many grams are left after 15 min? Click on screen to continue

69. 25 g Click on screen to continue

70. Thank You for Playing Jeopardy!