Chemistry Jeopardy Review!!!

1. Chemistry Jeopardy Review!!!

2. Final Jeopardy

3. Introduction to Chemistry 100 This is the definition of Chemistry

4. Introduction to Chemistry 200 In a lab report, this crucial section should be located between the materials/procedure and the analysis

5. Introduction to Chemistry 300 It is the name for the lab equipment pictured here

6. Introduction to Chemistry 400 The six easy to observe signs of a chemical change are color change, gas produced, odour change, solid produced light produced and this.

7. Introduction to Chemistry 500 Melting point is an example of this type of property

8. Introduction to Chemistry 600 This is the ability to reproduce the same result over and over. This doesn’t necessarily mean getting the correct result.

9. Introduction to Chemistry 700 If you had 350g of gold and you added 315g of gold to it, you would have this mass of gold.

10. Introduction to Chemistry 800 When converting grams to kilograms, you would use a conversion factor that looks like this.

11. Introduction to Chemistry 900 The units used to measure volume are derived from this SI Unit (be careful!).

12. Introduction to Chemistry 1000 This is the distance light would travel in one year if it was travelling 3.0 x 108 m/s

13. Atoms and Elements 100 The periodic table was organized by this Russian chemist.

14. Atoms and Elements 200 This chemist won the nobel prize in chemistry 100 years ago. She also won the nobel prize in physics in 1903.

15. Atoms and Elements 300 The diatomic elements are Hydrogen, Nitrogen, Bromine, Iodine, Chorine, Fluorine and this.

16. Atoms and Elements 400 This is the latin name for gold, and where it gets its symbol Au from

17. Atoms and Elements 500 This is the particle in an atom that has the most mass.

18. Atoms and Elements 600 The isotope represented below has this many neutrons:

19. Atoms and Elements 700 The lewis dot structure for a neutral iodine atom has this number of dots around it.

20. Atoms and Elements 800 This is the number of electrons the fundamental orbital holds.

21. Atoms and Elements 900 This is the abbreviated electron configuration for lead

22. Atoms and Elements 1000 This is the percent abundance of boron 11 (which has a mass of 11.009amu) to 2 decimal places. Boron’s other isotope is 10B (10.013 amu)

23. Molecules and Compounds 100 A triple bond occurs when this number of electrons are shared between two atoms

24. Molecules and Compounds 200 This is what happens with electrons when a metal bonds with a non-metal.

25. Molecules and Compounds 300 These are forces within a molecule such as ionic or covalent bonding. (enunciate please)

26. Molecules and Compounds 400 This is the number of nitrogen atoms in ammonium ferrocyanide.

27. Molecules and Compounds 500 This is the name given to the compound with the chemical formula: Cu3(BO3)2

28. Molecules and Compounds 600 This is the name of the compound with the following chemical formula: P4O10

29. Molecules and Compounds 700 This is the name of the compound with the chemical formula: HNO2

30. Molecules and Compounds 800 This is the molecular and electron pair geometry for XeH2

31. Molecules and Compounds 900 These are the intermolecular forces involved in hydrosulfuric acid

32. Molecules and Compounds 1000 This is the 3D drawing of hydrosulfuric acid

33. Chemical Reactions 100 One way to increase the rate of a reaction is to increase this so the molecules move around faster and collide more often

34. Chemical Reactions 200 If a substance is in a closed system with high temperature and low pressure it would most likely be in this state

35. Chemical Reactions 300 When aqueous barium iodide mixes with copper (II) sulfate, this precipitate forms

36. Chemical Reactions 400 This term means “Within heating” and can be used to describe a reaction where an energy term is on the reactants side of the balanced equation

37. Chemical Reactions 500 This is the name of the exothermic biochemical reaction that occurs when sugar combines with oxygen.

38. Chemical Reactions 600 When magnesium reacts with water, the reaction type is this.

39. Chemical Reactions 700 The activity series is used to determine if this type of reaction will occur

40. Chemical Reactions 800 When you balance the following equation using whole numbers, you end up with this coefficient in front of hydrochloric acid: __KMnO4+ __HCl __KCl + __MnCl2 + __H2O + __Cl2

41. Chemical Reactions 900 This is the word equation for the combination of sodium nitrate and potassium chloride

42. Chemical Reactions 1000 This is the net ionic equation for the reaction that occurs between hydrochloric acid and sodium hydroxide

43. Moles! 100 This is the molar mass of sodium

44. Moles! 200 This is the molar mass of aluminum borate

45. Moles! 300 This is the mass of 2.00 moles of chlorine gas

46. Moles! 400 This is how many atoms are in a 2.0 g sample of lead (II) iodide.

47. Moles! 500 2.3 moles of hydrogen gas would take up this volume at STP

48. Moles! 600 This is the percent composition of oxygen in water to one decimal place.

49. Moles! 700 A solution would have this concentration if you combine 3.42 moles of solute with 50mL of water.

50. Moles! 800 In the reaction between propane and oxygen, if we want to completely react 10.0g of propane, what is the least amount (volume) of oxygen we could use (@STP)?