1. B C D E A B C D E A B C D E A B C D E A B C D E A KINETIC ENERGY PERIODIC TRENDS STOICHIO- METRY GAS LAWS MOLECULAR STRUCUTRES

2. MOLECULAR STRUCTURES Question 1 What is the weakest intermolecular force?

3. London Dispersion Forces BOOM!

4. MOLECULAR STRUCTURES Question 2 What are the strongest intermolecular forces?

5. Hydrogen Bonds 40pts

6. MOLECULAR STRUCTURES Question 3 What structure does NH 3 have?

7. Trigonal Planar SWITCH!

8. MOLECULAR STRUCTURES Question 4 What bond angles does SF 6 have?

9. 90 o 100pts

10. MOLECULAR STRUCTURES Question 5 What are the two possible bond angles for bent structures?

11. 120 o and 105 o BOOM!

12. KINETIC ENERGY Question 1 What are the 3 parts of the Kinetic Theory of Matter?

13. 1)All matter is made of particles 2)All particles are under Brownian motion 3)All particles have complete elastic collisions 50pts

14. KINETIC ENERGY Question 2 What is the most common state of matter in the universe?

15. Plasma 10pts

16. KINETIC ENERGY Question 3 What is absolute zero?

17. The temperature at which all kinetic motion stops; 0 K BOOM!

18. KINETIC ENERGY Question 4 What is happening at “J”?

19. Condensation SWITCH!

20. KINETIC ENERGY Question 5 What is it called when atmospheric pressure and vapor pressure on a liquid are equal?

21. Boiling point BOOM!

22. PERODIC TRENDS Question 1 Which has a smaller atomic radii, F or Li?

23. Fluorine BOOM!

24. PERIODIC TRENDS Question 2 Why are cation atoms always smaller than their ground state atoms?

25. Cations have less electrons so their atomic radii is smaller 100pts

26. PERIODIC TRENDS Question 3 What force tells us if two elements will make an ionic, covalent, polar, or non-polar compound?

27. ∆EN  electronegativity SWITCH!

28. PERIODIC TRENDS Question 4 The Lanthanide series and Actinide series are part of what periodic group?

29. Inner Transition Metals 10pts

30. PERIODIC TRENDS Question 5 Why does ionization energy increase as an atom gets smaller?

31. As the atom gets smaller, the electrons are closer to the positive nucleus so it requires more energy to pull them away from the atom 100pts

32. STOICHIOMETRY Question 1 What is the volume of 1 mole of a gas at STP?

33. 22.4 L 10pts

34. STOICHIOMETRY Question 2 How many grams of sodium are needed to react with.071g of chlorine gas? 2Na (s) + Cl 2(g)  2NaCl (s)

35. 50pts 0.071 g Cl 2 71 g Cl 2 1 mol Cl 2 = 0.046 g Na 1 mol Cl 2 2 mol Na 46 g Na

36. STOICHIOMETRY Question 3 According to your calculations the theoretical yield for the production of NaCl is 13.6 grams. In the laboratory your actual yield is 11.8 grams of NaCl. What is the percent yield?

37. BOOM! 13.6 g NaCl 11.8 g NaCl x 100 Answer = 86.7 %

38. STOICHIOMETRY Question 4 What is the difference between an empirical formula and a molecular formula?

39. Empirical formula  lowest whole number ratio for compound (CH 2 O) Molecular formula  actual ratio of elements in compound (C 6 H 12 O 6 ) 10pts

40. STOICHIOMETRY Question 5 Caffeine has a molar mass of 194 g. It’s empirical formula is C 4 H 5 ON 2. What is its molecular formula?

41. C 4 H 5 ON 2 = 97.11g Ratio= 194g/ 97.11g = 2 2 x (C 4 H 5 ON 2 ) = C 8 H 10 O 2 N 4 40pts

42. GAS LAWS Question 1 What gas law is this demonstrating?

43. Charles 'Law V 1 /T 1 = V 2 /T 2 30pts

44. GAS LAWS Question 2 How should temperatures ALWAYS be calculated when dealing with gas laws?

45. Using Kelvin (K) 273 + o C BOOM!

46. GAS LAWS Question 3 The gas law that shows the relationship between temperature, pressure, and volume is called what?

47. The Combined Gas Law P 1 V 1 /T 1 = P 2 V 2 /T 2 BOOM!

48. GAS LAWS Question 4 Atmospheric pressure being 101.3 kPa comes from what gas law?

49. Dalton’s Law of Partial Pressures P total = P 1 + P 2 + P 3 + ….P n+ 50pts

50. GAS LAWS Question 5 What gas law does this demonstrate?

51. Boyle’s Law P 1 V 1 = P 2 V 2 20pts