Questions for Final Review Game (X)
1. Who is credited as the main developer of the periodic table? How did he arrange his table? How is this different from our current model of the periodic table?
2. Why are groups on the periodic table also called “families” sometimes? Why does this phenomenon happen?
3. Explain the trend for atomic radius. Which has a larger atomic radius: metals or nonmetals?
4. Explain the trend for electronegativity. Which group is more electronegative: the halogens or the alkaline earth metals?
5. Name some properties of the alkali metals.
6. What is special about the noble gases? Why is this the case?
7. How can you determine whether a bond is covalent or ionic?
8. How can you decide between polar covalent and nonpolar covalent?
9. What type of bonds are present in RbCl2?
10. What type of bonds are present in CO2?
11. What are the three intermolecular forces we discussed in class? Rank them in order from weakest to strongest.
12. What is the dominant intermolecular force in CO2?
13. What is the dominant intermolecular force in H2O?
14. List all of the intermolecular forces present in ammonia (NH3)?
15. What type of solid is KNO3?
16. What type of solids are made of elements from Group 14 (generally)? For example: graphite or diamond.
17. Name the three endothermic phase changes.
18. Name the three exothermic phase changes.
19. List the name and corresponding phases involved in the phase change. Then, list the phase change that is the opposite.
20. At what time does boiling begin?
21. Where would freezing occur on this curve?
22. At which segment(s) would there be a liquid present?
23. What is the name for 0°C based on the graph?
24. If you have a saturated solution of salt and you add more water to it, would the solution become unsaturated or supersaturated?
25. What do the words “miscible” and “immiscible” mean if you are talking about two liquids?
26. What is the solubility of potassium nitrate at 40°C?
27. How many grams of KClO3 could be dissolved in 100 grams of water at 65°C?
28. If 50 grams of KCl are dissolved in 50°C, is the solution saturated, unsaturated, or supersaturated?
29. Which compound is least soluble at 10°C?
30. What is the difference between an endothermic and exothermic reaction?
31. Which is true of an exothermic reaction?
a. The temperature in the system increases over the course of the reaction.
b. The temperature of the surroundings decreases over the course of the reaction.
c. The products have more energy than the reactants.
d. The reactants have more energy than the products.
32. In terms of the heat term “q,” what would the sign on this value be for an exothermic reaction? For an endothermic reaction?
33. According to Arrhenius, an acid is a substance that
a. contains a hydrogen ion (yields a hydrogen ion when mixed with water)
b. contains a hydroxide ion (yields a hydroxide ion when mixed with water)
c. has a pH greater than seven.
34. Which answer choice accurately describes the Bronsted-Lowry model of acids and bases?
a. Bases donate H+ ions; acids accept H+ ions.
b. Acids donate H+ ions; bases accept H+ ions.
c. Bases donate OH- ions; acids accept OH- ions.
d. Acids donate OH- ions; bases accept OH- ions.
35. All of the statements are true for bases except
a. Bases taste bitter.
b. Bases will turn red litmus paper blue.
c. Bases are corrosive and can cause severe burns.
d. Aqueous solutions of bases have a pH lower than seven.
36. All of the statements are true for acids except
a. Acidic solutions have pH’s lower than 7.
b. Sulfuric acid (H2SO4) and nitric acid (HNO3) are strong acids.
c. Every acid has a conjugate acid.
d. Acids will turn blue litmus paper red.
37. Label the following compounds as acid, base, both, or neither:
a. NO3-1
b. H2SO4
c. K2SO4
d. H2PO4-1
38. What is the hydrogen ion concentration of a solution of ammonia with an [OH-] of 7.5 x 10-3 M? Is this solution acidic or basic?
39. What is the pH of a 0.93 M solution of HCl?
40. What are the pOH, [H+], and [OH-] of a solution with a pH of 11.4? Is this solution acidic or basic?
41. Let’s say you have an empty plastic water bottle. If you keep trying to force air into the bottle, what will happen to the pressure over time? Why?
42. What is temperature? How does temperature affect the volume of a gas and why?
43. Which gas will effuse and diffuse faster: carbon monoxide or carbon dioxide?
44. Which gas will effuse and diffuse slower: CH4 or CH3OH?
45. What is the difference between the ground state and the excited state for an electron?
46. Which sublevels (s, p, d, or f) are located in the third principal energy level? How many electrons would fit in this third energy level?
47. How many orbitals are in the fourth energy level?
48. What would the Lewis structure look like for PCl3? What VSEPR shape would this molecule have?
49. What is the molecular geometry of CO2?
50. What is the molecular geometry of H2O? Is this molecule polar or nonpolar?
51. What is the VSEPR geometry of CO3? Is this molecule polar or nonpolar?
52. Draw the Lewis structure for SO42-. What is the shape of this molecule?
53. Of the VSEPR geometries, which will always be polar?
54. What mass of barium chloride (BaCl2) is needed to make 0.5 L of a 4.0 M solution?
55. What is the molarity of a solution in which 1.6 g of sodium hydroxide (NaOH) are dissolved in 125 mL of solution?
56. What is the molarity of a solution in which 5.0 g of sodium carbonate (Na2CO3) are dissolved in 200 mL of solution?
57. If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?
58. I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be?
59. If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?
60. Submarines need to be extremely strong to withstand the extremely high pressure of water pushing down on them. An experimental research submarine with a volume of 15,000 liters has an internal pressure of 1.2 atm. If the pressure of the ocean breaks the submarine forming a bubble with a pressure of 250 atm pushing on it, how big will that bubble be in L?
61. On hot days, you may have noticed that potato chip bags seem to “inflate”, even though they have not been opened. If I have a 250mL bag at a temperature of 19°C, and I leave it in my car which has a temperature of 60°C, what will the new volume of the bag be?
62. I place a balloon in my fridge that initially has a temperature of 220 C and an initial volume of 0.5 liters. Once the balloon reaches the temperature of the refrigerator, I measure the final volume as 0.47 L. What is the final temperature of my refrigerator in Kelvin? In °C?
63. A gas storage tank has a volume of 3.5 x 105 mL when the temperature is 27°C and the pressure is 1.0 atm. What is the new volume of the tank if the temperature drops to -10°C and the pressure drops to 0.95 atm?
64. Determine the temperature required for a 0.09494 g sample of hydrogen gas (H2) to fill a balloon to 1.20 L under 0.988 atm pressure.
65. If the pressure exerted by a gas at 25°C in a volume of 44 mL is 3.81 atm, how many moles of gas are present?
66. How many moles of gas are in a scuba tank if the temperature of the tank is 30°C and the pressure is 200 atm? The volume of the tank is 7 liters.
67. Which element has the electron configuration 1s22s22p63s23p3?
68. How many unpaired electrons does germanium have in its valence shell? (Hint: draw the orbital diagram first!)
69. What is the full electron configuration for cobalt? What is the noble gas (abbreviated) configuration?
70. What is the noble gas configuration for zirconium?
71. What is the orbital diagram configuration for sulfur?
72. Draw an orbital diagram for chlorine.
73. What do the coefficient, letter, and exponent signify in an electron configuration?
74. What is the electron configuration for iridium?
75. Titanium is a metal used in jet engines. Its specific heat is 0.523J/g·°C. If 5.88 g of titanium absorbs 4.78 J, what is the change in temperature?
76. Stainless steel accessories in cars are usually plated with chromium to give them a shiny surface and to prevent rusting. When 5.00 g of chromium at 23°C absorbs 62.5 J of heat, the temperature increases to 50.8°C. What is the specific heat of chromium?
77. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C?