Conceptual Chemistry Final Review 2013 Gas Laws Pressure Volume Temperature Number of gas molecules PV=nRT Light Wavelength Frequency Color Energy s, p, d, and f orbitals Atomic orbitals Electron configuration (ex: 1S 2 , 2S 2 , 2P 3 ) Organic Compounds Organic compounds are carbon- based Hydrocarbons Saturated vs. Unsaturated Hydrocarbons Alkane, Alkenes, and Alkynes Naming Hydrocarbons (prefixes:meth, eth, etc) Chemical Formulas of Hydrocarbons Chemical Structures of Hydrocarbons Stick Structures of Hydrocarbons Functional Groups (see reference sheet) Intermolecular Forces (IMFs) Define and Identify Relative strengths Valence Shell Electron Pair Repulsion (VSEPR) Determining Molecular Shape (see reference sheet) Detmining molecular polarity (Polar vs. Non Polar using lewis dot structure and mol. shape) Solutions Definition of Solute and Solvent Soluble vs. Insoluble “Likes Dissolve Likes” Saturated, Supersaturated, Unsaturated Effect of Temperature on Solubility of solids and gases Solubility Curves Water Water is a Polar Covalent molecule Hydrogen Bonds are strong dipole-dipoles Explain why a Meniscus can form in a cylinder Adhesion and Cohesion Capillary Action- alternating adhesion and cohesion Explain why bodies of water freeze top down Water is densest at 4˚C States of Water Evaporation, Condensation, Freezing, Melting Heating Curve of Water Boiling Point and Freezing Point Effect of solute (salt) on boiling/freezing point Effect of altitude on boiling point What is the Specific Heat of water and how does this property relate to temperature moderation in coastal areas Chemical properties of soap and how it works Acids and Bases The pH Scale is based on [H + ] Define acids, bases, and neutral solutions 1
Transcript
Conceptual Chemistry Final Review 2013Gas Laws
Pressure Volume Temperature Number of gas molecules PV=nRT
Light Wavelength Frequency Color Energy s, p, d, and f orbitals Atomic orbitals Electron configuration (ex: 1S2, 2S2, 2P3)
Organic Compounds Organic compounds are carbon-based Hydrocarbons Saturated vs. Unsaturated Hydrocarbons Alkane, Alkenes, and Alkynes Naming Hydrocarbons (prefixes:meth, eth, etc) Chemical Formulas of Hydrocarbons Chemical Structures of Hydrocarbons Stick Structures of Hydrocarbons Functional Groups (see reference sheet)
Intermolecular Forces (IMFs) Define and Identify Relative strengths
Valence Shell Electron Pair Repulsion (VSEPR) Determining Molecular Shape (see reference
sheet) Detmining molecular polarity (Polar vs. Non
Polar using lewis dot structure and mol. shape)
Solutions Definition of Solute and Solvent Soluble vs. Insoluble “Likes Dissolve Likes” Saturated, Supersaturated, Unsaturated Effect of Temperature on Solubility of solids
and gases Solubility Curves
Water Water is a Polar Covalent molecule Hydrogen Bonds are strong dipole-dipoles Explain why a Meniscus can form in a cylinder Adhesion and Cohesion
Capillary Action- alternating adhesion and cohesion
Explain why bodies of water freeze top down Water is densest at 4˚C States of Water Evaporation, Condensation, Freezing, Melting Heating Curve of Water Boiling Point and Freezing Point Effect of solute (salt) on boiling/freezing point Effect of altitude on boiling point What is the Specific Heat of water and how does
this property relate to temperature moderation in coastal areas
Chemical properties of soap and how it works
Acids and Bases The pH Scale is based on [H+] Define acids, bases, and neutral solutions Use a pH Scale to gather information Compare the [H+], [OH-] and pH of acidic, basic,
and neutral solutions Explain how Buffers maintain the pH of a
solution Neutralization Reactions & calculations
Nuclear Chemistry (Preliminary) Radioactive isotopes are unstable atoms Repulsion of protons in the nucleus can cause
emissions of particles Alpha particles Beta particles Gamma Rays Depth of penetration Half-Life Decay definition and calculations
Format (estimated)70 Multiple Choice Questions2 Constructed Response References ProvidedPeriodic TableElectronegativity TableOrganic Chemistry Functional GroupsElectron Pair and Molecular Geometry Flow ChartSpecific Heat Capacity TablePhase Change Data for Water
Resources AllowedSelf-made, handwritten, reference sheet (1 side of an 8.5x11)
44. Using the diagram to the right: The arrow is pointing to the .
45. Why is the surface of the liquid curved?
46. The attraction between water molecules can be described as adhesion / cohesion.
47. What causes capillary action?
48. Explain how ponds cool and freeze.
49. As water at 6˚C is cooled, the density of the water increases / decreases.
50. As water at 6˚C is heated, the density of the water increases / decreases.
51. As water at 3˚C is cooled, the density of the water increases / decreases.
52. As water at 3˚C is heated, the density of the water increases / decreases.
53. Which phase of matter takes the shape of the container and does not have a defined volume?
54. Which phase of matter takes the shape of the container and does have a defined volume?
55. Which phase of matter does not take the shape of the container and does have a defined volume?
56. Which state of matter is least organized?
57. Define boiling point.
58. Define freezing point.
59. If you add sugar to water, what happens to the boiling point? Why?
60. If you add sugar to water, what happens to the freezing point? Why?
61. When you add energy to an unknown substance and its temperature changes a lot, the specific heat capacity is relatively high / low.
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62. In coastal areas the temperatures are more / less moderate than land-locked areas. Explain.
63. Complete the following formula for a temperature change:
q = ____ ____ ____
64. Complete the following formula for a phase change:
q = ____ ____
65. Determine the amount of heat required or amount of heat released when 20 grams of aluminum changes from 90˚C to 10˚C. (Note: Joules are a unit of heat energy similar to Calories)
66. Determine the specific heat capacity of a substance, which required 102 J of energy to raise its temperature by 10˚C when you have 10 g of it. (Note: Joules are a unit of heat energy similar to Calories)
67. Using the table to the right: Identify the substance from the previous question.______________
68. How much energy is required to raise the temperature of 50 grams of water at 70oC to steam at 115oC? (Note: Hv= 540 cal/g, the specific heat of water is 1 cal/goC, and the specific heat of steam is 0.5 cal/goC
69. How much energy is released when 10 grams of water cools from 20oC and freezes to -10oC?
Specific Heat Capacity Table
Substance Specific Heat Capacity at 25oC in J/goC
vegetable oil 2.000air 1.020
magnesium 1.020aluminum 0.900
glass 0.840iron 0.444
nickel 0.440zinc 0.39
copper 0.385brass 0.380sand 0.290silver 0.240
tin 0.21lead 0.160gold 0.129
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70. Soap has a polar / nonpolar head and a polar / nonpolar tail.
71. Which end of a soap molecule dissolves grease and grime?
72. Which end of the soap can be dissolved in water?
73. What is the pH of distilled water?
74. If [H+] is 1 × 10-6, what is the pH?________ Is the substance acidic, basic, or neutral?
75. If the pH of a substance is 12, what is the [H+]? ________ Is the substance acidic, basic, or neutral?
76. If [OH-] is 1 × 10-6, what is the pH? _______ Is the substance acidic, basic, or neutral?
77. In a neutral solution, there are more / less / the same concentration of H+ than OH-.
78. In an acidic solution, there are more / less / the same concentration of H+ than OH-.
79. In a basic solution, there are more / less / the same concentration of H+ than OH-.
80. Define buffers.
81. What volume of 0.5M HCl is required to Neutralize 100 mL of 1.0 M NaOH?
82. What is the concentration of MgOH solution if it required 1.0 L to neutralize 1.0 L of 0.25 M H2(SO4)?
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The following may or may not be on the Final…details to come.
83. If atoms have the same atomic number, but different mass numbers, those two atoms are of an element?
84. If an alpha particle is emitted, what is actually being emitted? Beta particle? Gamma ray?
85. Which type of radiation can be stopped by a sheet of paper? A piece of aluminum? Lead?
86. Why do some elements (especially above atomic number 83) radioactive?
87. You have 4 grams of beryllium-11. The half-life of beryllium-11 is 14 seconds. How much do you have left after 42 seconds?
88. What is the half-life of a substance if you have ¼ of it left after 5 seconds?
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Conceptual Chemistry Final Exam – Constructed Response Practice I
Susie would like to investigate how solubility changes as temperature changes. First, she put 100 g of water, at 0°C, in a beaker. While keeping the temperature of the water constant, she slowly added strontium bromide and stirred vigorously. Once she had added 90 g of strontium bromide, undissolved crystals remained on the bottom of the beaker. Susie filtered the mixture to reclaim the undissolved crystals, which she dried and found to have a mass of 5 g. Thus, 85 g of strontium bromide had dissolved.
Susie then heated the solution to 10°C. While stirring the solution, she added more of the strontium bromide. After adding 95 g of the ionic compound, she found that crystals remained undissolved. Following the same procedure as before, she reclaimed 2 g of crystals. Thus, 93 g of strontium bromide had dissolved.
Susie repeated the procedure while heating the solution in increments of 10°C. Her data table is shown here.
Temperature (°C) Solubility (g/100 g water)0 8510 9320 10230 11240 12350 13660 150
1. Construct a Solubility Curve for Strontium Bromide using Susie’s data with temperature as the independent variable and solubility as the dependent variable (remember your units!)
2. As you increase the temperature, the solubility of strontium bromide
3. Based on your graph, predict the solubility of the strontium bromide at 45°C.
4. Based on your graph, predict the temperature needed in order for 100 g of strontium bromide to fully dissolve.
5. What kind of solution formed each time the maximum amount of the compound was dissolved at a given temperature?
6. What kind of solution would be formed if Susie allowed the solution to cool from 30°C to 20°C?
7. Would the solution (described in previous question) be stable?
If you increase the temperature more / less strontium bromide would dissolve in water.
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Conceptual Chemistry Final Exam 2012 – Practice Constructed Response II
Jack is enjoying a beautiful Vermont evening making S’mores on the camp fire. Jack puts a 15 g metal skewer into the fire for 30 seconds to clean it. The metal gets hot and burns his hand when he tries to put the marshmallow on the stick. His friend, Jill, puts her 15 g skewer into the same part of the fire, but her skewer doesn’t reach as high a temperature, even though she did the same thing that Jack did! The only difference in their skewers is the metal in them.
Jack returns to school in the fall and is thankful that he is taking Conceptual Chemistry. He hopes to learn about why the he got burned, but Jill didn’t.
Upon return to school, Jack and Jill were pleased to learn that they would be studying the effect of specific heat capacities on heat energy, mass, and change in temperature. Jack and Jill both bring in their metal skewers to class to use in Jack’s investigation.
The temperature of the room is 15C. Jack & Jill both applied 945 J of energy to their skewers. The temperature of Jack’s skewer rose to 315C. When Jill applied 945 J of energy to her skewer, the temperature of hers rose to 85C.
Answer the following questions. Make sure to include units for your final answer.
1. What is the specific heat capacity of Jack’s metal?
2. What is the identity of Jack’s metal?
3. What is the specific heat capacity of Jill’s metal?
4. What is the identity of Jill’s metal?
5. Using the concept of specific heat capacity, explain why the temperature of Jack’s skewer changes more than Jill’s skewer. Use evidence from Part II.
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