School Science Constructed Response
Earth Science Constructed Response
1.
Explain how the water table changes during times of heavy rain and drought. Sketch a simple
diagram and label zone of saturation, zone of aeration, and water table. (EEn.2.3.2)
Answer: During heavy rain, the water table rises because the water fills in all the empty spaces
underground. During a drought, the water table would go down because no new water is being added to
the aquifer, while water might still be being depleted by human use, plants, etc.
Simple diagram with ZOA, ZOS, and WT labeled:
2.
Explain the difference in permeability in a container of large, even sized particles vs. a container
of all different sized particles. (EEn.2.3.2)
Answer: Permeability describes how fast water can flow through an aquifer. If all the rocks were large
and of equal size, there would be a lot of open pore space in between where they don’t fit together. This
would allow water to flow through quickly. If there were many particles of various sizes, the smaller
pieces would fit in the holes left by the bigger pieces, which would decrease the overall open pore space
available for water to flow through. This would lead to lower permeability. So overall, the container with
large, evenly sized particles would have a greater permeability than the container with all different
sizes/shapes.
3.
Describe a real-world example of physical (a.k.a. mechanical) weathering. (EEn.2.1.3)
Answer: Some possible examples of real-world physical/mechanical weathering:
 Water gets into a crack in rock, freezes, expands, and causes the rock to break down further.
 The movements of water and wind can expose rocks to friction and abrasion from other
rocks, particles and surfaces, causing them to break apart.
 Growing plants or tree roots work their way into soil and break rocks apart further
 Other examples are possible!
4.
Describe how sand dunes form on the Outer Banks of NC. Draw a simple diagram if that helps
your description. (EEn.2.1.3)
Answer: Sand dunes form by the action of wind. The wind blows grains of sand on one side of the sand
dune onto the opposite side, or slip face. Unstable accumulation of sand builds up on the slip face.
Accumulation cascades down to the base, advancing the sand dune. A few simple diagrams:
5.
How can groundwater become polluted by something happening at Earth’s surface? Give a
specific example. (EEn.2.4.2)
Answer: If oil is spilled on Earth’s surface, it can seep into the groundwater by sinking through the pore
spaces in the soil until it reaches the zone of saturation. Fertilizer is another example of something that
may be used on the surface, but it could also seep into an aquifer. Essentially any harmful chemical
polluted on the surface has the potential of entering the groundwater if the soil/rock is permeable. Look at
this photo for more potential examples:
6.
List one alternative energy. Explain how that energy would reduce carbon dioxide, CO2 in our
atmosphere. How does that alternative energy source create electricity? (E.E. 2.8)
Answer:
Wind, hydroelectric, solar, biofuels



Reduce plant/factory emissions
Less use of fossil fuels leads to less extraction and depletion of fossil fuels
Reduction of transportation and import/export of fossil fuels
Wind creates power by windmills, turning the turbines that turns the generator
Solar can be harvested in solar panels
Water can be harvested in dams, water turning the turbines that turn the generator
7.
Identify what type of pressure system a hurricane is classified as. Describe two wind movements
seen in that type of pressure system (E.E. 2.5 )
Answer:
Low pressure system
Wind moves counter clockwise; inward; convergence at surface; rises at the eye; divergence aloft;
Coriolis effect causes wind to deflect to the right in the northern hemisphere
Chemistry Constructed Response
1.
A. State the period trend for atomic radius.
(Chm.1.3.2)
B. State the family trend for atomic radius.
C. Explain either the period or family trend in atomic radius using the following terms:
Electronegativity, Energy Levels, and Proton pull.
D. Explain either of the following statements below using the trends seen in the periodic table
(electronegativity, ionization energy, and atomic radius)
I. Fluorine is the most reactive nonmetal in the periodic table.
II. Francium is the most reactive metal in the periodic table.
2.
A. Write the Noble Gas electron configuration for Bromine (Br).
(Chm.1.3.2)
B. Draw an orbital diagram to match your Noble Gas configuration.
C. Explain using your configuration or orbital diagram what Bromine will do to become stable.
D. Which is larger: Bromine’s atomic radius or Bromine’s ionic radius. Explain your answer.
3. In the lab your class heated several different types of metals in boiling water. The hot metals were then
placed into a calorimeter containing room temperature water. The metal and water reached the same
temperature when together inside the calorimeter. (Chm.2.1.4)
A. Describe the flow of energy (called heat) within the calorimeter.
B. The temperature change of the metal was seen to be much greater than the temperature change
of the water within the calorimeter. Explain why.
C. Explain how knowing how much energy the water gained allowed us to calculate the specific
heat of the metal using q = mCp∆T.
4.
(Chm.1.1.4)
A. Write and balance the following nuclear equation: Sn-120 undergoes alpha emission.
B. Explain why we must balance all equations.
5.
(Chm.1.1.3)
A. An electron transitions from n=6 to n=2. What wavelength of EM radiation is emitted (in
nanometers (nm))?
B. An electron transitions from n=4 to n=1. What wavelength of EM radiation is emitted (in
nanometers (nm))?
C. Which transition (A or B) released a wave with more energy? Defend your answer by
comparing the wavelength and frequency of the 2 waves released.
6. The phase change diagram for a substance is provided below. (Chm.2.1.3 & Chm.2.1.2)
A. What is the boiling point of the substance?
B. Explain why there is no temperature change between points B-C and D-E.
C. What phase of matter is the substance at time =12 min?
7. Acids (you could also use bases here) are solutions with specific characteristics (Chm.3.2.2)
 Describe the chemical reaction which occurs between a nonmetal and water (if you do acidmetal with water if you do base)
 If Sulfur dioxide gas in the atmosphere combines with water, which product would result in
this chemical reaction? (if you do base – “If sodium metal is added to water, which product would
result in this chemical reaction?)
*This can be changed to match any bullet under the chemical reactions section of the reference table
8. A 2 M solution of CaF2 is made by dissolving CaF2 in enough water to make a 0.54 L. (Chm.3.2.3)
A. How many grams of CaF2 were dissolved to make the solution? Show your work.
B. Describe how (increasing, decreasing) the volume would affect the Molarity of the solution.
C. Describe how (increasing, decreasing) the mass of the solute would affect the Molarity of the
solution.
9. During a laboratory experiment, 75 grams of water @ 0oC is transformed into liquid @ 0oC.
(Chm.2.1.1)
A. Describe how this experiment confirms the law of conservation of energy.
B. How much heat energy is needed to completely change the state of the water? Show your work.
10. A 2 L container of hydrogen gas @ 27oC sits in a chemistry lab. (Chm.2.1.5)
A. Convert 27oC into Kelvin. Show your work.
B. Calculate the pressure of the hydrogen gas within the container.
C. Describe the change in pressure if the temperature is increased. (or decreased)
12. 30mL of 0.1 M NaOH solution is added to 15mL of an unknown concentration of HCl during a
titration before the endpoint is reached. Phenolphthalein is added to the HCl solution before beginning the
titration. (Chm.3.2.3)
A. Calculate the molarity of the HCl solution. Show your work.
B. Calculate the original pH of the NaOH (or HCl) solution. Show your work.
C. Describe the change in the HCl solution as the endpoint is reached.
D. Explain what happens to the hydrogen and hydoxide ions during the titration.
E. Describe the concentrations of the hydrogen and hydroxide ions at the endpoint.
13. Using sodium hydroxide is combined with carbonic acid: (Chm.2.2.2)
A. Predict the products and write the balanced equation, including the states of matter
B. Write the type of reaction
C. Explain the products states of matter
Answer:
A. 2NaOH(aq)+H2CO3
2CO3(aq)
+ 2 H2O(l)
B. This is a double replacement reaction
C. The sodium carbonate product is soluble and water is produced in its liquid state.
14. When barium chloride is combined with potassium sulfate, the resulting solution(s) have distinct
characteristics. (Chm.2.2.2)
A. Predict the products and write the balance equation
B. Describe the reaction and any state changes involved with this reaction.
Answer:
A. BaCl2 (aq)+K2SO4
4 (s)+ 2KCl(aq)
B. This is a double replacement reaction that produces solid barium sulfate as a precipate.
15. A uniformly made cylinder is filled with 16 liters of carbon dioxide at STP. If the temperature is
doubled, explain using the laws of chemistry what happens and prove it mathematically. .
(Chm.2.1.5)
Answer: Standard temperature is 25 C and standard pressure is 1 atm. Using the ideal gas law
PV=nRT we realize that we generally only vary one component at a time. Using P1 V 1=P2 V2,
Boyle’s
Law, we can prove the new pressure will be 2 atm.
Physical Science Constructed Response
1. List and describe three ways to increase the rate at which a substance dissolves. (PSc.2.1.2)
Answers: increase surface area, stirring, heat
2. Give the differences between a heterogeneous and homogenous mixture and give an example of each.
(PSc.2.1.1)
Answer: Heterogeneous different throughout, homogenous same throughout
Trail mix (hetero). Tea (homo)
3. (PSc.2.2.4 & PSc.2.1.3 & PSc.2.2.5)
A. Balance the chemical equation that takes place in fireworks
KClO4 KCl + O2
B. Describe two pieces of evidence that a chemical reaction has occurred during a fireworks display.
C. Identify the type of chemical reaction
Answer:
A. KClO4 KCl + 2O2
B. Light given off, you can not go back to the reactants after the reaction is complete
C. decomposition
4. Billy Bob Hoehandle runs from his house to the store and back to get a mountain dew. The distance to
the store is three miles from his house. (PSc.3.1.3)
A. Describe the difference in distance and displacement of his trip to the store.
B. Give a numerical value for the distance
C. Give a numerical value for the displacement
Answer: Distance is the total amount of miles traveled. 6 miles
Displacement is the distance from the start to the finish. 0 miles
5. List and describe the three types of heat transfer. Give an example of each. (PSc.3.1.1)
Answer: conduction - direct contact, pot on a stove
Radiation- Heat by waves, sun light
Convection- Heat flow by density differences, hot air balloon rising
6. Describe what type of phase changes a water molecule goes through at points A,B,C,D, and E on the
phase change graph. (PSc.3.1.1 & PSc.2.1.2)
Answers:
A- solid
B- heat of fusion
C- liquid
D-heat of vaporization
E- gas
Physics Free Response Question
1. A hallow cylinder and a solid cylinder having the same mass and diameter are released from rest
simultaneously at the top of an inclined plane. ( Phy.1.2)
A. Which reaches object reaches the bottom first?
B. Explain your answer to A
C. Would the results be different if two spheres would be used rather than cylinders?
Answers:
A. the objects would reach the bottom at the same time
B. law of gravity
C. it does not matter if you change the objects, they would both reach the bottom at the same
time.