EOCT Physical Science Chemical Properties of Matter
(EOCT_PhySci_Props_Matter)
1.
The more solute that can be dissolved in a solvent, the greater the solubility of the
A. solute.
B. solvent.
C. solution.
D. saturation.
2. What does it mean when a mixture is said to have reached saturation at a given
temperature and pressure?
A. A dilute solution has been formed.
B. There is more solute than solvent in the mixture.
C. As much solute as possible is dissolved in the solvent.
D. The solute and solvent have formed a heterogeneous mixture.
3.
Terry went for a walk several hours after a thunderstorm. He noticed a puddle of water
near the path and stirred it with a stick. The resulting muddy puddle was an example of
which of the following?
A. phase change
B. universal solvent
C. homogeneous mixture
D. heterogeneous mixture
4.
Jennifer has a flask of an unknown liquid. On close examination, she notices tiny
particles dispersed throughout the liquid. Which of the following is true?
A. It is a solution.
B. It is a pure substance.
C. It is a homogeneous mixture.
D. It is a heterogeneous mixture.
5.
Vinegar is a liquid solution containing acetic acid and water. It could be accurately
classified as which of the following?
A. a colloid
B. a compound
C. a homogeneous mixture
D. a heterogeneous mixture
6. Which process is represented by the following description: "sugar is added to
water and a sweet liquid results after stirring"?
A. melting
B. dissolving
C. evaporation
D. oxidation
7. What is the correct formula for the compound formed when lithium and oxygen
combine?
A.
B.
C.
D.
8. The water from hot springs near the Ebeko volcano in the Pacific Ocean has a very low
pH.
A low pH indicates which of the following about the water?
A. It has no detectable H_ or OH_ ions.
B. It has equal concentrations of H_ and OH_ ions.
C. It has high concentrations of H_ ions.
D. It has equal numbers of positive and negative ions.
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9. The table below shows the pH values of samples of substances.
According to the table, which of these substances is basic?
A. rainwater
B. drain cleaner
C. distilled water
D. soda water
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10. Many laboratory preparations of solutions call for stirring the solvent while adding
the solute. Which of the following is always an effect of this procedure?
A. It decreases the reactivity of the solute.
B. It decreases the solubility of the solute.
C. It brings the solute and solvent rapidly into contact.
D. It produces a double displacement reaction.
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11. The correct name for an aqueous solution of HCl is
A. chloric acid.
B. chlorous acid.
C. hydrochloric acid.
D. hydrogen chloride.
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Massachusetts Department of Education.
12. A student pours mineral salts into a bottle of cold water. Which of the following best
explains why shaking the bottle will affect the dissolving rate of the salt?
A. Shaking exposes the salts to the solvent more quickly.
B. Shaking helps more water to evaporate.
C. Shaking causes more ions to precipitate out of solution.
D. Shaking equalizes the water temperature.
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Massachusetts Department of Education.
13. The diagram below represents a sodium ion surrounded by several water molecules.
This diagram can be used to represent which of the following?
A. how sodium ions dissolve in water
B. how sodium is neutralized by water
C. how sodium metal makes bubbles in water
D. how sodium ions precipitate out as a solid in aqueous solution
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14. An unbalanced chemical equation is shown below.
What are the coefficients of the balanced equation?
A. 2:1:3
B. 2:2:3
C. 3:1:2
D. 3:2:2
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Massachusetts Department of Education.
15. Concrete is composed of Portland cement, rocks, sand, and water. Which of the
following best describes concrete?
A. an element
B. a compound
C. a homogenous mixture
D. a heterogeneous mixture
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Massachusetts Department of Education.
16. Which of the following substances has the highest concentration of hydrogen ions in
solution?
A. bleach – pH 13
B. water – pH 7
C. tomato juice – pH 4
D. vinegar – pH 3
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Massachusetts Department of Education.
17. Three 10 g samples of sugar are represented below.
Sample A dissolves in water more slowly than sample B. Sample B dissolves more
slowly than sample C. Which of the following best explains why sample A dissolves
most slowly?
A. It has the most volume.
B. It has the smallest surface area.
C. It has the largest number of sugar molecules.
D. It has the fewest bonds between sugar molecules.
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Massachusetts Department of Education.
18. Oxygen (O) atoms have six valence electrons and beryllium (Be) atoms have two
valence electrons. Which of the following is the correct formula for a compound made of
oxygen and beryllium?
A. BeO
B. BeO2
C. BeO2
D. BeO26
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Massachusetts Department of Education.
19.
During a physical science activity you are required to make a saturated solution of
sodium sulfate (Na2SO4) in water. At what temperature are you most likely to make such
a solution?
A. 0oC
B. 40oC
C. 125oC
D. 200oC
20.
During science lab, several students discovered that iodine dissolved readily in ethanol.
In this case, the ethanol would be classified as the
A. alloy.
B. solute.
C. solution.
D. solvent.
21.
You are given 100 ml of 20oC water at standard atmospheric pressure containing 0.16
grams of carbon dioxide gas. What should you do to INCREASE the amount of carbon
dioxide dissolved in this solution?
A. Decrease the temperature.
B. Increase the temperature.
C. Decrease the pressure.
D. Stir the solution.
22.
When making a solution of sugar and water, you begin with a 500 ml beaker, 10 grams of
sugar, and 400 ml of distilled water. Which procedure will allow you to dissolve the
MOST sugar in the LEAST amount of time?
A. Pour the sugar and water in the beaker.
B. Pour the sugar and water in the beaker and stir.
C. Pour the sugar and water in the beaker, stir, and heat over a hot plate.
D. Pour the sugar and water in the beaker, stir, and place the beaker in an ice bath.
23.
Which of these solutes, when dissolved in water, will ionize and form a solution that
conducts electricity?
A. O2
B. CH4
C. CaCl2
D. C6H12O6
24.
Based on the graph, the solubility of ______________ is LEAST influenced by an
increase in temperature.
A. Ba(NO3)2
B. NaCl
C. Na2HAsO4
D. Na2SO4
25.
Certain substances, when dissolved in water, produce ions in solution. Such substances
are called
A. electrolytes.
B. elements.
C. molecules.
D. nonpolar.
26.
Ammonia is a common base used in household cleaners. Which is a characteristic of a
base?
A. pH < 7
B. pH = 7
C. produces OH- in solution
D. turns blue litmus red
27.
During science lab, students were asked to test a variety of common household
substances and classify them as: acid, base, or neutral. Tests on shampoo produced the
following results.
felt slippery
pH 8.5
turned red litmus blue
These results indicate
A. shampoo is an acid.
B. shampoo is a base.
C. shampoo is neutral.
D. there is insufficient information to classify shampoo.
28.
Based on the graph, which compound is MOST soluble at 35oC?
A. Ba(NO3)2
B. NaCl
C. Na2HAsO4
D. Na2SO4
29.
White gold is actually an alloy of three metals:
85% gold
10% nickel
5% zinc
In this case, the solvent would be
A. gold.
B. nickel.
C. water.
D. zinc.
30.
The correct chemical formula for magnesium fluoride is
A. MgF.
B. Mg2F.
C. MgF2.
D. Mg7F2.
31.
The correct chemical formula for aluminum (Al+3) plus chlorine (Cl-1) is
A. AlCl.
B. AlCl3.
C. Al3Cl1.
D. Al3Cl.
32.
The correct name for the binary compound, Na2O, is
A. sodium oxide.
B. sodium oxygen.
C. disodium oxide.
D. disodium monoxide.
33.
The correct name for the binary compound, MgCl2, is
A. magnesium(II) chloride(I).
B. magnesium dichloride.
C. magnesium chlorine.
D. magnesium chloride.
34.
What is the correct name for the covalent compound CCl4?
A. carbon chloride
B. carbon tetrachloride
C. monocarbon chloride
D. monocarbon tetrachloride
35.
During science lab, Mr. Smith's students tested the reactivity of various metals in sulfuric
acid. When zinc was added to sulfuric acid, bubbles were produced, a sure sign that a
chemical reaction had taken place. Based on the law of conservation of matter, if 30
grams of zinc are added to 45 grams of sulfuric acid to produce just 1 gram of hydrogen
gas, how much zinc sulfate would also be produced? The formula for the chemical
reaction is as follows:
Zn + H2SO4 ZnSO4 + H2
A. 15 grams
B. 30 grams
C. 45 grams
D. 74 grams
36.
Which of these equations correctly represents a balanced synthesis reaction?
A. Na + Cl NaCl
B. 2Na + Cl2 2NaCl
C. NaOH + HCl NaCl + HOH
D. 2Na + O Na2O
37.
Hydrogen peroxide decomposes to form water and oxygen. This reaction is represented
by which of these balanced equations?
A. H2O2 H2O + 2O
B. H2O + O2 H2O2
C. 2H2O2 2H2O + O2
D. 2H2O2 2H2O + 2O
38.
In Antoine Lavoisier's classic experiment, mercuric (II) oxide is heated in a sealed
container. The solid red powder is changed into silver liquid mercury and oxygen gas. If
Lavoisier heated 50 grams of powdered mercuric oxide to produce 46.5 grams of liquid
mercury, how much oxygen would be released?
A. 3.5 grams
B. 16 grams
C. 32 grams
D. 96.5 grams
39.
Name the following compound:
N2O5
A. nitrous oxide
B. nitrogen oxide
C. nitrogen pentoxide
D. dinitrogen pentoxide
40.
Aluminum oxide decomposes to produce aluminum plus oxygen gas. Identify the
balanced equation for this decomposition reaction.
A. Al2O3 2Al + 3O
B. Al2O3 2Al + 3O2
C. 2Al2O3 4Al + 3O2
D. 4Al + 3O2 2Al2O3
41.
The coefficients of the correctly balanced equation for the reaction illustrated above
are —
A. 1, 1, 1.
B. 1, 1, 2.
C. 2, 1, 2.
D. 2, 2, 1.
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42. Soda water is a solution of carbon dioxide in water. This solution is composed of
a—
A. gaseous solute in a gaseous solvent
B. liquid solute in a liquid solvent
C. gaseous solute in a liquid solvent
D. liquid solute in a gaseous solvent
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43. The formula for lithium nitride is —
A.
B.
C.
D.
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44.
Which of the following aqueous solutions will cause litmus paper to turn red?
A. NaOH
B. NaCl
C. HCl
D. H2O
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45.
What type of reaction does this illustration represent?
A. Decomposition
B. Synthesis
C. Single-replacement
D. Double-replacement
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46. When
is heated in a crucible, there is a loss of water. How should a
student determine the amount of water lost?
A. Subtract the mass of the
from the mass of
B. Subtract the mass of the
C. Add the masses of
D. Multiply the masses of
from the mass of
and
and
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47. A balanced chemical equation has equal numbers of atoms of each type on both
sides of the equation. This illustrates the principle of —
A. conservation of energy
B. conservation of mass
C. action and reaction
D. natural selection
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48. The appropriate model for a decomposition reaction is —
A.
B.
C.
D.
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49. What is represented by the pH of a solution?
A. Partial pressure of hydrogen ions in the solution
B. Electronegativity of dissociated hydrogen ions in the solution
C. Concentration of hydrogen ions in the solution
D. Temperature of hydrogen ions in the solution
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50. The formula for dinitrogen tetroxide is —
A.
B.
C.
D.
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51.
When the above equation is balanced, the coefficient of the hydrochloric acid will be
—
A. 2.
B. 3.
C. 4.
D. 6.
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52. The correct name for
—
A. phosphorus (V) pentoxide.
B. phosphorus oxide.
C. phosphorus (II) oxide.
D. diphosphorus pentoxide.
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53.
Which pair of solutions would be acidic if mixed in equal quantities?
A. A and B
B. B and C
C. B and D
D. C and D
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54. Which of the following is a mixture?
A. Carbon
B. Glucose
C. Distilled water
D. Air
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55.
Which type of reaction is represented here?
A. Single replacement
B. Double replacement
C. Synthesis
D. Decomposition
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56. The correct formula for copper (I) bromide is —
A.
B.
C.
D.
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Answer Key
1. A) solute.
2. C) As much solute as possible is dissolved in the solvent.
3. D) heterogeneous mixture
4. D) It is a heterogeneous mixture.
5. C) a homogeneous mixture
6. B) dissolving
7. B)
8. C) It has high concentrations of H_ ions.
9. B) drain cleaner
10. C) It brings the solute and solvent rapidly into contact.
11. C) hydrochloric acid.
12. A) Shaking exposes the salts to the solvent more quickly.
13. A) how sodium ions dissolve in water
14. A) 2:1:3
15. D) a heterogeneous mixture
16. D) vinegar – pH 3
17. B) It has the smallest surface area.
18. A) BeO
19. B) 40oC
20. D) solvent.
21. A) Decrease the temperature.
22. C) Pour the sugar and water in the beaker, stir, and heat over a hot plate.
23. C) CaCl2
24. B) NaCl
25. A) electrolytes.
26. C) produces OH- in solution
27. B) shampoo is a base.
28. C) Na2HAsO4
29. A) gold.
30. C) MgF2.
31. B) AlCl3.
32. A) sodium oxide.
33. D) magnesium chloride.
34. B) carbon tetrachloride
35. D) 74 grams
36. B) 2Na + Cl2 2NaCl
37. C) 2H2O2 2H2O + O2
38. A) 3.5 grams
39. D) dinitrogen pentoxide
40. C) 2Al2O3 4Al + 3O2
41. D) 2, 2, 1.
42. C) gaseous solute in a liquid solvent
43. B)
44. C) HCl
45. A) Decomposition
46. A) Subtract the mass of the
from the mass of
47. B) conservation of mass
48. A)
49. C) Concentration of hydrogen ions in the solution
50. A)
51. D) 6.
52. D) diphosphorus pentoxide.
53. A) A and B
54. D) Air
55. B) Double replacement
56. A)