Chemistry I SOL Practice Test — Set 2 of 6

Set 2 of 6 — 50 more free Chemistry I SOL practice questions from official VDOE released tests.

1. 1. Iodine-131 is a radioactive isotope with a half-life of 8 days. How many grams of a 64 g sample of iodine-131 will remain at the end of 24 days?

   A56 gB48 gC32 gD8 g
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   Answer: D — 8 g

2. 2. Which of the following is the correct name for the compound MnF₃?

   AManganese fluoride(III)BManganese(III) fluorideCManganese(I) fluoride(III)DManganese(III) fluoride(II)
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   Answer: B — Manganese(III) fluoride

3. 3. The name of the salt formed by the neutralization of hydrochloric acid and sodium hydroxide is—

   Asodium chlorideBsodium chlorateCsodium chloriteDsodium hypochlorite
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   Answer: A — sodium chloride

4. 4. If the quantity of heat lost or gained is ΔH = mass × change in temperature × specific heat, what is the amount of heat required to raise 200.0 g of water from 22.0°C to 100.0°C? The specific heat of water is 4.180 J/(g·°C).

   A652.1 JB6,521 JC65,210 JD652,100 J
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   Answer: C — 65,210 J

5. 5. For the equation Mg(OH)₂ + HCl → MgCl₂ + H₂O the coefficients necessary to balance the equation correctly are—

   Aa = 2, b = 1, c = 1, d = 2Ba = 1, b = 2, c = 1, d = 2Ca = 1, b = 1, c = 1, d = 1Da = 2, b = 2, c = 1, d = 1
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   Answer: B — a = 1, b = 2, c = 1, d = 2

6. 6. A balloon is filled with 3.8 L of helium gas at STP. Approximately how many moles of helium are contained in the balloon?

   A0.17 molB0.26 molC72 molD85 mol
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   Answer: A — 0.17 mol

7. 7. Which of these elements has the smallest atomic radius?

   ABeryllium (Be)BOxygen (O)CSodium (Na)DSulfur (S)
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   Answer: B — Oxygen (O)

8. 8. If 250.0 mL of a 0.96 M solution of acetic acid (C₂H₄O₂) is diluted to 800.0 mL, what will be the approximate molarity of the final solution?

   A0.19 MB0.24 MC0.30 MD0.77 M
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   Answer: C — 0.30 M

9. 9. An atom contains 70 protons, 70 electrons, and 99 neutrons. What is the mass number?

   A239B169C140D70
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   Answer: C — 140

10. 10. Which set of equipment would be most useful to determine the density of a liquid?

    ABalance and periodic tableBPeriodic table and thermometerCBalance and graduated cylinderDGraduated cylinder and thermometer
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    Answer: C — Balance and graduated cylinder

11. 11. Sodium chloride conducts electricity when dissolved in water. What type of bond is present in NaCl?

    ANonpolar covalentBPolar covalentCHydrogenDIonic
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    Answer: D — Ionic

12. 12. A mixture is poured through filter paper in a funnel into a test tube, separating solid particles from a liquid. Which of the following substances is least likely to pass through the filter paper into the test tube?

    ADissolved gasesBDissolved saltsCLiquid solventsDSolid particles
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    Answer: D — Solid particles

13. 13. Which of the following represents the Lewis dot diagram of ammonia (NH₃), showing nitrogen as the central atom with three single bonds to hydrogen and one lone pair of electrons on nitrogen?

    AH–N–H with one lone pair on nitrogen and a third H bonded to NBH–H–N–H with no lone pairsCN bonded to three H atoms with no lone pairDH–N–H with two lone pairs on nitrogen
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    Answer: A — H–N–H with one lone pair on nitrogen and a third H bonded to N

14. 14. After 1911, most scientists accepted the theory that the nucleus of an atom was very dense, very small, and had a positive charge. What led scientists to accept this theory?

    ADalton’s theory of the atom was over 100 years old.BScientists before 1911 used the scientific method improperly.CA new model proved that quantum theory was inaccurate.DRutherford fired alpha particles at a thin sheet of gold foil.
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    Answer: D — Rutherford fired alpha particles at a thin sheet of gold foil.

15. 15. A sodium atom has an electron configuration of 1s² 2s² 2p⁶ 3s¹. If the sodium atom becomes ionized, its new electron configuration will be the same as which element?

    ALithiumBNeonCMagnesiumDPotassium
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    Answer: B — Neon

16. 16. Which reaction is correctly balanced?

    AFe₂ + CuSO₄ → FeSO₄ + CuBFe + CuSO₄ → FeSO₄ + CuC2Fe + CuSO₄ → 2FeSO₄ + CuDFe + 2CuSO₄ → 2FeSO₄ + Cu
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    Answer: B — Fe + CuSO₄ → FeSO₄ + Cu

17. 17. Which of the following particles has a positive one (+1) charge?

    AAlpha particleBElectronCNeutronDProton
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    Answer: D — Proton

18. 18. What is the mass of one mole of CO₂?

    A24 gB28 gC44 gD56 g
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    Answer: C — 44 g

19. 19. According to the periodic table, magnesium will most likely react with elements in which group?

    AGroup 1BGroup 2CGroup 17DGroup 18
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    Answer: C — Group 17

20. 20. A sample of gas is enclosed in a cylinder with a movable piston. If the temperature is kept constant and the piston moves downward, decreasing the volume, the pressure increases because the gas particles—

    AexpandBlose velocityCbecome smallerDcollide more frequently with the container walls
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    Answer: D — collide more frequently with the container walls

21. 21. Which of the following shows the correct number of atoms of each element in the formula Mg(NO₃)₂?

    A1 magnesium atom, 2 nitrogen atoms, and 6 oxygen atomsB1 magnesium atom, 2 nitrogen atoms, and 5 oxygen atomsC1 magnesium atom, 1 nitrogen atom, and 6 oxygen atomsD1 magnesium atom, 1 nitrogen atom, and 5 oxygen atoms
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    Answer: A — 1 magnesium atom, 2 nitrogen atoms, and 6 oxygen atoms

22. 22. A student is given a container of potassium nitrate crystals. To determine the exact mass of the potassium nitrate using a triple-beam balance, the student must know—

    Athe mass of the filled container and the chemical formulaBthe mass of the filled container and the densityCthe volume of the filled container and the volume of the crystalsDthe mass of the empty container and the mass of the filled container
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    Answer: D — the mass of the empty container and the mass of the filled container

23. 23. Carbon has two naturally occurring isotopes: C-12 (98.89%) and C-13 (1.108%). Which calculation should be used to determine the atomic mass of carbon?

    A(12 × 0.01108) + (13 × 0.9889)B(12 × 0.9889) − (13 × 0.01108)C(12 × 0.9889) + (13 × 0.01108)D(12 × 0.9889)
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    Answer: C — (12 × 0.9889) + (13 × 0.01108)

24. 24. AB + energy → A + B The general equation shown represents a reaction that is—

    Aexothermic decompositionBendothermic decompositionCendothermic synthesisDexothermic synthesis
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    Answer: B — endothermic decomposition

25. 25. A graph shows temperature on the vertical axis and heat added on the horizontal axis. Between point X and point Y, heat is added but the temperature remains constant. What most likely happens as the compound is heated from point X to point Y?

    AThe phase of the compound changes.BThe mass of the compound increases.CThe molecules lose potential energy.DThe molecules break apart into atoms.
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    Answer: A — The phase of the compound changes.

26. 26. To determine the identity of a substance, a student lists several properties. Which of the following is a chemical property?

    AOxidizes in airBConducts an electric currentCAttraction to a magnetDDissolves in water
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    Answer: A — Oxidizes in air

27. 27. A study lists properties of water and includes a graph showing vapor pressure (in mm Hg) on the vertical axis versus temperature (°C) on the horizontal axis from 0°C to 100°C. What is the independent variable in the study?

    AMolar massBMelting pointCVapor pressureDTemperature
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    Answer: D — Temperature

28. 28. Which of the following is a solid–solid solution?

    AAn alloy of gold and copperBA mixture of argon and kryptonCA strongly electrolytic acidDA neutralized base
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    Answer: A — An alloy of gold and copper

29. 29. Which of these compounds is most likely to contain an ionic bond?

    ACO₂BH₂OCNH₃DNaCl
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    Answer: D — NaCl

30. 30. Dry air is approximately 78% nitrogen, 21% oxygen, and 1% other gases. What is the partial pressure of nitrogen at standard atmospheric pressure (101.3 kPa)?

    A21.0 kPaB79.0 kPaC101.3 kPaD760.0 kPa
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    Answer: B — 79.0 kPa

31. 31. A gas has a volume of 100.0 mL at a pressure of 600.0 mm Hg. If the temperature is constant, what is the volume at 800.0 mm Hg?

    A33.33 mLB66.67 mLC75.00 mLD133.0 mL
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    Answer: C — 75.00 mL

32. 32. Which solution has the greatest concentration?

    A2.0 moles of solute in 1.0 L of solutionB0.3 mole of solute in 0.6 L of solutionC2.0 moles of solute in 10.0 L of solutionD0.1 mole of solute in 0.5 L of solution
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    Answer: A — 2.0 moles of solute in 1.0 L of solution

33. 33. Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag This chemical equation is an example of a—

    Asynthesis reactionBdecomposition reactionCdouble-replacement reactionDsingle-replacement reaction
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    Answer: D — single-replacement reaction

34. 34. Which element is a noble gas?

    AFluorine (F)BHydrogen (H)CNitrogen (N)DXenon (Xe)
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    Answer: D — Xenon (Xe)

35. 35. To determine if a reaction is exothermic, a student should use a—

    ApH probeBmotion sensorCpressure sensorDtemperature probe
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    Answer: D — temperature probe

36. 36. What is the name of NH₄OH?

    AAmmonium hydroxideBNitrogen hydroxideCNitrogen oxygen hydrideDAmmonium oxygen hydride
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    Answer: A — Ammonium hydroxide

37. 37. A student hypothesizes that the solubility of a solute in water is nearly constant as temperature varies. Which procedure best tests this hypothesis?

    AResearch properties of many solutesBMeasure solubility at five different temperaturesCDraw molecular diagramsDMeasure solubility of different solutes at one temperature
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    Answer: B — Measure solubility at five different temperatures

38. 38. ? P +? Br₂ →? PBr₃ Which set of coefficients balances this equation?

    A3, 1, 1B2, 3, 2C3, 2, 3D2, 6, 2
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    Answer: B — 2, 3, 2

39. 39. The table below shows volume and pressure of a gas at constant temperature. Volume (m³): 0.3, 0.4, 0.5, 0.8, 1.0 Pressure (kPa): 498, 409, 247, 203, 150 After graphing the data, the volume is—

    Adirectly proportional to pressureBdirectly proportional to pressure squaredCinversely proportional to pressure squaredDinversely proportional to pressure
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    Answer: D — inversely proportional to pressure

40. 40. What is the correct name for the compound P₄O₆?

    APhosphoric acidBPhosphorus oxideCPhosphorus(IV) oxideDTetraphosphorus hexoxide
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    Answer: D — Tetraphosphorus hexoxide

41. 41. 2Fe(s) + O₂(g) → 2FeO(s) This reaction is classified as—

    AsynthesisBdecompositionCsingle replacementDdouble replacement
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    Answer: A — synthesis

42. 42. As heat is added to a substance undergoing a phase change, the temperature remains constant because the energy is used to—

    Abreak covalent bondsBlower specific heatCovercome intermolecular forcesDoppose electron cloud repulsion
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    Answer: C — overcome intermolecular forces

43. 43. 2Na + 2H₂O → 2NaOH + H₂ How many moles of hydrogen gas are produced when 0.066 mol of sodium reacts completely?

    A0.022 molB0.033 molC0.066 molD0.099 mol
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    Answer: B — 0.033 mol

44. 44. The accepted value for the specific heat of aluminum is 0.897 J/(g·°C). Which set of experimental values shows the greatest accuracy and precision?

    A0.847, 0.847, 0.848B0.896, 0.899, 0.896C0.897, 1.04, 1.03D0.936, 0.876, 0.879
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    Answer: B — 0.896, 0.899, 0.896

45. 45. A 1.0 M aqueous solution of which substance would have the lowest pH?

    ANH₃BHClCBa(OH)₂DNaF
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    Answer: B — HCl

46. 46. What is the chemical formula for iron(II) phosphide?

    AFe₃PBFe₃P₂CFeP₂DFe₃P₂
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    Answer: D — Fe₃P₂

47. 47. In a mixture of oxygen (O₂) and nitrogen (N₂), nitrogen exerts 80.0% of the total pressure. If the total pressure is 2.0 atm, what pressure is exerted by oxygen?

    A0.20 atmB0.40 atmC0.80 atmD1.6 atm
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    Answer: B — 0.40 atm

48. 48. 2H₃PO₄ + 3Mg(OH)₂ → Mg₃(PO₄)₂ + 6H₂O How many moles of water are produced when 0.24 mol of H₃PO₄ is neutralized?

    A0.24 molB0.48 molC0.72 molD1.44 mol
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    Answer: C — 0.72 mol

49. 49. A student measures the mass of a 1.00 g aluminum rod as 0.99 g. The best estimate of the percent error associated with this measurement is —

    A0.01%B0.1%C1%D10%
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    Answer: C — 1%

50. 50. The most efficient way to determine whether a reaction is an exothermic chemical reaction is to use —

    Aan oxygen probeBa temperature probeCa pressure probeDa pH probe
    Show answer

    Answer: B — a temperature probe

Practice items adapted from Virginia Department of Education released SOL tests. Practice items are provided for study purposes and are not affiliated with or endorsed by the Virginia Department of Education.