name: regents practice exam 2 2016

Name: Regents Practice Exam 2 2016

A) +1 B) +2 C) 0 D) –1

1. A neutron has a charge of

A) alpha particle B) beta particleC) neutron D) proton

2. Which particle has the least mass?

A) each atom in the sample has 29 protonsB) atoms in the sample react with oxygenC) the sample melts at 1768 KD) the sample can conduct electricity

3. A sample of matter must be copper if

A) charge of an electronB) conductivity of an electronC) location of an electronD) mass of an electron

4. In the electron cloud model of the atom, an orbital isdefined as the most probable

A) atomic number B) mass numberC) number of isotopes D) number of moles

5. The elements on the Periodic Table are arranged inorder of increasing

A) tantalum B) rheniumC) osmium D) hafnium

6. Which element has the highest melting point?

A) energy, volume, and massB) energy, volume, and chargeC) mass, charge, and energyD) mass, charge, and volume

7. In a chemical reaction, there is conservation of

A) the same crystal structure and the sameproperties

B) the same crystal structure and differentproperties

C) different crystal structures and the sameproperties

D) different crystal structures and differentproperties

8. At STP, both diamond and graphite are solidscomposed of carbon atoms. These solids have

A) 1.0 g B) 4.8 g C) 48 g D) 480 g

9. The gram-formula mass of a compound is 48 grams.The mass of 1.0 mole of this compound is

A) A bond is broken as energy is absorbed.B) A bond is broken as energy is released.C) A bond is formed as energy is absorbed.D) A bond is formed as energy is released.

10. Given the balanced equation representing a reaction:Cl2 Cl + ClWhat occurs during this reaction?

A) Cl atom B) F atomC) O atom D) S atom

11. Which atom has the weakest attraction for theelectrons in a bond with an H atom?

A) ammonia B) mercuryC) propane D) water

12. Which substance can not be broken down by achemical change?

A) Both the boiling point and the freezing point ofNaCl(aq) are lower.

B) Both the boiling point and the freezing point ofNaCl(aq) are higher.

C) The boiling point of NaCl(aq) is lower, and thefreezing point of NaCl(aq) is higher.

D) The boiling point of NaCl(aq) is higher, andthe freezing point of NaCl(aq) is lower.

13. At standard pressure, how do the boiling point andthe freezing point of NaCl(aq) compare to theboiling point and the freezing point of H20(l)?

A) average kinetic energy of its particlesB) average potential energy of its particlesC) total kinetic energy of its particlesD) total potential energy of its particles

14. The temperature of a sample of matter is a measureof the

A) have no potential energyB) have strong intermolecular forcesC) are arranged in a regular, repeated geometric

patternD) are separated by great distances, compared

to their size

15. According to the kinetic molecular theory, theparticles of an ideal gas

A) The volume of the NO2(g) is greater than thevolume of the N2O4(g).

B) The volume of the NO2(g) is less than thevolume of the N2O4(g).

C) The rate of the forward reaction and the rateof the reverse reaction are equal.

D) The rate of the forward reaction and the rate ofthe reverse reaction are unequal.

16. Given the equation representing a closed system:

N2O4(g) 2NO2(g)Which statement describes this system atequilibrium?

A) activation energy B) kinetic energyC) heat of reaction D) rate of reaction

17. In a chemical reaction, the difference between thepotential energy of the products and the potentialenergy of the reactants is equal to the

A) decreases the reaction rate and has a higheractivation energy

B) decreases the reaction rate and has a loweractivation energy

C) increases the reaction rate and has a higheractivation energy

D) increases the reaction rate and has a loweractivation energy

18. For a given chemical reaction, the addition of acatalyst provides a different reaction pathway that

A) carbon atoms B) hydrogen atomsC) oxygen atoms D) nitrogen atoms

19. Which atoms can bond with each other to formchains, rings, or networks?

A) at least one single carbon-carbon bondB) at least one multiple carbon-carbon bondC) two or more single carbon-carbon bondsD) two or more multiple carbon-carbon bonds

20. A molecule of an unsaturated hydrocarbon musthave

A) an acid B) an aldehydeC) an ester D) a ketone

21. Given a formula of a functional group:

An organic compound that has this functional groupis classified as

A) Oxidation and reduction both occur at theanode.

B) Oxidation and reduction both occur at thecathode.

C) Oxidation occurs at the anode, andreduction occurs at the cathode.

D) Oxidation occurs at the cathode, and reductionoccurs at the anode.

22. Which statement describes where the oxidation andreduction half-reactions occur in an operatingelectrochemical cell?

A)

B)

C)

D)

23. Given a formula representing a compound:

Which formula represents an isomer of thiscompound?

A) chemical energy to electrical energyB) electrical energy to chemical energyC) nuclear energy to thermal energyD) thermal energy to nuclear energy

24. Which energy conversion occurs in an operatingelectrolytic cell?

A) alcoholsB) alkynesC) organic acidsD) saturated hydrocarbons

25. Which compounds can be classified as electrolytes?

A) OH– ions B) O2– ionsC) K+ ions D) H+ ions

26. Potassium hydroxide is classified as an Arrheniusbase because KOH contains

A) deposition B) distillationC) filtration D) titration

27. In which laboratory process is a volume of solutionof known concentration used to determine theconcentration of another solution?

A) H+ acceptor B) H+ donorC) OH– acceptor D) OH– donor

28. According to one acid-base theory, an acid is an

A) formation of covalent bondsB) formation of ionic bondsC) conversion of matter to energyD) conversion of energy to matter

29. Energy is released during the fission of Pu-239atoms as a result of the

A) stable nuclei emit alpha particlesB) stable nuclei emit beta particlesC) unstable nuclei emit alpha particlesD) unstable nuclei emit beta particles

30. Atoms of I-131 spontaneously decay when the

A) fewer valence electronsB) more valence electronsC) fewer electron shellsD) more electron shells

31. Compared to the atoms of nonmetals in Period 3, theatoms of metals in Period 3 have

A) iodine and silver B) iodine and xenonC) tin and silver D) tin and xenon

32. Which elements are malleable and good conductorsof electricity?

A) lithium atom B) potassium atomC) rubidium atom D) sodium atom

33. Which atom in the ground state requires the least amount of energy to remove its valence electron?

A) FeS B) Fe2S3

C) FeSO3 D) Fe2(SO3)3

34. What is the chemical formula of iron(III) sulfide?

A) 20% B) 27% C) 46% D) 53%

35. What is the percent composition by mass of sulfur inthe compound MgSO4 (gram-formula mass = 120.grams per mole)?

A) HCl B) KClC) NaCl D) NH4Cl

36. Which compound becomes less soluble in water asthe temperature of the solution is increased?

A) 70.0 g B) 90.0 gC) 180. g D) 800. g

37. Given the balanced equation representing a reaction:

2H2 + O2 2H2OWhat is the mass of H2O produced when 10.0 gramsof H2 reacts completely with 80.0 grams of O2 ?

A) Formulas A and B are both empirical.B) Formulas A and B are both molecular.C) Formula A is empirical, and formula B is

molecular.D) Formula A is molecular, and formula B is

empirical.

38. Given two formulas representing the samecompound:

Formula A CH3Formula B C2H6Which statement describes these formulas?

A) decompositionB) double replacementC) single replacementD) synthesis

39. Given the balanced equation representing areaction:

Which type of reaction is represented by thisequation?

A) both the air and the water to the cylinderB) both the cylinder and the air to the waterC) the air to the water and from the water to the

cylinderD) the cylinder to the water and from the water

to the air

40. In a laboratory where the air temperature is 22°C, asteel cylinder at 100.°C is submerged in a sample ofwater at 40.°C. In this system, heat flows from

A)

B)

C)

D)

41. Which diagram represents a physical change, only?

A) 1 and 3 B) 1 and 5C) 4 and 2 D) 4 and 3

42. During a laboratory activity to investigate reactionrate, a student reacts 1.0-gram samples of solid zincwith 10.0-milliliter samples of HCl(aq). The tablebelow shows information about the variables in fiveexperiments the student performed.

Which two experiments can be used to investigatethe effect of the concentration of HCl(aq) on thereaction rate?

A) from 400. K to 200. KB) from 200. K to 400. KC) from 400.°C to 200.°CD) from 200.°C to 400.°C

43. Which temperature change would cause a sample ofan ideal gas to double in volume while the pressureis held constant?

A) 8.0°C B) 14°CC) 30.°C D) 55°C

44. A 36-gram sample of water has an initialtemperature of 22°C. After the sample absorbs 1200joules of heat energy, the final temperature of thesample is

A) Molecules of Br2 are polar, and molecules of I2 are nonpolar.

B) Molecules of I2 are polar, and molecules of Br2 are nonpolar.

C) Molecules of Br2 have stronger intermolecularforces than molecules of I2 .

D) Molecules of I2 have stronger intermolecularforces than molecules of Br2 .

45. Which statement explains why Br2 is a liquid at STPand I2 is a solid at STP?

A) Ba(NO3)2 + Na2SO4 ®BaSO4 + 2NaNO3

B) H3PO4 + 3KOH ®K3PO4 + 3H2OC) Fe(s) + S(s) ®FeS(s)D) NH3(g) + HCl(g) ®NH4Cl(s)

46. Which balanced equation represents anoxidation-reduction reaction?

A) KCl(aq) B) CaO(aq)C) NaOH(aq) D) H2SO4(aq)

47. Which solution reacts with LiOH(aq) to produce asalt and water?

A) 6.0 mL B) 12 mLC) 24 mL D) 48 mL

48. Which volume of 2.0 M NaOH(aq) is needed tocompletely neutralize 24 milliliters of 1.0 MHCl(aq)?

A) combustionB) decompositionC) nuclear fusionD) oxidation-reduction

49. Which type of reaction releases the greatest amountof energy per mole of reactant?

A) 94 Be + 11H ® 63Li + 42

B) 147N + 42 He ® 178O + 11HC) 23994Pu + 10n ® 14458Ce + 9436Kr + 210nD) 23892U ® 23490Th + 42He

50. Which balanced equation represents naturaltransmutation?

51. Explain, in terms of protons and neutrons, whyU-235 and U-238 are different isotopes of uranium.

Base your answers to questions 52 through 54 on the information below.The bright-line spectra for three elements and a mixture of elements are shown below.

52. Explain, in terms of both electrons and energy, how the bright-line spectrum of an element isproduced.

53. Identify all the elements in the mixture.

54. State the total number of valence electrons in a cadmium atom in the ground state.

Base your answers to questions 55 through 59 on the information below.The ionic radii of some Group 2 elements are given in the table below.

55. On the grid, mark an appropriate scale on the axis labeled "Ionic Radius (pm)."

56. On the same grid, plot the data from the data table. Circle and connect the points.

57. Estimate the ionic radius of strontium.

58. State the trend in ionic radius as the elements in Group 2 are considered in order of increasing atomicnumber.

59. Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomicradius.

Base your answers to questions 60 and 61 on theinformation below.The balanced equation below represents thedecomposition of potassium chlorate.

2KClO3(s) ®2KCl(s) + 3O2(g)60. Determine the oxidation number of chlorine in the

reactant in the equation.

61. State why the entropy of the reactant is less than theentropy of the products.

Base your answers to questions 62 and 63 on the information below.

At 550°C, 1.00 mole of CO2(g) and 1.00 mole of H2(g) are placed in a 1.00-liter reaction vessel. Thesubstances react to form CO(g) and H2O(g). Changes in the concentrations of the reactants and theconcentrations of the products are shown in the graph below.

62. Determine the change in the concentration of CO2(g) between time t 0 and time t 1.

63. What can be concluded from the graph about the concentrations of the reactants and theconcentrations of the products between time t 1 and time t 2?


A reaction between bromine and a hydrocarbon is represented by the balanced equation below.

64. Identify the type of organic reaction.

65. Write the name of the homologous series to which the hydrocarbon belongs.

Base your answers to questions 66 through 68 on theinformation below.

Ozone, O3(g), is produced from oxygen, O2(g) byelectrical discharge during thunderstorms. Theunbalanced equation below represents the reactionthat forms ozone.

66. Balance the equation for the production of ozone,using the smallest whole-number coefficients.

67. Identify the type of bonding between the atoms in anoxygen molecule.

68. Explain, in terms of electron configuration, why anoxygen molecule is more stable than an oxygenatom.

Base your answers to questions 69 and 70 on theinformation below.

Natural gas is a mixture that includes butane, ethane,methane, and propane. Differences in boiling pointscan be used to separate the components of naturalgas. The boiling points at standard pressure for thesecomponents are listed in the table below.

69. Identify a process used to separate the componentsof natural gas.

70. List the four components of natural gas in order ofincreasing strength of intermolecular forces.

Base your answers to questions 71 through 73 on the information below.

In 1864, the Solvay process was developed to makesoda ash. One step in the process is represented bythe balanced equation below.

NaCl + NH3 + CO2 + H2O NaHCO3 + NH4Cl71. Write the chemical formula for one compound in the

equation that contains both ionic bonds andcovalent bonds.

72. Explain, in terms of electronegativity difference,why the bond between hydrogen and oxygen in awater molecule is more polar than the bond betweenhydrogen and nitrogen in an ammonia molecule.

73. In the space draw a Lewis electron-dot diagram forthe reactant containing nitrogen in the equation.

74. A student prepared two mixtures, each in a labeledbeaker. Enough water at 20.°C was used to make100 milliliters of each mixture.

Classify each mixture using the term"homogeneous" or the term "heterogeneous."


A student prepared two mixtures, each in a labeled beaker. Enough water at 20.°C was used to make100 milliliters of each mixture.

75. Determine the volume of the Fe filings used to produce mixture 2.

76. Describe a procedure to physically remove the water from mixture 1.


A student performed a laboratory activity to observe the reaction between aluminum foil and anaqueous copper(II) chloride solution. The reaction is represented by the balanced equation below.

2Al(s) + 3CuCl2(aq) ®3Cu(s) + 2AlCl3(aq) + energy

The procedures and corresponding observations for the activities are given below.

77. State one observation that indicates Cu2+ ions became Cu atoms.

78. Describe one change in the procedure that would cause the reaction to occur at a faster rate.

79. State one safety procedure the student should perform after completing the laboratory activity.

Base your answers to questions 80 through 82 on theinformation below.

Some carbonated beverages are made by forcingcarbon dioxide gas into a beverage solution. When abottle of one kind of carbonated beverage is firstopened, the beverage has a pH value of 3.

80. State, in terms of the pH scale, why this beverage isclassified as acidic.

81. Using Table M, identify one indicator that is yellowin a solution that has the same pH value as thisbeverage.

82. After the beverage bottle is left open for severalhours, the hydronium ion concentration in thebeverage solution decreases to of the originalconcentration. Determine the new pH of thebeverage solution.


Polonium-210 occurs naturally, but is scarce. Polonium-210 is primarily used in devices designed toeliminate static electricity in machinery. It is also used in brushes to remove dust from camera lenses.Polonium-210 can be created in the laboratory by bombarding bismuth-209 with neutrons to createbismuth-210. The bismuth-210 undergoes beta decay to produce polonium-210. Polonium-210 has ahalf-life of 138 days and undergoes alpha decay.

83. State one beneficial use of Po-210.

84. Complete the nuclear equation for the decay of Po-210, by writing a notation for the missing product.

85. Determine the total mass of an original 28.0-milligram sample of Po-210 that remains unchangedafter 414 days.

Answer KeyRegents Practice Exam 2

1. C2. B3. A4. C5. A6. B7. C8. D9. C10. A11. D12. B13. D14. A15. D16. C17. C18. D19. A20. B21. A22. C23. B24. B25. C26. A27. D28. B29. C30. D31. A32. C33. C34. B35. B

36. A37. B38. C39. C40. D41. A42. D43. B44. C45. D46. C47. D48. B49. C50. D51. – A U-235 atom has

92 protons and 143neutrons, and aU-238 atom has 92protons and 146neutrons. – A U-235atom and a U-238atom have the samenumber of protonsbut a differentnumber of neutrons.

52. – When electrons inan excited statereturn to a lowerenergy state, specificamounts of energyare emitted. Theseenergies areassociated withspecific wavelengthsof light that arecharacteristic of thebright-line spectrumof an element. –Energy is emittedwhen excitedelectrons fall back tolower shells.

53. – lithium andstrontium

54. – 255.

56.

57. – 117 pm 2 pm58. – As the atomic

number of elementsin Group 2increases, the ionicradius increases. –The ionic radiusincreases.

59. – The valenceelectron shell of aGroup 2 atom is lostwhen it becomes anion. – A Group 2 ionhas two fewerelectrons than theatom from which itwas formed.

60. – +561. – The gaseous

product is moredisordered than thesolid reactant. – Thesolid reactant ismore ordered thanthe products.

62. – –0.27 mol/L – 0.27mol/L

63. – Between time t 1 and time t 2, theconcentrations of thereactants and theconcentrations of theproducts are nolonger changing. –The concentrationsof the reactants andthe products remainconstant. – Theconcentration ofeach reactant is 0.73mol/L, and theconcentration ofeach product is 0.27mol/L.

64. – addition –halogenation –bromination

65. – alkene or alkenes.66.

67. – nonpolar covalent– covalent – doublecovalent

68. – Both atoms in anO2 molecule haveachieved a noble gaselectronconfiguration. – Anoxygen atom doesnot have a stableoctet of valenceelectrons.

69. – fractionaldistillation –distillation

70.

Answer KeyRegents Practice Exam 2

71. NaHCO3 or NH4Cl.72. – The

electronegativitydifference is 1.4 forH and O, which ishigher than the 0.9for H and N. – Thedifference inelectronegativitybetween hydrogenand oxygen isgreater than that forhydrogen andnitrogen.

73.

74. – Mixture 1:homogeneous –Mixture 2:heterogeneous

75. – 2.02 cm3

76. – Heat mixture 1until all the waterevaporates. – Allowthe water toevaporate.

77. – The solution is nolonger blue green. –A reddish-brownsolid is formed.

78. – Heat the solutionbefore adding thealuminum foil. –Increase theconcentration of theCuCl2 solution. –Cut the Al foil intoeven smaller pieces.

79. – Thoroughly washthe lab equipmentand return it to itsproper storage place.– Dispose of thechemicals asdirected by theteacher. – Washhands before leavingthe lab room.

80. – The beverage isacidic because itspH value is below 7.– A pH of 3 is in theacid range on the pHscale.

81. – bromthymol blue –bromcresol green –thymol blue

82. – 683. – Polonium-210 is

used to eliminatestatic electricity inmachinery. –removes dust fromcamera lenses

84. –85. – 3.5 mg

name: regents practice exam 2 2016

Documents