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1 What is the number of protons in an atom with
  the electron configuration of 2-5?
  (1) 5                     (3) 3
  (2) 2                     (4) 7

2 In the wave-mechanical model of an atom, an
  orbital is defined as
  (1) a region of the most probable neutron
      location
  (2) a region of the most probable electron
      location
  (3) the straight-line path of a neutron
  (4) the straight-line path of an electron

3 In the ground state, which shell of a potassium
  atom has an electron with the greatest amount of
  energy?
  (1) first                (3) third
  (2) second               (4) fourth

4 Which phrase describes two atoms that contain
  the same number of protons but a different
  number of neutrons?
  (1) ions of the same element
  (2) isotopes of the same element
  (3) a mixture of different elements
  (4) nuclides of different elements

5 All atoms of an element have the same
  (1) mass number
  (2) atomic mass
  (3) number of neutrons
  (4) number of protons

6 Which Group 15 element is classified as a metal?
  (1) N                  (3) As
  (2) P                  (4) Bi

7 Compared to the number of electron shells and
  radius of an aluminum atom in the ground state,
  a boron atom in the ground state has
  (1) fewer electron shells and a smaller radius
  (2) fewer electron shells and a larger radius
  (3) more electron shells and a smaller radius
  (4) more electron shells and a larger radius

8 Hydrogen sulfide, H2S, is classified as a
  (1) compound with atoms in a fixed proportion
  (2) compound with atoms in a proportion that
      can vary
  (3) mixture with atoms in a fixed proportion
  (4) mixture with atoms in a proportion that can
      vary

9 A structural formula differs from a molecular
  formula in that a structural formula shows the
  (1) arrangement of atoms
  (2) number of atoms
  (3) ratio of atoms
  (4) types of atoms

10 Which type of reaction occurs when a compound
   is separated into its elements?
   (1) synthesis
   (2) decomposition
   (3) single replacement
   (4) double replacement

11 Which terms represent two categories of
   compounds?
   (1) chemical and physical
   (2) chemical and molecular
   (3) ionic and physical
   (4) ionic and molecular

12 When an atom of hydrogen and an atom of
   chlorine combine to form a molecule of hydrogen
   chloride, a bond is
   (1) formed as energy is absorbed
   (2) formed as energy is released
   (3) broken as energy is absorbed
   (4) broken as energy is released

13 All atoms of the element vanadium must have
   the same
   (1) atomic number
   (2) mass number
   (3) number of neutrons plus electrons
   (4) number of protons plus neutrons

14 Which sample of matter can be separated into
   two different substances by physical means?
   (1) liquid bromine
   (2) gaseous propane
   (3) solid sodium acetate
   (4) aqueous magnesium sulfate

15 Two liquids can be separated by distillation due
   to a difference in
   (1) concentration       (3) boiling point
   (2) conductivity        (4) heat of fusion

16 Which unit can be used to express the
   concentration of a PbCl2(aq) solution?
   (1) kelvins              (3) pascals
   (2) kilojoules per gram (4) parts per million

17 Compared to the freezing point and boiling point
   of water at 1.0 atm, a 0.5 M aqueous solution of
   NaCl at 1.0 atm has
   (1) a lower freezing point and a lower boiling
       point
   (2) a lower freezing point and a higher boiling
       point
   (3) a higher freezing point and a lower boiling
       point
   (4) a higher freezing point and a higher boiling
       point

18 Which form of energy is converted to thermal
   energy when propane burns in air?
   (1) chemical           (3) mechanical
   (2) electrical         (4) nuclear

19 According to the kinetic molecular theory, which
   statement explains why an ideal gas can be
   compressed to a smaller volume?
   (1) The motion of the gas particles is circular and
       orderly.
   (2) The force of attraction between the gas
       particles is strong.
   (3) As the gas particles collide, the total energy
       of the system decreases.
   (4) The gas particles are separated by great
       distances relative to their size.

20 Under which conditions of temperature and
   pressure does a sample of propane behave least
   like an ideal gas?
   (1) 250. K and 1.0 atm (3) 500. K and 1.0 atm
   (2) 250. K and 5.0 atm (4) 500. K and 5.0 atm

21 Compared to a 1.0-L sample of CO2(g) in a
   sealed, rigid container at STP, a 1.0-L sample of
   CH4(g) in a sealed, rigid container at STP has the
   same
   (1) density
   (2) molar mass
   (3) chemical properties
   (4) number of molecules

22 A chemical reaction occurs when

23 What is the purpose of adding a catalyst to a
   chemical reaction?
   (1) to decrease the potential energy of the
       products
   (2) to increase the potential energy of the
       reactants
   (3) to convert solid reactants to liquid reactants
   (4) to provide an alternate reaction pathway

24 Systems in nature tend to undergo changes
   toward
   (1) lower energy and less disorder
   (2) lower energy and greater disorder
   (3) higher energy and less disorder
   (4) higher energy and greater disorder

25 Which reaction occurs at the anode in an
   electrochemical cell?
   (1) neutralization    (3) reduction
   (2) oxidation         (4) substitution

26 As more NaCl(s) is dissolved in a dilute,
   unsaturated NaCl(aq) solution, the conductivity
   of the solution
   (1) decreases as the ion concentration decreases
   (2) decreases as the ion concentration increases
   (3) increases as the ion concentration decreases
   (4) increases as the ion concentration increases

27 Which substance always forms when an Arrhenius
   acid reacts with an Arrhenius base?

28 Which symbol represents a nuclear emission
   with the greatest mass and the greatest ionizing
   power?

29 One potential benefit of nuclear fusion reactions is
   (1) reactor meltdown
   (2) uncontrolled chain reaction
   (3) production of large amounts of energy
   (4) production of radioactive waste materials

30 Determining the age of a wooden beam from a
   sunken ship is an example of a beneficial use of
   (1) Lewis structures
   (2) polyatomic ions
   (3) radioactive nuclides
   (4) homogeneous mixture

 Some questions
may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
 31 Given the bright-line spectra of four elements and the spectrum of a mixture formed from two of these
    elements:

Which two elements are present in this mixture?
(1) A and Q                                       (3) G and Q
(2) A and E                                       (4) G and E

32 What is the approximate mass of an atom that has 10 electrons, 10 protons, and 9 neutrons?
   (1) 10. u                                         (3) 20. u
   (2) 19 u                                          (4) 29 u

33 Which electron configuration represents the electrons of an atom in an excited state?
   (1) 2-7-3                                         (3) 2-8-8-1
   (2) 2-8-2                                         (4) 2-8-9-2

34 Given information about the naturally occurring
   isotopes of bromine:

Which numerical setup can be used to determine
the atomic mass of bromine?
(1)   (78.92 u)(50.69) + (80.92 u)(49.31)
(2)   (80.92 u)(50.69) + (78.92 u)(49.31)
(3)   (78.92 u)(0.5069) + (80.92 u)(0.4931)
(4)   (80.92 u)(0.5069) + (78.92 u)(0.4931)

35 What is a chemical name of the compound CuS?
   (1) copper(I) sulfide   (3) copper(II) sulfide
   (2) copper(I) sulfate   (4) copper(II) sulfate

36 Given the equation representing a reaction:

What is the mass of N2(g) produced when
1.0 gram of H2(g) completely reacts with 15.0
grams of NO(g) to produce 9.0 grams of H2O(g)?
(1) 7.0 g               (3) 25.0 g
(2) 14.0 g              (4) 28.0 g

37 An atom of which element bonds with an atom of
   hydrogen to form the most polar bond?
   (1) bromine             (3) fluorine
   (2) chlorine            (4) iodine

38 Given the diagram representing a classification
   of matter:

Which types of matter are represented by X and
Z in the diagram?
(1) X is mixture, and Z is substance.
(2) X is substance, and Z is mixture.
(3) X is element, and Z is compound.
(4) X is compound, and Z is element.

39 Based on Table G, which sample, when added
   to 100. grams of water and thoroughly stirred,
   produces a heterogeneous mixture at 20.°C?
   (1) 20. g of KCl        (3) 80. g of KCl
   (2) 20. g of KI         (4) 80. g of KI

40 How many milliliters of 1 M HCl(aq) must be
   diluted with water to make exactly 500 mL of 0.1
   M HCl(aq)?
   (1) 10 mL                (3) 100 mL
   (2) 50 mL                (4) 5000 mL

41 Which two particle diagrams represent two different phases of the same compound, only?

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

42 A sample of KCl(s) is dissolved in water to form KCl(aq). When the water in the KCl(aq) is completely
   evaporated, KCl(s) remains. Which statement describes a property of the KCl(s) after the water evaporated?
   (1) The KCl(s) becomes a molecular compound. (3) The melting point of the KCl(s) is unchanged.
   (2) The molar mass of the KCl(s) decreases.      (4) The KCl(s) conducts an electric current.

43 Which statement describes ice and liquid water in a stoppered flask at 0°C at equilibrium?
   (1) The rate of melting must equal the rate of freezing.
   (2) The rate of freezing must be greater than the rate of melting.
   (3) The mass of the ice must equal the mass of the liquid water.
   (4) The mass of the ice must be greater than the mass of the liquid water.

44 Given the equation representing a system at equilibrium in a sealed, rigid container:

When heat is added to the system, the concentration of N2(g)
(1) decreases and the concentration of NO(g) decreases
(2) decreases and the concentration of NO(g) increases
(3) increases and the concentration of NO(g) increases
(4) increases and the concentration of NO(g) decreases

45 Given the potential energy diagram for a reaction:

Which numbered interval represents   the
activation energy of the reaction?
(1) 1                      (3) 3
(2) 2                      (4) 4

46 Given the formula representing a compound:

What is a chemical name for the compound?
(1) 2-chloropentene     (3) 4-chloropentene
(2) 2-chloropentane     (4) 4-chloropentane

47 Which formula represents a saturated organic
   compound?

48 The     compounds     CH3CH2CH2OH        and
   CH3OCH2CH3 have different
   (1) numbers of carbon atoms per mole
   (2) numbers of hydrogen atoms per mole
   (3) functional groups
   (4) molecular masses

49 The diagram and ionic equation below represent
   an operating voltaic cell.

Which phrase describes the direction of electron
flow in this cell?
(1) from Ni(s) through the wire to Mg(s)
(2) from Mg(s) through the wire to Ni(s)
(3) from Ni2+(aq) ions through the salt bridge to
    Mg2+(aq) ions
(4) from Mg2+(aq) ions through the salt bridge
    to Ni2+(aq) ions

50 Given the equation representing a reaction at
   equilibrium:

According to one acid-base theory, which pair are
the H+ donors?
(1)   NH3(aq) and H2O(l)
(2)   NH3(aq) and OH-(aq)
(3)   NH4+(aq) and H2O(l)
(4)   NH4+(aq) and OH-(aq)

[1] Allow 1 credit for Au or gold.

Base your answers to questions 52 through 54 on the information below and on your knowledge of chemistry.
         Fluorine, chlorine, bromine, and iodine are located in Group 17 and are called halogens.
      52 State, in terms of electrons, why these halogens have similar chemical properties. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The halogen atoms all have seven valence electrons.
         Since atoms of these elements have the same number of outer shell electrons, they tend to have
         similar properties.
         same number of valence electrons
         All halogen atoms need one more electron to form a stable octet.

53 Compare the radius of a chlorine atom to the radius of a Cl- ion. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The chlorine atom is smaller than a chloride ion.
         The Cl- ion is larger.
         The atom is smaller.

54 In the space in your answer booklet, draw a Lewis electron-dot diagram for an atom of
   fluorine in the ground state. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit. The positions of the electrons may vary.

Base your answers to questions 55 through 57 on the information below and on your knowledge of chemistry.
         A sample of helium gas in a sealed, rigid container is at 240. K and 120. kPa. The
      temperature is increased to 360. K.
      55 State the number of significant figures to which the given pressure is expressed. [1]

[1] Allow 1 credit for 3 or three.

56 Determine the pressure of the helium at 360. K. [1]

[1] Allow 1 credit for 180. kPa or 180 kPa.

57 Show a numerical setup for converting 120. kPa to atmospheres. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit. Acceptable responses include, but are not limited to:

Base your answers to questions 58 and 59 on the information below and on your knowledge of chemistry.
         The table and graph below show information about five aldehydes.

58 Based on the graph, determine the boiling point of butanal at standard pressure. [1]

[1] Allow 1 credit for any value from 340. K to 360. K, inclusive.

59 Determine the mass of 3.00 moles of propanal using the molar mass given in the
   table. [1]

[1] Allow 1 credit for 174 g or any value from 173.997 g to 174.3 g, inclusive.

Base your answers to questions 60 through 62 on the information below and on your knowledge of chemistry.
          A 100.-mL sample of liquid water is heated in a flask to boiling at 1 atm. As the water
      boils, some liquid water changes phase to water vapor. The equation below represents this
      change.

60 Describe the change in potential energy of the water molecules that vaporize during
   boiling. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The potential energy of the water molecules increases.
         The water vapor molecules have greater potential energy.
         The steam has more PE.

61 Compare the entropy of the H2O(l) to the H2O(g) that is formed. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The entropy of the liquid is less than the entropy of the gas.
         H2O(l) has less entropy.
         The gas is more random.
         Steam is more disordered.

62 Determine the mass of liquid water that vaporizes if 7700 joules of energy is absorbed
   by the H2O(l) at 100.°C. [1]

[1] Allow 1 credit for 3.4 g or any value from 3.4 g to 3.41 g, inclusive.

Base your answers to questions 63 through 65 on the information below and on your knowledge of chemistry.
         Tritium, hydrogen-3, is a radioisotope.
      63 State the number of neutrons in an atom of tritium. [1]

[1] Allow 1 credit for 2 or two.

64 Complete the nuclear equation in your answer booklet for the decay of tritium by writing
   a notation for the missing nuclide. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit. Acceptable responses include, but are not limited to:

65 Based on Table N, identify a nuclide that has the same decay mode as tritium, but has
   a longer half-life. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit for any nuclide on Table N that decays by β- emission and has a half-life longer than
    12.31 y. Acceptable responses include, but are not limited to:

Part C
Answer all questions in this part.
Directions (66-85): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. Base your answers to questions 66 through 69 on the information below and on your knowledge of chemistry. Phosphorus combines with oxygen to form an oxide that reacts with water to produce phosphoric acid, which is an important industrial compound used to produce fertilizers. An unbalanced equation for the production of phosphoric acid is shown below.

66 Balance the equation in your answer booklet for the production of phosphoric acid,
   using the smallest whole-number coefficients. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

67 Write the empirical formula of the solid reactant in the equation. [1]

[1] Allow 1 credit for P2O5. The order of the elements may vary.

68 Show a numerical setup for calculating the percent composition by mass of phosphorus
   in P4O10 (formula mass = 283.89 u). [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit. Acceptable responses include, but are not limited to:

Note: Do not allow credit if the fraction is not multiplied by 100.

69 Determine the oxidation state of phosphorus in the phosphoric acid. [1]

[1] Allow 1 credit for +5 or 5+.

Base your answers to questions 70 through 73 on the information below and on your knowledge of chemistry.
         Calcium oxide, CaO, also known as lime, is an important industrial chemical. Lime can
      be obtained by the heating of limestone, which is mainly calcium carbonate, CaCO3. An
      equation representing the reaction for the production of lime is shown below.

70 State the solubility of limestone in water. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         CaCO3 has very low solubility.
         Limestone is not soluble in water.
         insoluble

71 State evidence from the equation that the reaction to form lime is endothermic. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The energy term is on the reactant side of the equation.
         Heat is on the left side of the equation.
         Heat must be added to decompose limestone and form lime.

72 Identify the noble gas that has atoms in the ground state with the same electron
   configuration as the calcium ion, in the ground state, in the CaCO3. [1]

[1] Allow 1 credit for Ar or argon

73 State the type of chemical bonding in a sample of CaO. [1]

[1] Allow 1 credit for ionic bonding or ionic.

Base your answers to questions 74 and 75 on the information below and on your knowledge of chemistry.
           During a laboratory activity, a student places 20.0 mL of HCl(aq) of unknown
      concentration into a flask. The solution is titrated with 0.10 M KOH(aq) until the HCl(aq)
      is exactly neutralized. At the end of the titration, the volume of KOH(aq) added is 42.0 mL.
      During the laboratory activity appropriate safety equipment was used and safety procedures
      were followed.
      74 Compare the number of moles of H+(aq) ions to the number of moles of OH-(aq) ions
         in the titration mixture when the HCl(aq) is exactly neutralized by the KOH(aq). [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The number of moles of H+(aq) ions is equal to the number of moles of OH-(aq) ions.
         The number of hydrogen ions is the same as the number of hydroxide ions.
         The ratio of H+ to OH- is 1:1.

75 Determine the concentration of the HCl(aq) solution using the titration data. [1]

[1] Allow 1 credit for 0.21 M or any value from 0.2 M to 0.21 M, inclusive.

Base your answers to questions 76 and 77 on the information below and on your knowledge of chemistry.
          A scientific sampling instrument landed on a comet. Four of the organic compounds
      detected on the comet are methyl isocyanate, propanone, propanal, and ethanamide. The
      structural formula for methyl isocyanate is shown below:

76 Identify the element in these four compounds that makes them organic compounds. [1]

[1] Allow 1 credit for C or carbon.

77 Write the names of the two organic compounds detected on the comet that are isomers
   of each other. [1]

[1] Allow 1 credit for propanone and propanal.

Base your answers to questions 78 through 81 on the information below and on your knowledge of chemistry.
          During a laboratory activity appropriate safety equipment is used and safety
      procedures are followed. A student tests samples of four different metals using 0.20 M
      aqueous metal ion solutions of the same four metals. The student uses a 24-well plate as the
      reaction container for the different metal and solution combinations.
          Before placing a metal strip in each solution, the student cleans the surface of the
      metal strip with sandpaper. The 24-well plate diagram below shows the setup and results of
      the investigation. In each vertical column, the metal strips are all the same metal. For each
      horizontal row, all of the solutions contain the same type of metal ion.

78 Using the results of the student's investigation, state evidence that zinc metal is more
   active than copper metal. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The Cu metal is less active than Zn metal since Cu metal does not react with any of the
         solutions and Zn metal reacts with two solutions.
         Zinc metal is more chemically active than copper metal, because zinc reacts with Fe2+ ions and
         copper does not.
         The Zn(s) reacted with the Cu2+(aq), but the Cu(s) does not react with the Zn2+(aq).
         Zinc is dark in more solutions.
    Note: Do not allow credit for a response based on Table J.

79 Compare the number of electrons lost by the Mg(s) placed in the Zn2+(aq) solution to
   the number of electrons gained by the Zn2+(aq). [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The Mg(s) strip loses the same number of electrons that the Zn2+(aq) ions gain.
         The number of electrons lost and gained are equal.
         equal
         same

80 Write a balanced, half-reaction equation for the reduction of the copper ions. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit. Acceptable responses include, but are not limited to:

Note: Do not allow credit for the e without the minus sign (-).

81 State why the student was instructed to clean the surface of the metal strips with
   sandpaper before placing each strip into an aqueous metal ion solution. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         Sanding the surface of the metal strip exposes unoxidized metal for a possible reaction.
         Cleaning the metal provides a fresh metal surface for the reaction.
         If a reaction will occur, it is more likely with pure metal available.
         removes tarnish
         increase surface area of the pure metal

Base your answers to questions 82 and 83 on the information below and on your knowledge of chemistry.
          Tetrachloromethane, CCl4, was used as a dry cleaning solvent until it was banned for this
      use in the U.S. in 1970 due to its toxicity. This solvent was replaced in many dry cleaning
      processes by tetrachloroethene, C2Cl4. Another currently available alternative dry cleaning
      solvent is 1-bromopropane. The table below shows the boiling points of these solvents.

82 Explain, in terms of intermolecular forces, why tetrachloroethene has a higher boiling
   point than tetrachloromethane. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         The tetrachloroethene has stronger intermolecular forces than in CCl4.
         The attractions between the molecules of tetrachloromethane are weaker.
         C2Cl4 has stronger IMFs.

83 Draw a structural formula for 1-bromopropane. [1]

Answer: Answer: MODEL ANSWER GIVEN BELOW

[1] Allow 1 credit.

Note: Do not allow credit if only some of the H atoms bonded to C atoms are shown.

Base your answers to questions 84 and 85 on the information below and on your knowledge of chemistry.
         When a neutron is absorbed by a uranium-235 nucleus, the nucleus can split. One
      possible nuclear reaction is represented by the balanced equation below.

    In this reaction, the products have a mass that is 0.180 u less than the mass of the
reactants.
84 Compare the energy released per gram of reactant during this reaction to the energy
   released per gram of reactant in a chemical reaction. [1]

[1] Allow 1 credit. Acceptable responses include, but are not limited to:
         This nuclear reaction releases more energy per gram than a chemical reaction.
         The nuclear reaction releases more energy.
         A chemical reaction releases less energy.

85 Determine the time required for an 8.00-mg sample of Sr-90 to decay until only
   2.00 mg of the sample remains unchanged. [1]

[1] Allow 1 credit for 58.2 y. Significant figures do not need to be shown.

  Try the Quiz :     Physical Setting / Chemistry - New York Regents August 2022 Exam