2022 (Aug.): NY Regents - Chemistry - Sara Cowley | Library

Instructions

From the New York State Education Department. The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY. Internet. Available from https://www.nysedregents.org/Chemistry/822/chem82022-exam.pdf; accessed 13, June, 2023.

Standard tagging pending.

1.

What is the number of protons in an atom with the electron configuration of 2-5?

2.

In the wave-mechanical model of an atom, an orbital is defined as

3.

In the ground state, which shell of a potassium atom has an electron with the greatest amount of energy?

4.

Which phrase describes two atoms that contain the same number of protons but a different number of neutrons?

5.

All atoms of an element have the same

6.

Which Group 15 element is classified as a metal?

7.

8.

Hydrogen sulfide, H2S, is classified as a

9.

A structural formula differs from a molecular formula in that a structural formula shows the

10.

Which type of reaction occurs when a compound is separated into its elements?

11.

Which terms represent two categories of compounds?

12.

When an atom of hydrogen and an atom of chlorine combine to form a molecule of hydrogen chloride, a bond is

13.

All atoms of the element vanadium must have the same

14.

Which sample of matter can be separated into two different substances by physical means?

15.

Two liquids can be separated by distillation due to a difference in

16.

Which unit can be used to express the concentration of a \mathrm{PbCl_2(aq)} solution?

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

18.

Which form of energy is converted to thermal energy when propane burns in air?

19.

According to the kinetic molecular theory, which statement explains why an ideal gas can be compressed to a smaller volume?

20.

Under which conditions of temperature and pressure does a sample of propane behave least like an ideal gas?

21.

Compared to a 1.0-L sample of \mathrm{CO_2(g)} in a sealed, rigid container at \mathrm{STP}, a 1.0-L sample of \mathrm{CH_4(g)} in a sealed, rigid container at \mathrm{STP} has the same

22.

A chemical reaction occurs when

23.

What is the purpose of adding a catalyst to a chemical reaction?

24.

Systems in nature tend to undergo changes toward

25.

Which reaction occurs at the anode in an electrochemical cell?

26.

As more \mathrm{NaCl(s)} is dissolved in a dilute, unsaturated \mathrm{NaCl(aq)} solution, the conductivity of the solution

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

30.

Determining the age of a wooden beam from a sunken ship is an example of a beneficial use of

The 2011 Edition Reference Tables for Physical Setting/Chemistry can be found here.

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?

32.

What is the approximate mass of an atom that has 10 electrons, 10 protons, and 9 neutrons?

33.

Which electron configuration represents the electrons of an atom in an excited state?

34.

Given information about the naturally occurring isotopes of bromine:

Which numerical setup can be used to determine the atomic mass of bromine?

35.

What is a chemical name of the compound \mathrm{CuS}?

36.

Given the equation representing a reaction:

\mathrm{2H_2(g)+2NO(g) → N_2(g)+2H_2O(g)}

What is the mass of \mathrm{N_2(g)} produced when 1.0 gram of \mathrm{H_2(g)} completely reacts with 15.0 grams of \mathrm{NO(g)} to produce 9.0 grams of \mathrm{H_2O(g)}?

37.

An atom of which element bonds with an atom of hydrogen to form the most polar bond?

38.

Given the diagram representing a classification of matter:

Which types of matter are represented by X and Z in the diagram?

39.

Based on Table G, which sample, when added to 100. grams of water and thoroughly stirred, produces a heterogeneous mixture at 20.°C?

40.

How many milliliters of \mathrm{1\space M\space HCl(aq)} must be diluted with water to make exactly 500 mL of \mathrm{0.1\space M\space HCl(aq)}?

41.

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

42.

A sample of \mathrm{KCl(s)} is dissolved in water to form \mathrm{KCl(aq)}. When the water in the \mathrm{KCl(aq)} is completely evaporated, \mathrm{KCl(s)} remains. Which statement describes a property of the \mathrm{KCl(s)} after the water evaporated?

43.

Which statement describes ice and liquid water in a stoppered flask at 0°C at equilibrium?

44.

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

\mathrm{N_2(g)+O_2(g)+182.6\space kJ ⇌ 2NO(g)}

When heat is added to the system, the concentration of \mathrm{N_2(g)}

45.

Given the potential energy diagram for a reaction:

Which numbered interval represents the activation energy of the reaction?

46.

Given the formula representing a compound:

What is a chemical name for the compound?

47.

Which formula represents a saturated organic compound?

48.

The compounds \mathrm{CH_3CH_2CH_2OH} and \mathrm{CH_3OCH_2CH_3} have different

49.

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

Which phrase describes the direction of electron flow in this cell?

50.

Given the equation representing a reaction at equilibrium:

\mathrm{NH_3(aq)+H_2O(\ell)\rightleftharpoons NH_4^+(aq)+OH^-(aq)}

According to one acid-base theory, which pair are the \mathrm{H^+} donors?

51.

Identify a metal from Table J that is less active than silver.

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.

53.

Compare the radius of a chlorine atom to the radius of a \mathrm{Cl^-} ion

54.

In the Show Your Work space, draw a Lewis electron-dot diagram for an atom of fluorine in the ground state.

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.

56.

Determine the pressure of the helium at 360. K.

_______ kPa

57.

Show a numerical setup for converting 120. kPa to atmospheres.

Base your answers to questions 58 and 59 on the information below and on your knowledge of chemistry. 

The table and graph at the left show information about five aldehydes.

58.

Based on the graph, determine the boiling point of butanal at standard pressure.

_______ K

59.

Determine the mass of 3.00 moles of propanal using the molar mass given in the table.

_______ g

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 fl ask to boiling at 1 atm. As the water boils, some liquid water changes phase to water vapor. The equation below represents this change.

\mathrm{H_2O(\ell)+heat → H_2O(g)}

60.

Describe the change in potential energy of the water molecules that vaporize during boiling.

61.

Compare the entropy of the \mathrm{H_2O(\ell)} to the \mathrm{H_2O(g)} that is formed.

62.

Determine the mass of liquid water that vaporizes if 7700 joules of energy is absorbed by the \mathrm{H_2O(\ell)} at 100.°C.

_______ g

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.

_______ 

64.

Complete the nuclear equation in the Show Your Work space for the decay of tritium by writing a notation for the missing nuclide.

The Show Your Work space is available to you as an option.

_______

65.

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

The Show Your Work space is available to you as an option.

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. 

\mathrm{P_4O_{10}(s)+H_2O(\ell) → H_3PO_4(aq)+energy}

66.

Balance the equation in the Show Your Work space for the production of phosphoric acid, using the smallest whole-number coefficients.

67.

Write the empirical formula of the solid reactant in the equation.

68.

Show a numerical setup for calculating the percent composition by mass of phosphorus in \mathrm{P_4O_{10}} (formula mass = 283.89 u).

69.

Determine the oxidation state of phosphorus in the phosphoric acid.

_______ 

Base your answers to questions 70 through 73 on the information below and on your knowledge of chemistry. 

Calcium oxide, \mathrm{CaO}, also known as lime, is an important industrial chemical. Lime can be obtained by the heating of limestone, which is mainly calcium carbonate, \mathrm{CaCO_3}. An equation representing the reaction for the production of lime is shown below. 

\mathrm{CaCO_3(s)+heat → CaO(s)+CO_2(g)}

70.

State the solubility of limestone in water.

71.

State evidence from the equation that the reaction to form lime is endothermic.

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 \mathrm{CaCO_3}.

73.

State the type of chemical bonding in a sample of \mathrm{CaO}.

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 \mathrm{HCl(aq)} of unknown concentration into a flask. The solution is titrated with 0.10 M \mathrm{KOH(aq)} until the \mathrm{HCl(aq)} is exactly neutralized. At the end of the titration, the volume of \mathrm{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 \mathrm{H^+(aq)} ions to the number of moles of \mathrm{OH^-(aq)} ions in the titration mixture when the \mathrm{HCl(aq)} is exactly neutralized by the \mathrm{KOH(aq)}.

75.

Determine the concentration of the HCl(aq) solution using the titration data.

_______ M

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.

77.

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

_______  and _______ 

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.

79.

Compare the number of electrons lost by the Mg(s) placed in the \mathrm{Zn^{2+}(aq)} solution to the number of electrons gained by the \mathrm{Zn^{2+}(aq)}.

80.

In the Show Your Work space, write a balanced, half-reaction equation for the reduction of the copper ions.

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.

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.

83.

In the Show Your Work space, draw a structural formula for 1-bromopropane.

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.

^1_0\mathrm{n}+^{235}_{92}\mathrm{U}\rightarrow^{90}_{38}\mathrm{Sr}+^{142}_{54}\mathrm{Xe}+4^1_0\mathrm{n}+\mathrm{energy}

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.

85.

Determine the time required for an 8.00-mg sample of \mathrm{Sr-90} to decay until only 2.00 mg of the sample remains unchanged.

_______  y

2022 (Aug.): NY Regents - Chemistry