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2023: NY Regents - Chemistry

Last updated 3 months ago

85 questions

Note from the author:

Instructions

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From the New York State Education Department. The University of the State of New York Regents High School Examination Physical Setting Chemistry January 2023. Internet. Available from https://www.nysedregents.org/Chemistry/123/chem12023-exam.pdf; accessed 3, May, 2023.

From the New York State Education Department. The University of the State of New York Regents High School Examination Physical Setting Chemistry January 2023. Internet. Available from https://www.nysedregents.org/Chemistry/123/chem12023-exam.pdf; accessed 3, May, 2023.

Scroll through the document embedded here to access the 2011 Edition Reference Tables for Physical Setting/Chemistry.

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Question 49

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Question 50

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Directions (51-65): Record your answers in the spaces provided. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

Question 51

51.

Explain, in terms of neutrons and protons, why P-32 and P-31 are different isotopes of phosphorus.

Question 52

52.

Determine the oxidation state of chromium in K2CrO4.

Base your answers to questions 53 and 54 on the information below and on your knowledge of chemistry.

The first four elements in Group 14 are carbon, silicon, germanium, and tin. These elements form compounds with chlorine that have similar formulas. Two examples of these formulas are silicon tetrachloride, SiCl4, and germanium tetrachloride, GeCl4.

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Base your answers to questions 55 through 57 on the information below and on your knowledge of chemistry.

The equation to the left represents the reaction between ammonia and hydrogen chloride.

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S4.KI.5.2a

Base your answers to questions 58 through 60 on the information below and on your knowledge of chemistry. 

A sample of helium gas, \mathrm{He(g)}, is placed in a rigid cylinder sealed with a movable piston. The temperature of the helium is 25.0°C. The volume of the helium is 300. milliliters and the pressure is 0.500 atmosphere.

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Base your answers to questions 61 and 62 on the information below and on your knowledge of chemistry. 

During a laboratory activity, a student places 21.0 mL of hydrochloric acid solution, \mathrm{HCl(aq)}, of unknown concentration into a flask. The solution is titrated with 0.125 M \mathrm{NaOH(aq)} until the acid is exactly neutralized. The volume of \mathrm{NaOH(aq)} added is 18.5 milliliters. During this laboratory activity, appropriate safety equipment is used and safety procedures are followed.

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Base your answers to questions 63 through 65 on the information below and on your knowledge of chemistry. 

The table below lists the hydronium ion concentration and pH values of four different solutions and distilled water. The pH value is missing for sample 2.

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Directions (66-85): Record your answers in the spaces provided. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

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Base your answers to questions 77 through 79 on the information below and on your knowledge of chemistry. 

Before the year 1828, it was thought that organic compounds were produced only by living organisms and that inorganic compounds were made from nonliving substances. Urea is an organic compound. In 1828, a chemist heated ammonium cyanate and produced urea, which is very soluble in water. The equation below represents this reaction.

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Base your answers to questions 80 and 81 on the information below and on your knowledge of chemistry. 

When a voltmeter is connected in the circuit of a voltaic cell, an electrical measurement called voltage can be read on the meter. The voltage of the cell is affected if the concentration of the solute in the half-cells is changed. The diagram, the ionic equation, and the graph below represent a copper-zinc cell. When the switch is closed, electricity flows through the circuit as the cell operates at constant temperature.

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Which conclusion was developed as a result of the gold foil experiment?

Atoms are mostly empty space.

All atoms are hard, indivisible spheres.

Atoms have different volumes.

All atoms have the same volume.

Which two particles each have a mass approximately equal to one atomic mass unit?

positron and proton

positron and electron

neutron and electron

neutron and proton

An excited potassium atom emits a specific amount of energy when one of its electrons moves from

the first shell to the fourth shell

the second shell to the fourth shell

the fourth shell to the fifth shell

the fourth shell to the second shell

Which list of elements includes a metal, a metalloid, and a noble gas?

Rb, Cl, Ne

Sr, Si, Rn

Rn, Cl, Ne

Si, Rb, Sr

Which element has the lowest density at 298 K and 101.3 kPa?

argon

flourine

nitrogen

oxygen

Which phrase describes the crystal structure and properties of two different forms of solid carbon called diamond and graphite?

same crystal structure and same properties

same crystal structure and different properties

different crystal structures and different properties

different crystal structures and same properties

Which element has chemical properties most similar to sodium?

magnesium

oxygen

phosphorus

rubidium

Which substance contains elements chemically combined in a fixed proportion?

magenese

methane

silicon

strontium

Which property can be used to differentiate between a 50.-gram sample of solid potassium nitrate at STP and a 50.-gram sample of solid silver chloride at STP?

mass

temperature

phase

solubility

Which type of bond forms when electrons are equally shared between two atoms?

a polar covalent bond

a nonpolar covalent bond

a hydrogen bond

an ionic bond

Which statement describes the changes in bonding and energy that occur when a molecule of iodine, \mathrm{I_2}, forms two separate atoms of iodine?

A bond is formed as energy is absorbed.

A bond is formed as energy is released.

A bond is broken as energy is absorbed.

A bond is broken as energy is released.

The degree of polarity in the bond between a hydrogen atom and an oxygen atom in a molecule of water can be assessed using the difference in

densities

electronegativities

melting points

intermolecular forces

Which substance can not be broken down by a chemical change?

ammonia

ethanol

krypton

water

Which sample of matter is a mixture?

\mathrm{CO_{2}(g)}

\mathrm{CCl_{4}}(\ell)

\mathrm{MgCl_{2}(aq)}

\mathrm{Sn(s)}

Which term is used to express the concentration of an aqueous solution?

parts per million

heat of fusion

pressure at 0 celsius

volume at 0 celsius

The particles in which sample have the lowest average kinetic energy?

50. g of sulfur at 273 K

40. g of aluminum at 298 K

30. g of sulfur at 303 K

20. g of aluminum at 323 K

Which process represents a chemical change?

Iodine sublimes.

Water evaporates.

An ice cube melts.

A candle burns in air

Which equation represents a physical equilibrium?

Systems in nature tend to undergo changes toward

higher energy and higher entropy

higher energy and lower entropy

lower energy and higher entropy

lower energy and lower entropy

Which formula represents a hydrocarbon?

C2H6

C2H5OH

C2H5Cl

C2H6O

Which statement describes the bonding in an alkyne molecule?

There is at least one carbon-to-carbon double bond.

There is at least one carbon-to-carbon triple bond

There is at least one carbon-to-oxygen single bond.

There is at least one carbon-to-oxygen double bond.

Which compound has a functional group that contains two oxygen atoms?

1-propanamine

2-chloropropane

methyl propanoate

methyl ethyl ether

Which term identifies a type of organic reaction?

deposition

distillation

polymerization

vaporization

In an electrochemical cell, oxidation occurs at the

anode

cathode

salt bridge

switch

Which energy conversion occurs in an operating electrolytic cell?

chemical energy to electrical energy

electrical energy to chemical energy

nuclear energy to electrical energy

electrical energy to nuclear energy

One acid-base theory states that a base is an

H- donor

H- acceptor

H+ donor

H+ acceptor

The acidity or alkalinity of a solution can be measured by its

pH value

electronegativity value

boiling point

freezing point

When the nucleus of an atom of neon-19 decays, which particle is emitted?

^{4}_{2}\mathrm{He}

^{0}_{-1}\mathrm{e}

^{1}_{0}\mathrm{n}

_{+1}^{0}\mathrm{e}

Which nuclear emission has the greatest mass?

positron

gamma ray

beta particle

alpha particle

Which statement describes the net change that occurs during nuclear fission?

Electrons are converted to protons.

Protons are converted to electrons.

Mass is converted to energy

Energy is converted to mass.

What is the net charge of a monatomic ion that has 15 protons, 16 neutrons, and 18 electrons?

2+

2-

3+

3-

The table below shows the atomic masses and natural abundances of the two naturally occurring isotopes of rhenium.

Which general trend is observed as the elements in Period 2 are considered from left to right?

Atomic mass decreases.

Melting point increases.

Electronegativity increases

First ionization energy decreases.

Which formula represents chromium(III) oxide?

CrO3

Cr3O

Cr2O3

Cr3O2

Given the balanced equation representing a reaction:
2KClO3 + energy \rightarrow 2KCl + 3O2

What is the mass of KCl produced when 24.51 grams of KClO3 reacts completely to produce 9.60 grams of O2?

5.31g

14.91g

34.11g

43.71g

Which equation represents conservation of atoms?

One mole of bromine gas, Br2, has a mass of

35.0 g

70.0 g

79.9 g

159.8 g

Given the equation representing a reaction:

2NaCl \rightarrow 2Na + Cl2

Which type of reaction does this equation represent?

double replacement

decomposition

synthesis

single replacement

Which statement describes the charge and the radius of the magnesium ion formed when a magnesium atom loses two electrons?

The Mg ion is positive and has a radius larger than the Mg atom.

The Mg ion is negative and has a radius larger than the Mg atom

The Mg ion is positive and has a radius smaller than the Mg atom.

The Mg ion is negative and has a radius smaller than the Mg atom

An oxide ion, O2- has the same electron configuration as an atom of which noble gas?

helium

neon

argon

krypton

What is the vapor pressure of propanone at 45 degrees celsius?

21 kPa

60. kPa

70. kPA

79 kPa

Based on Table G, what is the mass of \mathrm{KCl} that must be dissolved in 200. grams of H2O at 10.\degree\mathrm{C} to make a saturated solution?

15g

30.g

60.g

120.g

Based on Table I, which chemical equation represents a reaction with a heat of reaction that indicates a net release of energy?

The greatest increase in entropy occurs when a 1.00-gram sample of water changes from

solid to liquid

solid to gas

gas to liquid

liquid to solid

Which particle diagram represents one substance, only?

Based on Table J, atoms of which metal will lose electrons to \mathrm{Ca}^{2+} ions?

aluminum

lead

nickel

potassium

Which aqueous solution is the best conductor of an electrical current?

Given the equation representing a reaction:

^2_1\mathrm{H}+ ^3_1\mathrm{H}\rightarrow^4_2\mathrm{He}+ ^1_0\mathrm{n}
 
This equation represents

sublimation

condensation

fission

fusion

Which formula represents 2-butene?

Given a formula representing a compound: 

Which formula represents an isomer of the compound?

Question 53

53.

State the general trend in atomic radius as these four elements are considered in order of increasing atomic number.

Question 54

54.

State, in terms of electron configuration, why silicon and germanium both form tetrachloride compounds.

Question 55

55.

Explain, in terms of distribution of charge, why a molecule of compound 1 is polar.

Question 56

56.

Draw a Lewis electron-dot diagram for a molecule of compound 2.

Question 57

57.

Identify the two types of chemical bonds in the product of this reaction.

Question 58

58.

State, in terms of the average distance between the helium atoms, why the density of the gas increases when the piston is pushed farther into the rigid cylinder.

Question 59

59.

Determine the volume of the helium gas when the pressure is increased to 1.50 atm and the temperature remains at 25.0°C.

Question 60

60.

Compare the number of helium atoms in the cylinder at a pressure of 0.500 atm to the number of helium atoms in the cylinder when the pressure is increased to 1.50 atm by pushing the piston in.

Question 61

61.

Explain, in terms of ions, why the hydrochloric acid solution can conduct an electric current.

Question 62

62.

Determine the concentration of the \mathrm{HCl(aq)} solution, using the titration data.

Question 63

63.

Determine the pH value of sample 2.

Question 64

64.

Identify the ion released by the compound dissolved in sample 4 that allows the compound to be classified as an Arrhenius base.

Question 65

65.

State how many times greater the hydronium ion concentration is in sample 4 than it is in sample 5.

Base your answers to questions 66 through 68 on the information below and on your knowledge of chemistry. 

Boric acid, H3BO3, is heated to produce tetraboric acid, H2B4O7, and water. The equation below represents the reaction to form tetraboric acid.

The tetraboric acid is then used to make borax, which is used as a cleaning agent. Borax, Na2B4O7.

Question 66

66.

Explain why the formula for tetraboric acid is an empirical formula.

Question 67

67.

Determine the number of moles of boric acid that react in the equation to produce 10 moles of water.

Question 68

68.

Show a numerical setup for calculating the mass, in grams, of a 0.200-mole sample of borax.

Base your answers to questions 69 through 71 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 uses the lab equipment shown in the diagram below to determine the heat of combustion of candle wax.

Heat of combustion is defined as the amount of heat released when a known mass of a substance is burned and can be measured in joules per gram. At the start of the activity, the mass of the candle and the mass of the water are measured. The starting temperature of the water is 5.0°C, and the air temperature in the room is 22.0°C. The candle is lit, and the water is stirred with a stirring rod. Several minutes later, the candle is extinguished, and the student measures the temperature of the water in the can. When the candle is cool, the student measures the final mass of the candle. Lab activity results are shown in the table below.

Question 69

69.

State the number of significant figures used to express the value for the mass of the water in the can.

Question 70

70.

State the direction of the heat flow between the air and the water in the can before the candle is lit.

Question 71

71.

Determine the amount of heat absorbed by the water.

Base your answers to questions 72 through 76 on the information below and on your knowledge of chemistry. 

A process was developed in 1912 to produce ammonia gas from atmospheric nitrogen gas and hydrogen gas. Iron can be used as a catalyst. The equation representing this system at equilibrium is shown below.

Question 72

72.

State evidence from the equation that the forward reaction is exothermic.

Question 73

73.

Compare the rate of the forward reaction to the rate of the reverse reaction at equilibrium.

Question 74

74.

On the labeled axes in the Show Your Work space, draw a potential energy diagram for the forward reaction represented in this equation.

Question 75

75.

State, in terms of moles of gases, why the equilibrium shifts to the right due to an increase in pressure on the system at constant temperature.

Question 76

76.

State what happens to the rate of forward reaction when the iron is added to this system.

Question 77

77.

Identify the element present in urea that is present in all organic compounds.

Question 78

78.

Compare the formula mass of the two compounds in the equation.

Question 79

79.

State, in terms of molecular polarity, why urea is very soluble in water.

Question 80

80.

Based on the graph, determine the voltage of the cell if the Cu(NO3)2(aq) concentration is 1.5M.

Question 81

81.

Write a balanced half-reaction equation for the oxidation of zinc that occurs in this operating cell.

Base your answers to questions 82 through 85 on the information below and on your knowledge of chemistry. 

Synthetic radioisotopes may be made by bombarding other nuclides with neutrons. The equations below represent a sequence of reactions converting stable iron–58 to cobalt–60, which is used in medical treatments.

Question 82

82.

State the neutron to proton ratio for an atom of the ^{58}\mathrm{Fe} in equation 1.

Question 83

83.

State, in terms of elements, why equation 2 represents a transmutation reaction.

Question 84

84.

Identify the particle represented by X in equation 3.

Question 85

85.

Determine the fraction of an original sample of Co-60 that remains unchanged after 15.813 years.