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2023: NY Regents - Chemistry

By Sara Cowley
Last updated 5 months ago
85 Questions
Note from the author:
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.

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

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

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

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

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

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

Which element has chemical properties most similar to sodium?

Which substance contains elements chemically combined in a fixed proportion?

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?

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

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?

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

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

Which sample of matter is a mixture?

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

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

Which process represents a chemical change?

Which equation represents a physical equilibrium?

Systems in nature tend to undergo changes toward

Which formula represents a hydrocarbon?

Which statement describes the bonding in an alkyne molecule?

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

Which term identifies a type of organic reaction?

In an electrochemical cell, oxidation occurs at the

Which energy conversion occurs in an operating electrolytic cell?

One acid-base theory states that a base is an

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

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

Which nuclear emission has the greatest mass?

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

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

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?

Which formula represents chromium(III) oxide?

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?

Which equation represents conservation of atoms?

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

Given the equation representing a reaction:

2NaCl \rightarrow 2Na + Cl2

Which type of reaction does this equation represent?

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

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

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

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?

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

Which particle diagram represents one substance, only?

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

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

Which formula represents 2-butene?

Given a formula representing a compound:

Which formula represents an isomer of the compound?

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.

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

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.

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

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

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.

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

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

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

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.

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.

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

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.

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.

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

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

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.

Determine the pH value of sample 2.

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

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

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.
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.

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

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

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.

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

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

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.

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

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

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

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.

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

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.


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

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

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

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.


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

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.

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

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

Identify the particle represented by X in equation 3.

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