100 Ways to Pass the Chemistry Regents

Multiple Choice

Matter is classified as a

• substance, only

• substance or as a mixture of substances

• homogenous mixture, only

• homogenous mixture or as a heterogeneous mixture

Multiple Choice

A compound is a substance composed of two or more elements that are

• physically mixed in a fixed proportion

• physically mixed in a variable proportion

• chemically combined in a fixed proportion

• chemically combined in a variable proportion

Multiple Choice

In a chemical reaction, there is conservation of

• energy, volume, and mass

• energy, volume, and charge

• mass, charge, and energy

• mass, charge, and volume

Multiple Choice

Which statement describes a chemical property of iron?

• Iron can be flattened into sheets.

• Iron conducts electricity and heat.

• Iron combines with oxygen to form rust.

• Iron can be drawn into a wire.

Multiple Choice

Which substance can be broken down by chemical means?

• ammonia

• aluminum

• antimony

• argon

Multiple Choice

Equal amounts of ethanol and water are mixed at room temperature and at

101.3 kPa. Which process is used to separate ethanol from the mixture?

• distillation

• reduction

• filtration

• ionization

Multiple Choice

A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different

• boiling points

• densities

• particle size

• solubilities

Multiple Choice

At STP, solid carbon can exist as graphite or as diamond. These two forms of carbon have

• the same properties and the same crystal structures

• the same properties and different crystal structures

• different properties and the same crystal structures

• different properties and different crystal structures

Multiple Choice

According to the kinetic molecular theory for an ideal gas, all gas particles

• are in random, constant, straight-line motion

• are separated by very small distances relative to their sizes

• have strong intermolecular forces

• have collisions that decrease the total energy of the system

Multiple Choice

According to the kinetic molecular theory, which statement describes the particles of an ideal gas?

• The gas particles are arranged in a regular pattern.

• The force of attraction between the gas particles is strong.

• The gas particles are hard spheres in continuous circular motion.

• The collisions of the gas particles may result in the transfer of energy.

Multiple Choice

Under which conditions of temperature and pressure does carbon dioxide gas behave most like an ideal gas?

• low temperature and low pressure

• low temperature and high pressure

• high temperature and low pressure

• high temperature and high pressure

Multiple Choice

Under which conditions of temperature and pressure would a 1-liter sample of a real gas behave most like an ideal gas?

• 100 K and 0.1 atm

• 100 K and 10 atm

• 500 K and 0.1 atm

• 500 K and 10 atm

Multiple Choice

The amount of randomness of the atoms in a system is an indication of the

• entropy of the system

• polarity of the system

• excited state of the atoms

• ground state of atoms

Multiple Choice

Chemical systems in nature tend to undergo changes toward

• lower energy and lower entropy

• lower energy and higher entropy

• higher energy and lower entropy

• higher energy and higher entropy

Multiple Choice

The entropy of a sample of carbon dioxide increases as the carbon dioxide changes from

• gas to liquid

• gas to solid

• liquid to solid

• solid to gas

Multiple Choice

At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of NO(g) have

• qual masses and the same number of molecules

• different masses and a different number of molecules

• equal volumes and the same number of molecules

• different volumes and a different number of molecules

Multiple Choice

According to Reference Table H, what is the vapor pressure of propanone at 45°C?

• 22 kPa

• 33 kPa

• 70 kPa

• 98 kPa

Multiple Choice

The temperature of a sample of matter is a measure of the

• average potential energy of the particles of the sample

• average kinetic energy of the particles of the sample

• total nuclear energy of the sample

• total thermal energy of the sample

Multiple Choice

A few pieces of dry ice (solid carbon dioxide), at -78°C are placed in a flask that contains air at 21°C. The flask is sealed by placing an uninflated balloon over the mouth of the flask. As the balloon inflates, the dry ice disappears and no liquid is observed in the flask.

State the direction of heat flow that occurs between the dry ice and the air in the flask.

• flask to the air

• air to the flask

Multiple Choice

At standard pressure, which element has a melting point higher than standard temperature?

• $$F_2$$

• $$Br_2$$

• $$Fe$$

• $$Hg$$

Multiple Choice

In which process does a solid change directly into a vapor?

• condensation

• deposition

• solidification

• sublimation

Multiple Choice

According to the wave-mechanical model, an orbital is defined as the most probable location of

• a proton

• a neutron

• a positron

• an electron

Multiple Choice

Which statement describes the location of two types of subatomic particles in a helium atom?

• Protons and neutrons are located in the nucleus.

• Protons and neutrons are located outside the nucleus.

• Protons and electrons are located in the nucleus.

• Protons and electrons are located outside the nucleus.

Multiple Choice

What is the charge of the nucleus of a copper atom?

• +1

• +2

• +29

• +64

Multiple Choice

An atom that contains six protons, six neutrons, and six electrons has a mass of approximately

• 12 u

• 12 g

• 18 u

• 18 g

Multiple Choice

Positrons and beta particles have

• the same charge and the same mass

• the same charge and different masses

• different charges and the same mass

• different charges and different masses

Multiple Choice

An atom is electrically neutral because the

• number of protons equals the number of electrons

• number of protons equals the number of neutrons

• ratio of the number of neutrons to the number of electrons is 1:1

• ratio of the number of neutrons to the number of protons is 2:1

Multiple Choice

If two atoms are isotopes of the same element, the atoms must have

• the same number of protons and the same number of neutrons

• the same number of protons and a different number of neutrons

• a different number of protons and the same number of neutrons

• a different number of protons and a different number of neutrons

Multiple Choice

The atomic mass of an element is the weighted average of the

• number of protons in the isotopes of that element

• number of neutrons in the isotopes of that element

• atomic numbers of the naturally occurring isotopes of that element

• atomic masses of the naturally occurring isotopes of that element

Multiple Choice

The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of bromine.

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

• (78.92 u)(50.69) + (80.92 u)(49.31)

• (78.92 u)(49.31) + (80.92 u)(50.69)

• (78.92 u)(0.5069) + (80.92 u)(0.4931)

• (78.92 u)(0.4931) + (80.92 u)(0.5069)

Multiple Choice

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

• 2–8–8

• 2–8–8–2

• 2–7–8–1

• 2–7–8–3

Multiple Choice

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

• 2-1

• 2-7-4

• 2-8-7

• 2-4

Multiple Choice

When an excited electron in an atom moves to the ground state, the electron

• absorbs energy as it moves to a higher energy state

• absorbs energy as it moves to a lower energy state

• emits energy as it moves to a higher energy state

• emits energy as it moves to a lower energy state

Multiple Choice

Which electron transition in an excited atom results in a release of energy?

• first shell to the third shell

• second shell to the fourth shell

• third shell to the fourth shell

• fourth shell to the second shell

Multiple Choice

A specific amount of energy is emitted when excited electrons in an atom in a sample of an element return to the ground state. This emitted energy can be used to determine the

• mass of the sample

• volume of the sample

• identity of the element

• number of moles of the element

Multiple Choice

Given the bright-line spectra of three elements and the spectrum of a mixture formed from at least two of these elements:

Which elements are present in this mixture?

• E and D, only

• E and G, only

• D and G, only

• D, E, and G

Multiple Choice

Which type of reaction occurs when a high energy particle collides with the nucleus of an atom, converting that atom to an atom of a different element?

• addition

• neutralization

• substitution

• transmutation

Multiple Choice

Which nuclear equation represents a natural transmutation?

• Choice 1

• Choice 2

• Choice 3

• Choice 4

Multiple Choice

Which radioisotopes have the same decay mode and have half-lives greater than 1 hour?

• Au-198 and N-16

• Ca-37 and Fe-53

• I-131 and P-32

• Tc-99 and U233

Multiple Choice

The amount of energy released from a fission reaction is much greater than the energy released from a chemical reaction because in a fission reaction

• mass is converted into energy

• energy is converted into mass

• ionic bonds are broken

• covalent bonds are broken

Multiple Choice

In which type of reaction do two lighter nuclei combine to form one heavier nucleus?

• combustion

• reduction

• nuclear fission

• nuclear fusion

Multiple Choice

Which balanced equation represents nuclear fusion?

• Choice 1

• Choice 2

• Choice 3

• Choice 4

Multiple Choice

Which type of nuclear reaction is represented by the equation?

• fission

• fusion

• beta decay

• alpha decay

Multiple Choice

A nuclear fission reaction and a nuclear fusion reaction are similar because both reactions

• form heavy nuclides from light nuclides

• form light nuclides from heavy nuclides

• release a large amount of energy

• absorb a large amount of energy

Multiple Choice

Which radioisotope is used to determine the age of once-living organisms?

• carbon-14

• cobalt-60

• iodine-131

• uranium-238

Multiple Choice

Which nuclide is used to investigate human thyroid gland disorders

• carbon-14

• potassium-37

• cobalt-60

• iodine-131

Multiple Choice

Which radioactive isotope is used in treating cancer?

• carbon-14

• cobalt-60

• lead-208

• uranium-239

Multiple Choice

One benefit of nuclear fission reactions is

• nuclear reactor meltdowns

• storage of waste materials

• biological exposure

• production of energy

Multiple Choice

On the present Periodic Table of the Elements, the elements are arranged according to increasing

• number of oxidation states

• number of neutrons

• atomic mass

• atomic number

Multiple Choice

What is a property of most metals?

• hey tend to gain electrons easily when bonding.

• They tend to lose electrons easily when bonding.

• They are poor conductors of heat.

• high electronegativities

Multiple Choice

The high electrical conductivity of metals is primarily due to

• high ionization energies

• filled energy levels

• mobile electrons

• high electronegativities

Multiple Choice

Which two characteristics are associated with metals?

• low first ionization energy and low electronegativity

• first ionization energy and high electronegativity

• high first ionization energy and low electronegativity

• high first ionization energy and high electronegativity

Multiple Choice

In the ground state, an atom of which element has seven valence electrons?

• sodium

• phosphorus

• nitrogen

• fluorine

Multiple Choice

Which list of elements consists of a metal, a metalloid, and a nonmetal?

• Li, Na, Rb

• Cr, Mo, W

• Sn, Si, C

• O, S, Te

Multiple Choice

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

• Be, Si, Cl, Kr

• C, N, Ne, Ar

• K, Fe, B, F

• Na, Zn, As, Sb

Multiple Choice

Strontium and barium have similar chemical properties because atoms of these elements have the same number of

• protons

• neutrons

• electron shells

• valence electrons

Multiple Choice

When an atom of lithium loses an electron, the atom becomes a

• negative ion with a radius smaller than the radius of the atom

• negative ion with a radius larger than the radius of the atom

• positive ion with a radius smaller than the radius of the atom

• positive ion with a radius larger than the radius of the atom

Multiple Choice

What occurs when an atom of chlorine forms a chloride ion?

• The chlorine atom gains an electron, and its radius becomes smaller

• The chlorine atom gains an electron, and its radius becomes larger.

• The chlorine atom loses an electron, and its radius becomes smaller.

• The chlorine atom loses an electron, and its radius becomes larger

Multiple Choice

Which term indicates how strongly an atom attracts the electrons in a chemical bond?

• alkalinity

• atomic mass

• electronegativity

• activation energy

Multiple Choice

The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as

• first ionization energy

• activation energy

• conductivity

• electronegativity

Multiple Choice

What occurs when an atom of chlorine and an atom of hydrogen become a molecule of hydrogen chloride?

• A chemical bond is broken and energy is released.

• A chemical bond is broken and energy is absorbed.

• A chemical bond is formed and energy is released.

• A chemical bond is formed and energy is absorbed.

Multiple Choice

What occurs when potassium reacts with chlorine to form potassium chloride?

• Electrons are shared and the bonding is ionic.

• Electrons are shared and the bonding is covalent.

• Electrons are transferred and the bonding is ionic.

• Electrons are transferred and the bonding is covalent.

Multiple Choice

Which elements can react to produce a molecular compound?

• calcium and chlorine

• hydrogen and sulfur

• lithium and fluorine

• magnesium and oxygen

Multiple Choice

Which type of bonding is found in all molecular substances?

• covalent bonding

• hydrogen bonding

• ionic bonding

• metallic bonding

Multiple Choice

Which statement explains why a C–O bond is more polar than a F–O bond?

• At STP, carbon has a greater density than fluorine.

• A carbon atom has more valence electrons than a fluorine atom.

• The difference in electronegativity between carbon and oxygen is greater than that between fluorine and oxygen.

• The difference in first ionization energy between carbon and oxygen is greater than that between fluorine and oxygen.

Multiple Choice

Which formula represents a nonpolar molecule containing polar covalent bonds?

• Choice 1

• Choice 2

• Choice 3

• Choice 4

Multiple Choice

The relatively high boiling point of water is due to water having

• hydrogen bonding

• metallic bonding

• nonpolar covalent bonding

• strong ionic bonding

Multiple Choice

Hydrogen bonding is a type of

• strong covalent bond

• weak ionic bond

• strong intermolecular force

• weak intermolecular force

Multiple Choice

Which compound has hydrogen bonding between its molecules?

• CH₄

• CaH₂

• KH

• NH₃

Multiple Choice

Which type of bonding is present when valence electrons move within the sample?

• metallic bonding

• hydrogen bonding

• covalent bonding

• ionic bonding

Multiple Choice

Which list consists of types of chemical formulas?

• atoms, ions, molecules

• metals, nonmetals, metalloids

• empirical, molecular, structural

• synthesis, decomposition, neutralization

Multiple Choice

Which formula is an empirical formula?

• CH₄

• C₂H₆

• C₃H₆

• C₄H₁₀

Multiple Choice

Which type of chemical reaction is represented by this equation?

• synthesis

• decomposition

• single replacement

• double replacement

• combustion

Multiple Choice

Which types of chemical reactions are represented by these equations?

• single replacement and decomposition

• single replacement and double replacement

• synthesis and decomposition

• synthesis and double replacement

Multiple Choice

Which type of chemical reaction is represented by this equation?

• synthesis

• decomposition

• single replacement

• double replacement

• combustion

Multiple Choice

What is the chemical formula for copper(II) hydroxide?

• CuOH

• CuOH₂

• Cu₂(OH)

• Cu(OH)₂

Multiple Choice

At 298 K and 1 atm, which noble gas has the lowest density?

• Ne

• Kr

• Xe

• Rn

Multiple Choice

In a laboratory activity, the density of a sample of vanadium is determined to be 6.9 g/cm3 at room temperature. What is the percent error for the determined value?

• 0.15%

• 0.87%

• 13%

• 15%

Multiple Choice

If 46 grams of Na and 71 grams of Cl2 react completely, what is the total mass of NaCl produced?

• 58.5 g

• 117 g

• 163 g

• 234 g

Multiple Choice

The molar mass of Ba(OH)₂

• 154.3 g

• 155.3 g

• 171.3 g

• 308.6 g

Math Response

Calculate the percent composition by mass of water in CaSO₄ • 2H₂O.

__%

Type answer here

Correct Answer: 21

Deg^°

Rad

Multiple Choice

A hydrate is a compound that includes water molecules within its crystal structure. During an experiment to determine the percent by mass of water in a hydrated crystal, a student found the mass of the hydrated crystal to be 4.10 grams. After heating to constant mass, the mass was 3.70 grams. What is the percent by mass of water in this crystal?

• 90. 90%

• 11%

• 9.8%

• 0.40%

Multiple Choice

What is the total number of moles of O₂(g) that must react completely with 5.00 moles of C₄H₁₀(g)?

• 10.0

• 20.0

• 26.5

• 32.5

Multiple Choice

What is the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH?

• 0.5 M

• 2 M

• 8 M

• 80 M

Multiple Choice

At standard pressure, how do the boiling point and the freezing point of NaCl(aq) compare to the boiling point and the freezing point of H₂O(ℓ)?

• Both the boiling point and the freezing point of NaCl(aq) are lower.

• Both the boiling point and the freezing point of NaCl(aq) are higher.

• The boiling point of NaCl(aq) is lower, and the freezing point of NaCl(aq) is higher.

• The boiling point of NaCl(aq) is higher, and the freezing point of NaCl(aq) is lower.

Multiple Choice

A 5.0-gram sample of Fe(s) is to be placed in 100. milliliters of HCl(aq). Which changes will result in the fastest rate of reaction?

• increasing the surface area of Fe(s) and increasing the concentration of HCl(aq)

• increasing the surface area of Fe(s) and decreasing the concentration of HCl(aq

• decreasing the surface area of Fe(s) and increasing the concentration of HCl(aq)

• decreasing the surface area of Fe(s) and decreasing the concentration of HCl(aq)

Multiple Choice

A chemical reaction occurs when reactant particles

• are separated by great distances

• have no attractive forces between them

• collide with proper energy and proper orientation

• convert chemical energy into nuclear energy

Multiple Choice

Which term is defined as the difference between the potential energy of the products and the potential energy of the reactants in a chemical reaction?

• activation energy

• thermal energy

• heat of fusion

• heat of reaction

Multiple Choice

Each interval on the axis labeled “Potential Energy (kJ/mol)” represents 10. kilojoules per mole. What is the activation energy of the forward reaction?

• 10. 10. kJ/mol

• 30. 30 kJ/mol

• 40. 40. kJ/mol

• 60. kJ/mol

Multiple Choice

Determine if the reaction is endothermic or exothermic.

• 10. endothermic

• 30. exothermic

Multiple Choice

Addition of a catalyst can speed up a reaction by providing an alternate reaction pathway that has a

• lower activation energy

• higher activation energy

• lower heat of reaction

• higher heat of reaction

Multiple Choice

Some solid KNO₃ remains at the bottom of a stoppered flask containing a saturated KNO₃(aq) solution at 22°C. Which statement explains why the contents of the flask are at equilibrium?

• The rate of dissolving is equal to the rate of crystallization.

• The rate of dissolving is greater than the rate of crystallization.

• The concentration of the solid is equal to the concentration of the solution

• The concentration of the solid is greater than the concentration of the solution.

Multiple Choice

Which statement must be true when solution equilibrium occurs?

• The solution is at STP.

• The solution is supersaturated.

• The concentration of the solution remains constant.

• The masses of the dissolved solute and the undissolved solute are equal.

Multiple Choice

Which type of substance yields hydrogen ions, H⁺, in an aqueous solution?

• an Arrhenius acid

• an Arrhenius base

Multiple Choice

Which statement describes one acid-base theory?

• An acid is an H⁺ acceptor, and a base is an H⁺ donor.

• An acid is a H⁺ donor, and a base is an H⁺ acceptor

Multiple Choice

Which type of reaction occurs when an Arrhenius acid reacts with an Arrhenius base to form a salt and water?

• combustion

• decomposition

• neutralization

• saponification

Multiple Choice

Which indicator is blue in a solution that has a pH of 5.6?

• bromcresol green

• bromthymol blue

• methyl orange

• thymol blue

Multiple Choice

Which process uses a volume of solution of known concentration to determine the concentration of another solution?

• distillation

• substitution

• transmutation

• titration

Multiple Choice

Which statement describes an electrolyte?

• An electrolyte conducts an electric current as a solid and dissolves in water.

• An electrolyte conducts an electric current as a solid and does not dissolve in water.

• When an electrolyte dissolves in water, the resulting solution conducts an electric current.

• When an electrolyte dissolves in water, the resulting solution does not conduct an electric current.

Multiple Choice

When a sample of Mg(s) reacts completely with O₂(g), the Mg(s) loses 5.0 moles of electrons. How many moles of electrons are gained by the O₂(g)?

• 1.0 M

• 2.5 M

• 5.0 M

• 10.0 M

Multiple Choice

Which metal reacts spontaneously with NiCl₂(aq)?

• Au(s)

• Cu(s

• Sn(s)

• Zn(s)

Multiple Choice

Which energy change occurs in an operating voltaic cell?

• chemical to electrical

• electrical to chemical

• chemical to nuclear

• nuclear to chemical

Multiple Choice

What is the direction of electron flow in the external circuit in this operating cell.

• Cu(s) electrode to Ag(s) electrode

• Ag(s) electrode to Cu(s) electrode

Multiple Choice

Which statement describes the reactions in an electrochemical cell (voltaic and electrolytic)?

• Oxidation occurs at the anode, and reduction occurs at the cathode.

• Oxidation occurs at the cathode, and reduction occurs at the anode.

• Oxidation and reduction both occur at the cathode.

• Oxidation and reduction both occur at the anode.

Multiple Choice

An electrolytic cell differs from a voltaic cell because an electrolytic cell

• generates its own energy from a spontaneous physical reaction

• generates its own energy from a nonspontaneous physical reaction

• requires an outside energy source for a spontaneous chemical reaction to occur

• requires an outside energy source for a nonspontaneous chemical reaction to occur

Multiple Choice

When a voltaic cell operates, ions move through the

• anode

• cathode

• salt bridge

• external circuit (wire)

Multiple Choice

All organic compounds must contain the element

• phosphorus

• oxygen

• carbon

• nitrogen

Multiple Choice

The only two elements in alkenes and alkynes are

• carbon and nitrogen

• carbon and hydrogen

• oxygen and nitrogen

• oxygen and hydrogen

Multiple Choice

This compound is classified as an

• aldehyde

• alkene

• alkyne

• alcohol

Multiple Choice

Which formula represents an alkene?

• C₂H₆

• C₃H₆

• C₄H₁₀

• C₅H₁₂

Multiple Choice

Which formula represents an unsaturated hydrocarbon?

• C₂H₄

• C₃H₈

• C₄H₁₀

• C₅H₁₂

Multiple Choice

Which formula represents an unsaturated hydrocarbon?

Multiple Choice

An alcohol and an ether have the same molecular formula, C₂H₆O. These two compounds have

• the same functional group and the same physical and chemical properties

• the same functional group and different physical and chemical properties

• different functional groups and the same physical and chemical properties

• different functional groups and different physical and chemical properties

Multiple Choice

Which class of organic compounds has molecules that contain nitrogen atoms?

• alcohol

• amine

• ether

• ketone

Multiple Choice

The organic compound represented by the condensed structural formula CH₃CH₂CH₂CHO is classified as an

• alcohol

• aldehyde

• ester

• ether

Multiple Choice

This compound is classified as an

• amide

• amine

• aldehyde

• alcohol

Multiple Choice

Which organic-compound classes are represented by these structural formulas, as shown from left to right?

• ester, organic acid, ketone

• ester, aldehyde, organic acid

• ketone, aldehyde, alcohol

• ketone, organic acid, alcohol

Multiple Choice

What is the IUPAC name of the compound with the following structural formula?

• propanone

• propanal

• butanone

• butanal

Multiple Choice

The isomers butane and methylpropane have

• the same molecular formula and the same properties

• the same molecular formula and different properties

• different molecular formulas and the same properties

• different molecular formulas and different properties

Multiple Choice

Which formulas represent compounds that are isomers of each other?

Multiple Choice

Which type of reaction is represented by the equation below?

• esterification

• fermentation

• saponification

• polymerization

Multiple Choice

A reaction between an alcohol and an organic acid is classified as

• fermentation

• esterification

• saponification

• substitution

Multiple Choice

Which reaction results in the production of soap?

• esterification

• fermentation

• polymerization

• saponification

Multiple Choice

Which type of organic reaction produces both water and carbon dioxide?

• addition

• combustion

• esterification

• fermentation

Multiple Choice

Which type of reaction is represented by this equation?

• fermentation

• addition

• substitution

• polymerization

Multiple Choice

This reaction is best described as

• addition involving a saturated hydrocarbon

• addition involving an unsaturated hydrocarbon

• substitution involving a saturated hydrocarbon

• substitution involving an unsaturated hydrocarbon