WorksheetsChemistry Mock Regents Review 24-25
Total questions: 85
Worksheet time: 3hrs 50mins
Which proposal in the development of the modern model of the atom was made before the others?
Atoms are hard, indivisible spheres of different sizes.
Atoms are mostly empty space with a small dense nucleus.
Atoms have electrons that have wavelike properties.
Atoms have an internal structure that contains negative particles.
According to the wave-mechanical model, in the ground state, the 10 electrons of a neon atom would be located
in the nucleus
in orbitals
in the first shell
in the valence shell
Which statement describes two different isotopes of carbon?
The isotopes contain the same number of neutrons and have the same atomic number.
The isotopes contain the same number of neutrons but have a different atomic number.
The isotopes contain a different number of neutrons but have the same atomic number.
The isotopes contain a different number of neutrons and have a different atomic number.
An element that is a very reactive metal could have an atomic number of
9
2
19
79
Which element is listed with the number of protons in each of its atoms?
nitrogen, 14
silicon, 14
oxygen, 16
phosphorus, 16
What is the overall charge on the nucleus of a fluorine atom?
-1
-9
+9
+19
As the elements with atomic numbers 11 through 17 are considered in order of increasing atomic number, the classification of the elements changes from
metal to metalloid to nonmetal
metal to nonmetal to metalloid
nonmetal to metalloid to metal
nonmetal to metal to metalloid
At STP, which property can be used to differentiate one-mole samples of Cl2(g) and Kr(g)?
phase
pressure
chemical reactivity
temperature
Two gaseous forms of oxygen are diatomic oxygen, O2, and ozone, O3. These two forms of oxygen have
the same molecular structure and the same properties
the same molecular structure and different properties
different molecular structures and the same properties
different molecular structures and different properties
A compound consists of two or more different elements that are
physically mixed in a fixed proportion
physically mixed in a proportion that can vary
chemically combined in a fixed proportion
chemically combined in a proportion that can vary
Compared to the chemical and physical properties of the compound CO, the compound CO2 has
the same chemical properties and the same physical properties
the same chemical properties and different physical properties
different chemical properties and the same physical properties
different chemical properties and different physical properties
Which phrase describes the molecular polarity of and the charge distribution in an HCl molecule?
nonpolar with an asymmetrical charge distribution
nonpolar with a symmetrical charge distribution
polar with an asymmetrical charge distribution
polar with a symmetrical charge distribution
Which atom forms an ion with a radius larger than the atomic radius?
calcium atom
oxygen atom
lead atom
tin atom
Which sample can be classified as a substance?
air
argon
soil
seawater
A 1.0-gram sample of NaCl(s) is dissolved in 100. grams of water at 25°C, and another 1.0-gram sample of NaCl(s) is dissolved in 50. grams of water at 25°C. Which property of the two resulting mixtures will be different?
color of the components in the mixture
particle size of the components in the mixture
polarity of the components in the mixture
proportion by mass of the components in the mixture
Based on Table G, which compound has the greatest solubility in 100. grams of water at 10.°C?
HCl
NaCl
KCl
NH4Cl
According to the kinetic molecular theory, ideal gas particles
are separated by small distances relative to their size
do not transfer energy when they collide with each other
have attractive forces between them
move in random, constant, straight-line motion
A reaction is most likely to occur when the reacting particles collide with proper orientation and proper
charge
energy
mass
volume
A sample of SO2(g) and a sample of NO2(g) contain the same number of molecules when they have the same
mass, temperature, and volume
mass, temperature, and pressure
pressure, volume, and temperature
pressure, volume, and mass
Which term identifies the strong intermolecular forces found in a sample of liquid water?
ionic bonding
covalent bonding
hydrogen bonding
metallic bonding
Which mathematical expression represents the heat of reaction for a chemical change?
(PE of the products) – (PE of the reactants)
(PE of the products) + (PE of the reactants)
(PE of the products) ÷ (PE of the reactants)
(PE of the products) × (PE of the reactants)
Catalysts can increase the rate of a chemical reaction by providing
an alternate reaction pathway with a higher activation energy
the same reaction pathway with a higher activation energy
an alternate reaction pathway with a lower activation energy
the same reaction pathway with a lower activation energy
Which term represents the disorder of a system?
entropy
mole
quanta
pressure
Which element must be present in all organic compounds?
nitrogen
hydrogen
carbon
sulfur
Based on Table R, which functional group allows a compound to be classified as an organic acid?
(1)
(2)
(3)
(4)
In a voltaic cell, oxidation occurs
at the cathode
at the anode
in the salt bridge
in the external circuit
Which positive ion must be present in an aqueous solution of an Arrhenius acid?
H3O+
Na+
NH4+
Rb+
A change that converts an atom of one element to another element is called
neutralization
oxidation
sublimation
transmutation
Which radiation has the least ionizing power and greatest penetrating power?
alpha particles
beta particles
gamma emissions
positron emissions
Which nuclear emission is listed with its notation?
alpha particle, 1_2p
beta particle, 0_-1e
neutron, 0_0γ
proton, 0_1β
What is represented by diagram 2?
a positive ion of hydrogen
a negative ion of hydrogen
an atom of hydrogen in an excited state
an atom of hydrogen in the ground state
The table below gives the atomic mass and the abundance of the two naturally occurring isotopes of copper. Naturally Occurring Isotopes of Copper Isotope Notation | Atomic Mass of the Isotope (u) | Natural Abundance (%) Cu-63 | 62.93 | 69.15 Cu-65 | 64.93 | 30.85 Which numerical setup can be used to calculate the atomic mass of the element copper?
(1) (62.93 u)(30.85) + (64.93 u)(69.15)
(2) (62.93 u)(69.15) + (64.93 u)(30.85)
(3) (62.93 u)(0.3085) + (64.93 u)(0.6915)
(4) (62.93 u)(0.6915) + (64.93 u)(0.3085)
Which subatomic particles were discovered as the result of experiments with cathode ray tubes?
electrons
neutrons
positrons
protons
Which change in electron location in an atom of calcium is accompanied by the greatest amount of energy emitted?
from shell 1 to shell 2
from shell 2 to shell 1
from shell 1 to shell 4
from shell 4 to shell 1
As the atomic number increases in Group 2 from Be to Ba, the first ionization energy
decreases, and the atomic radius decreases
decreases, and the atomic radius increases
increases, and the atomic radius decreases
increases, and the atomic radius increases
Given the equation representing a reaction: 3Mg(s) + N₂(g) → Mg₃N₂(s) What is the mass of Mg₃N₂ that is produced when 14.58 grams of magnesium completely reacts with 5.60 grams of nitrogen?
8.98 g
10.46 g
20.18 g
49.34 g
Which Lewis electron-dot diagram represents a molecule of H₂S?
[Diagram 1]
[Diagram 2]
[Diagram 3]
[Diagram 4]
What is the vapor pressure of water at 90.°C?
40. kPa
68 kPa
94 kPa
150. kPa
A sample is composed of two different substances that can be separated by using filter paper. This sample is classified as
a heterogeneous mixture
a homogeneous mixture
a single compound
an unsaturated solution
Which solutions react to produce an insoluble compound?
KCl(aq) + LiCl(aq) →
LiCl(aq) + NaNO₃(aq) →
NaCl(aq) + AgClO₃(aq) →
KNO₃(aq) + AgClO₃(aq) →
What is the amount of heat energy absorbed when 40.0 grams of water is heated from 10.0°C to 30.0°C?
1.67 × 10³ J
3.34 × 10³ J
5.02 × 10³ J
2.67 × 10⁵ J
What is a chemical name of this compound?
2,3,3-trimethylbutane
2-methyl-2-ethylbutane
2,3-dimethylpentane
2,3-ethylpentane
During which intervals is the potential energy decreasing while the average kinetic energy remains constant?
BC and AB
BC and DE
EF and AB
EF and DE
Which formula represents a hydrocarbon?
CO₂
C₃H₈
C₂H₄O₂
C₃H₈O
Which type of organic reaction produces carbon dioxide and water?
combustion
esterification
fermentation
saponification
Which half-reaction equation represents the oxidation of lithium?
Li⁺ + e⁻ → Li
Li + e⁻ → Li⁺
Li → Li + e⁻
Li → Li⁺ + e⁻
Based on Table J, which ionic equation represents a spontaneous reaction that can occur in a voltaic cell?
Fe(s) + Mg²⁺(aq) → Fe²⁺(aq) + Mg(s)
Fe(s) + Mg(s) → Fe²⁺(aq) + Mg²⁺(aq)
Fe²⁺(aq) + Mg²⁺(aq) → Fe(s) + Mg(s)
Fe²⁺(aq) + Mg(s) → Fe(s) + Mg²⁺(aq)
Given the equation representing a system at equilibrium: NH₃(g) + H₂O(ℓ) ⇌ NH₄⁺(aq) + OH⁻(aq) In this system, the H₂O(ℓ) acts as
an acid, because it accepts an H⁺
an acid, because it donates an H⁺
a base, because it accepts an H⁺
a base, because it donates an H⁺
Which indicator is blue in a solution that has a pH value of 7.0?
bromcresol green
methyl orange
phenolphthalein
thymol blue
Which radioisotope requires long-term storage to prevent the risk of biological exposure?
N-16
K-42
Pu-239
Au-198
State the number of valence electrons in an atom of sulfur-32 in the ground state.
6
2
4
8
State the number of neutrons in an atom of sulfur-33.
(a)
Compare the electrical conductivity of an alkali metal at STP with the electrical conductivity of a halogen at STP.
State the type of chemical bonds formed when an alkali metal and a halogen react to form a compound.
(a)
Explain, in terms of electrons, why the halogens are all placed in the same group on the Periodic Table.
Halogens are all placed in the same group because they each have seven valence electrons.
Halogens are all placed in the same group because they each have a full outer shell of electrons.
Halogens are all placed in the same group because they each have two valence electrons.
Halogens are all placed in the same group because they each have eight valence electrons.
Balance the equation for the reaction, using the smallest whole number coefficients.
3Ag2S + 2Al → 6Ag + Al2S3
2Ag2S + 3Al → 4Ag + Al3S2
Ag2S + 2Al → 2Ag + Al2S
3Ag2S + Al → 6Ag + AlS3
Determine the gram-formula mass of the aluminum sulfide product.
(a)
Show a numerical setup for calculating the number of moles of silver sulfide in a 546-gram sample of Ag2S (gram-formula mass = 248 g/mol).
Base your answers to questions 59 through 61 on the information below and on your knowledge of chemistry. Hydrogen gas and iodine gas can combine in a reversible reaction to form hydrogen iodide gas. The equation below represents this system at equilibrium in a sealed, rigid container. H2(g) + I2(g) + 53.0 kJ ⇌ 2HI(g) 59 State evidence from the equation that the forward reaction is endothermic.
The equation shows that 53.0 kJ is absorbed (on the reactant side), indicating the forward reaction is endothermic.
The equation shows that 53.0 kJ is released (on the product side), indicating the forward reaction is exothermic.
The equation shows that energy is only involved in the reverse reaction, not the forward reaction.
The equation shows that the reaction occurs without any energy change.
State, in terms of reaction rates, why the concentration of HI(g) remains constant when the system is at equilibrium.
State how an increase in temperature affects the concentration of HI(g).
An increase in temperature decreases the concentration of HI(g).
An increase in temperature increases the concentration of HI(g).
An increase in temperature does not affect the concentration of HI(g).
An increase in temperature causes the concentration of HI(g) to remain constant.
State, in terms of carbon-carbon bonds, why butane is saturated.
Identify the class of organic compounds to which the organic product in the equation belongs.
The organic product belongs to the class of alkyl halides (haloalkanes).
The organic product belongs to the class of alcohols.
The organic product belongs to the class of carboxylic acids.
The organic product belongs to the class of ethers.
Based on the boiling point data, compare the strength of the intermolecular forces in 1-chlorobutane to the strength of the intermolecular forces in 2-chlorobutane.
The intermolecular forces in 1-chlorobutane are stronger than those in 2-chlorobutane because 1-chlorobutane has a higher boiling point.
The intermolecular forces in 2-chlorobutane are stronger than those in 1-chlorobutane because 2-chlorobutane has a higher boiling point.
The intermolecular forces in both 1-chlorobutane and 2-chlorobutane are equal because they are both chlorobutanes.
The boiling point does not provide any information about the strength of intermolecular forces in 1-chlorobutane and 2-chlorobutane.
Draw a structural formula for the 2-chlorobutane.
State the number of significant figures in the mass of the hydrated CuSO4 sample used by student 1.
3 significant figures
1 significant figure
2 significant figures
4 significant figures
Determine the percent composition by mass of water in the hydrated CuSO4 sample, based on the data for student 1.
34% (calculated as (1.02/3.00) × 100 = 34%)
25% (calculated as (0.75/3.00) × 100 = 25%)
50% (calculated as (1.50/3.00) × 100 = 50%)
66% (calculated as (2.00/3.00) × 100 = 66%)
Show a numerical setup for calculating the percent error for the percent composition by mass of water in the hydrated CuSO4 sample as determined by student 2.
|37.0% - 36.1%| / 36.1% × 100
|36.1% - 37.0%| / 37.0% × 100
|37.0% + 36.1%| / 36.1% × 100
|37.0% - 36.1%| / 37.0% × 1000
State the number of electrons shared between the nitrogen atom and one of the hydrogen atoms in an ammonia molecule.
1
2
3
4
Identify the noble gas that has atoms in the ground state with the same electron configuration as the nitrogen atom in a molecule of ammonia.
Helium
Neon
Argon
None
Determine the energy required to break all of the bonds in 0.250 mol of H–H bonds in the H₂(g).
54.6 kJ
108 kJ
217 kJ
436 kJ
Compare the density of the helium in the cylinder when the volume is 50.0 mL to the density of the helium in the cylinder when the volume is decreased to 25.0 mL.
The density doubles when the volume is decreased to 25.0 mL.
The density is halved when the volume is decreased to 25.0 mL.
The density remains the same when the volume is decreased to 25.0 mL.
The density decreases to one-fourth when the volume is decreased to 25.0 mL.
State one change in temperature and one change in pressure that will cause the gas in the cylinder to behave more like an ideal gas.
Increase temperature and decrease pressure.
Decrease temperature and increase pressure.
Increase both temperature and pressure.
Decrease both temperature and pressure.
Determine the number of moles of NaNO3 in 0.15 L of the solution.
Write a chemical name for NaNO3.
(a)
Compare the boiling point of the solution in sample 1 at standard pressure to the boiling point of water at standard pressure.
The boiling point of the solution in sample 1 is higher than the boiling point of pure water at standard pressure.
The boiling point of the solution in sample 1 is lower than the boiling point of pure water at standard pressure.
The boiling point of the solution in sample 1 is the same as the boiling point of pure water at standard pressure.
The boiling point of the solution in sample 1 cannot be compared to that of pure water at standard pressure.
Identify the electrode that attracts the Cu2+ ions as the cell operates.
The bracelet (cathode) attracts the Cu2+ ions.
The anode attracts the Cu2+ ions.
The salt bridge attracts the Cu2+ ions.
The electrolyte attracts the Cu2+ ions.
Determine the oxidation state of sulfur in CuSO4.
(a)
Write a balanced half-reaction equation for the reduction of Cu2+ ions that occurs in this cell.
Cu2+ + 2e- → Cu(s)
Cu(s) → Cu2+ + 2e-
Cu2+ → Cu(s) + 2e-
Cu(s) + 2e- → Cu2+
Base your answers to questions 80 through 82 on the information below and on your knowledge of chemistry. In a titration, 15.0 mL of hydrochloric acid, HCl(aq), of unknown concentration is exactly neutralized by the addition of 8.0 mL of 0.15 M KOH(aq). The pH value of the HCl(aq) solution is 1.1 before the titration begins. 80 Complete the equation in your answer booklet for the reaction that occurs in this titration by writing the formula for each product.
HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)
HCl(aq) + KOH(aq) → KOH(aq) + H2(g)
HCl(aq) + KOH(aq) → H2O(l) + Cl2(g)
HCl(aq) + KOH(aq) → KCl(aq) + H2(g)
State the pH value of the solution when the H+(aq) ion concentration in the acid has decreased by a factor of 10 compared to its original value.
2.1
1.1
3.1
4.1
Determine the molarity of the HCl(aq), by using the titration data.
0.080 M
0.020 M
0.50 M
0.0080 M
Based on Table N, state the decay mode for U-235.
(a)
Complete the nuclear equation in your answer booklet for the decay of Ba-141, by writing a notation for the missing product.
The missing product is an electron (beta particle), written as ⁰₋₁e or β⁻.
The missing product is a proton, written as ¹₁H.
The missing product is an alpha particle, written as ⁴₂He or α.
The missing product is a neutron, written as ¹₀n.
Compare the amount of energy released by the fission of one mole of uranium-235 to the amount of energy released by the combustion of one mole of octane fuel, C₈H₁₈.
The fission of one mole of uranium-235 releases much more energy than the combustion of one mole of octane.
The combustion of one mole of octane releases much more energy than the fission of one mole of uranium-235.
Both processes release approximately the same amount of energy.
Neither process releases any significant energy.
