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WorksheetsPractice Chemistry Regents (326)
Total questions: 69
Worksheet time: 6hrs 45mins
Which phrase describes the nucleus of any atom?
has an overall positive charge
has an overall negative charge
contains negative electrons
contains positive electrons
Which two particles each have a mass of approximately one atomic mass unit?
an electron and a proton
an electron and a positron
a neutron and a proton
a neutron and a positron
The wave-mechanical model of the atom describes the location of electrons as
loosely packed in the nucleus of an atom
as densely packed in the nucleus of an atom
in circular paths around the nucleus
in orbitals outside the nucleus
When a ground state electron in an atom moves to an excited state, the electron
absorbs energy as it moves to a higher energy state
absorbs energy as it moves to a lower energy state
releases energy as it moves to a higher energy state
releases energy as it moves to a lower energy state
Which statement describes a chemical property of iron?
Iron is malleable.
Iron conducts electricity.
Iron reacts with nitric acid.
Iron has a high melting point.
Diamond and graphite are two forms of solid carbon. These two forms of carbon have
different crystal structures and different properties
different crystal structures and the same properties
the same crystal structure and different properties
the same crystal structure and the same properties
Which substance can be broken down by a chemical change?
cobalt
ethane
krypton
manganese
Based on Table I, which equation represents conservation of mass and energy?
1
2
3
4
At STP, which property can be used to differentiate a 10-gram sample of NaCl(s) from a 10-gram sample of NaNO₃(s)?
mass of the sample
temperature of the sample
solubility in water
phase at STP
What is the number of electrons shared between the two atoms in an O₂ molecule?
6
2
3
4
Which changes in both charge and radius occur when an atom loses an electron?
A negative ion is formed with a smaller radius than the atom.
A negative ion is formed with a larger radius than the atom.
A positive ion is formed with a smaller radius than the atom.
A positive ion is formed with a larger radius than the atom.
Which statement describes what occurs when two iodine atoms react to produce an iodine molecule?
A bond forms and energy is absorbed.
A bond forms and energy is released.
A bond breaks and energy is absorbed.
A bond breaks and energy is released.
Which process can be used to separate a mixture of two liquids having different boiling points?
deposition
distillation
filtration
sublimation
Which statement describes a solution of sodium chloride in water?
The mixture is heterogeneous, the solute is NaCl and the solvent is H₂O.
The mixture is heterogeneous, the solute is H₂O and the solvent is NaCl.
The mixture is homogeneous, the solute is NaCl and the solvent is H₂O.
The mixture is homogeneous, the solute is H₂O and the solvent is NaCl.
At STP, which property would be the same for 1.0 liter of helium and 1.0 liter of argon?
boiling point
density
mass
number of atoms
The melting of an ice cube is an example of an
endothermic, chemical change
endothermic, physical change
exothermic, chemical change
exothermic, physical change
Which statement explains the low boiling point of hydrogen, H₂, at standard pressure?
Hydrogen has strong covalent bonds.
Hydrogen has weak covalent bonds.
Hydrogen has strong intermolecular forces.
Hydrogen has weak intermolecular forces.
In chemical reactions, which term is defined as the difference between the potential energy of the products and the potential energy of the reactants?
heat of fusion
heat of reaction
thermal conductivity
electrical conductivity
Which phrase describes what happens to the reaction pathway and activation energy of a reaction to which a catalyst is added?
the same pathway with the same activation energy
the same pathway with a lower activation energy
a different pathway with the same activation energy
a different pathway with a lower activation energy
An atom of which element is bonded to the carbon atom in the amide functional group?
iodine
nitrogen
phosphorus
sulfur
Which statement describes the two isomers of butane?
They have the same molecular formula but different structural formulas.
They have the same molecular formula and the same structural formula.
They have different molecular formulas and different structural formulas.
They have different molecular formulas but the same structural formula.
Which substance is an Arrhenius base?
HNO3
KNO3
LiOH
CH3COOH
Which statement represents neutralization?
An Arrhenius acid and an Arrhenius base react to produce water and a salt.
An Arrhenius acid and a salt react to produce water and an Arrhenius base.
Water and an Arrhenius acid react to produce an Arrhenius base and a salt.
Water and a salt react to produce an Arrhenius base and an Arrhenius acid.
A tenfold increase in hydronium ion concentration is represented by
a decrease of one unit of pH
a decrease of 10 units of pH
an increase of one unit of pH
an increase of 10 units of pH
Which Lewis electron-dot diagram represents an atom of nitrogen in the ground state?
Diagram 1
Diagram 2
Diagram 3
Diagram 4
(106.905 u)(51.8%) + (108.905 u)(48.2%)
(106.905 u)(51.8) + (108.905 u)(48.2)
(106.905 u)(48.2%) + (108.905 u)(51.8%)
(106.905 u)(48.2) + (108.905 u)(51.8)
A potassium atom has a mass number of 37. What is the number of neutrons in this atom?
15
18
22
37
At room temperature, a student determines the density of a sample of nickel to be 9.79 g/cm³. Based on Table S, what is the student's percent error for the density of nickel?
Hint: use formula on Table T
0.091%
0.10%
9.1%
10.%
Compared to the metals in Period 2, the nonmetals in Period 2 have
lower first ionization energies and lower electronegativity values
lower first ionization energies and higher electronegativity values
higher first ionization energies and lower electronegativity values
higher first ionization energies and higher electronegativity values
Which formula represents calcium hydride?
CaH
CaH2
CaOH
Ca(OH)2
What is the number of moles in a 78.8-gram sample of MgCO3 (gram-formula mass = 84.3 g/mol)?
0.949 mol
0.935 mol
0.843 mol
1.070 mol
Given the equation representing a reaction: F2(g) + 2KCl(aq) → 2KF(aq) + Cl2(g), Which type of chemical reaction is represented by the equation?
synthesis
decomposition
single replacement
double replacement
Based on Table H, which compound has the strongest intermolecular forces at 60 kPa?
ethanoic acid
ethanol
propanone
water
Which particle diagram represents a sample of xenon at STP?
Diagram (1)
Diagram (2)
Diagram (3)
Diagram (4)
Based on Table G, which compound is less soluble in water as the temperature increases from 0°C to 100°C?
KNO3
NH3
KClO3
NH4Cl
How many moles of KI are needed to make 0.50 L of a 0.20 M aqueous solution?
0.10 mol
0.25 mol
0.40 mol
0.70 mol
A solution is prepared using 9.80 grams of NaHCO3 in enough water to make 1500. grams of total solution. What is the concentration of the solution expressed in parts per million?
1
2
3
4
A potential energy diagram for a chemical reaction is given below. Each interval on the potential energy axis represents 100. kilojoules of potential energy. What can be concluded from the diagram?
The reaction is endothermic, and the heat of reaction is -200 kJ.
The reaction is endothermic, and the heat of reaction is +200 kJ.
The reaction is exothermic, and the heat of reaction is +200 kJ.
The reaction is exothermic, and the heat of reaction is -200 kJ.
Which aqueous solution has the greatest ability to conduct an electric current?
0.10 M NaCl(aq)
0.010 M NaCl(aq)
0.10 M C6H12O6(aq)
0.010 M C6H12O6(aq)
Compare the energy of an electron in the first shell of a technetium atom to the energy of an electron in the third shell of the same atom.
State, in terms of protons and neutrons, why the various nuclides of technetium are isotopes of each other.
Show a numerical setup for calculating the volume of this sample of gas at 298 K and 1.00 atm.
State a change in pressure that will cause the gas in the cylinder to behave more like an ideal gas.
State the direction of heat flow between the candle flame and the beaker of water during the time the candle is lit.
Show a numerical setup for calculating the amount of heat, in joules, absorbed by the water in the beaker as a result of the burning candle.
State how the molecular motion of the water molecules in the beaker changes as the temperature increases.
Compare the rate of the forward reaction to the rate of the reverse reaction when the system is at equilibrium.
State how the equilibrium shifts when the pressure on the equilibrium system is increased at constant temperature.
Compare the entropy of a sample of dinitrogen tetroxide gas at 25°C and 1.0 atmosphere to the entropy of the same sample of dinitrogen tetroxide liquid at 15°C and 1.0 atmosphere.
Based on Table J, state why Cu(s) reacts spontaneously with Ag+(aq).
During a laboratory activity, 15.0 mL of hydrochloric acid, HCl(aq), is exactly neutralized by 18.2 mL of 0.11 M sodium hydroxide, NaOH(aq). During the laboratory activity, appropriate safety equipment is used and safety procedures are followed.
Write the name of the laboratory procedure used in this activity.
During a laboratory activity, 15.0 mL of hydrochloric acid, HCl(aq), is exactly neutralized by 18.2 mL of 0.11 M sodium hydroxide, NaOH(aq). During the laboratory activity, appropriate safety equipment is used and safety procedures are followed.
Show a numerical setup for calculating the molarity of the HCl(aq) solution.
Several elements are considered endangered because there is a risk of these elements becoming unavailable for commercial uses in the next 100 years. Helium, zinc, gallium, indium, and tellurium are included in the list of these endangered elements.
Identify the three endangered elements listed in the passage that are classified as metals.
Explain, in terms of electrons, why gallium and indium have similar chemical properties.
Compare the density of a sample of helium at STP with the density of a sample of tellurium at STP.
Explain, in terms of electron shells, why the atomic radius of an atom of indium is greater than the atomic radius of an atom of gallium when both atoms are in the ground state.
Determine the percent composition by mass of nitrogen in HNO3
(gram-formula mass = 63.0 g/mol).
Balance equation 1 in your answer booklet, using the smallest whole-number coefficients.
Show a numerical setup for calculating the gram-formula mass of the NO2(g) produced in equation 2.
Determine the number of moles of oxygen required to completely react with 4.0 moles of NO(g) in equation 2.
State the molecular polarity for each of the reactants in the equation. (Refer to the balanced equation for photosynthesis provided in the worksheet.)
In the space in your answer booklet, draw a Lewis electron-dot diagram for a molecule of water.
Based on Table S, compare the strength of attraction of a carbon atom for electrons with the strength of attraction of an oxygen atom for the electrons in a bond between them. (Note: Table S is not provided in the image.)
State, in terms of element classification, why CO2 is a molecular compound.
Write the empirical formula for glucose.
Identify the liquid tested by the student that is most acidic.
State the color of bromcresol green after the indicator is added to a sample of lemon juice.
Complete the equation in your answer booklet by writing the formula of the missing product in the reaction of aqueous potassium hydroxide with the vinegar, acetic acid.
KOH + HC2H3O2 → KC2H3O2 + ___________
Based on the pH value in the table, compare the concentration of hydronium ions to the concentration of hydroxide ions in the distilled water.
