GENERAL CHEMISTRY FINAL EXAM – QUESTIONS AND ANSWERS | VERIFIED AND WELL
DETAILED ANSWERS | PLUS RATIONALES | GUARANTEED PASS | LATEST EXAM UPDATE
Core Domains Atomic Structure and Periodicity Chemical Bonding and Molecular Geometry
Stoichiometry and Solution Chemistry Thermodynamics and Thermochemistry Chemical
Kinetics and Equilibrium Acids, Bases, and Electrochemistry
Introduction The purpose of this comprehensive final examination is to rigorously evaluate
candidates' mastery of core general chemistry principles, advanced problem-solving
methodologies, and laboratory safety protocols. The assessment measures essential skills
and knowledge, including quantitative reasoning, chemical reaction analysis,
thermodynamic calculations, and molecular property prediction. Designed with a robust
blend of traditional multiple-choice items and complex scenario-based challenges, the exam
tests the student's ability to apply theoretical chemical concepts to real-world laboratory and
industrial situations. Special emphasis is placed on critical thinking, ethical data reporting,
regulatory safety compliance, and effective decision-making under realistic constraints.
Section One: Questions 1–100
Question 1
A. 3.01 x 10^23 B. 6.022 x 10^23 C. 1.204 x 10^24 D. 1.505 x 10^23
B. 6.022 x 10^23 Explanation: Avogadro's number defines the number of constituent
particles, usually atoms or molecules, that are contained in one mole of a given substance,
exactly equal to 6.022 x 10^23 per mole.
Question 2
A. Mass is created or destroyed during chemical reactions. B. Energy is conserved in an
isolated system. C. The total mass of reactants equals the total mass of products in a closed
system. D. Volume remains constant during gas-phase reactions at constant temperature.
C. The total mass of reactants equals the total mass of products in a closed system.
Explanation: The law of conservation of mass dictates that matter cannot be created or
destroyed in a chemical reaction, meaning the total mass of all starting materials equals the
total mass of the resulting products in a closed container.
Question 3
A. Ionic bond B. Nonpolar covalent bond C. Polar covalent bond D. Metallic bond
C. Polar covalent bond Explanation: A polar covalent bond occurs when two atoms
with differing electronegativities share electrons unequally, creating a partial positive charge
on one atom and a partial negative charge on the other.
Question 4
,A. Temperature B. Catalyst C. Surface area D. Enthalpy of reaction
D. Enthalpy of reaction Explanation: While temperature, catalysts, and surface area
directly alter the rate of a chemical reaction by changing activation energy or collision
frequency, the overall enthalpy of reaction is a state function that dictates energy change,
not reaction speed.
Question 5
A. 1s^2 2s^2 2p^6 3s^1 B. 1s^2 2s^2 2p^5 C. 1s^2 2s^2 2p^6 3s^2 D. 1s^2 2s^2 2p^6 3s^2
3p^1
A. 1s^2 2s^2 2p^6 3s^1 Explanation: Sodium has an atomic number of 11, meaning
it possesses 11 electrons. The correct electron configuration fills orbitals sequentially up to
the 3s orbital with a single valence electron.
Question 6
A. Molarity B. Molality C. Mass percentage D. Mole fraction
B. Molality Explanation: Molality is defined as the number of moles of solute
dissolved per kilogram of solvent. Unlike molarity, it does not change with temperature
because mass does not fluctuate with thermal expansion.
Question 7
A. An increase in pressure shifts the equilibrium to the side with fewer moles of gas. B. An
increase in temperature shifts an exothermic equilibrium to the right. C. Adding a reactant
shifts the equilibrium to the left. D. A catalyst changes the equilibrium position of a
reversible reaction.
A. An increase in pressure shifts the equilibrium to the side with fewer moles of gas.
Explanation: According to Le Chatelier's principle, system stress caused by increased
pressure is mitigated by shifting equilibrium toward the side with fewer moles of gas to
reduce overall pressure.
Question 8
A. pH = -log[OH-] B. pOH = -log[H+] C. pH + pOH = 14 at standard conditions D. Kw =
[H+][OH-] = 1.0 x 10^-7
C. pH + pOH = 14 at standard conditions Explanation: At standard temperature, the
ion-product constant of water is 1.0 x 10^-14, which leads directly to the logarithmic
relationship that pH plus pOH equals 14.
Question 9
A. Anode B. Cathode C. Salt bridge D. External wire
, B. Cathode Explanation: By definition in electrochemistry, reduction always occurs at
the cathode, regardless of whether the electrochemical cell is galvanic or electrolytic.
Question 10
A. Fluorine B. Cesium C. Oxygen D. Nitrogen
B. Cesium Explanation: Atomic radius increases down a group and decreases across a
period from left to right. Cesium is located near the bottom left of the periodic table, giving
it the largest atomic radius among common elements.
Question 11
A. London dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding D. Ionic
bonding
C. Hydrogen bonding Explanation: Hydrogen bonding is a particularly strong type of
intermolecular force that occurs when hydrogen is covalently bonded to highly
electronegative atoms such as nitrogen, oxygen, or fluorine.
Question 12
A. q = m x C x ΔT B. PV = nRT C. ΔG = ΔH - TΔS D. E = mc^2
A. q = m x C x ΔT Explanation: The specific heat capacity equation, q = mCΔT, is used
to calculate the heat absorbed or released by a substance when its temperature changes
without undergoing a phase change.
Question 13
A. Zero order B. First order C. Second order D. Third order
B. First order Explanation: For a first-order reaction, the half-life is independent of
the initial concentration of the reactant, a characteristic defined by the equation t_1/2 =
0.693 / k.
Question 14
A. Strong acid B. Weak acid C. Strong base D. Weak base
A. Strong acid Explanation: Strong acids, such as hydrochloric acid or nitric acid,
dissociate completely into their constituent ions when dissolved in an aqueous solution.
Question 15
A. Oxidation involves the gain of electrons. B. Reduction involves the loss of electrons. C. The
oxidizing agent is itself reduced during a redox reaction. D. The reducing agent gains
electrons in a chemical reaction.
, C. The oxidizing agent is itself reduced during a redox reaction. Explanation: In redox
chemistry, the oxidizing agent promotes oxidation in another species by accepting electrons,
which inherently causes the oxidizing agent to undergo reduction.
Question 16
A. Linear B. Bent C. Trigonal planar D. Tetrahedral
B. Bent Explanation: Water has two bonding pairs and two lone pairs around the
central oxygen atom, which repels the bonds downward according to VSEPR theory, resulting
in a bent molecular geometry with an angle near 104.5 degrees.
Question 17
A. Joule B. Pascal C. Kelvin D. Mole
B. Pascal Explanation: Pressure is defined as force per unit area, and its standard SI
unit is the pascal, equivalent to one newton per square meter.
Question 18
A. Sublimation B. Deposition C. Condensation D. Melting
A. Sublimation Explanation: Sublimation is the phase transition in which a substance
passes directly from a solid state to a gaseous state without passing through the
intermediate liquid phase.
Question 19
A. 22.4 liters B. 11.2 liters C. 44.8 liters D. 1.0 liter
A. 22.4 liters Explanation: According to ideal gas laws, one mole of any ideal gas
occupies a standard molar volume of 22.4 liters at standard temperature and pressure.
Question 20
A. Principal quantum number (n) B. Angular momentum quantum number (l) C. Magnetic
quantum number (m_l) D. Spin quantum number (m_s)
A. Principal quantum number (n) Explanation: The principal quantum number,
designated as n, primarily determines the overall energy level and average distance of the
electron orbital from the nucleus.
Question 21
A. Buffer solution B. Saturated solution C. Supersaturated solution D. Standard solution
A. Buffer solution Explanation: A buffer solution is specifically designed to resist
significant changes in pH when small amounts of strong acids or strong bases are
introduced, usually consisting of a weak conjugate acid-base pair.
DETAILED ANSWERS | PLUS RATIONALES | GUARANTEED PASS | LATEST EXAM UPDATE
Core Domains Atomic Structure and Periodicity Chemical Bonding and Molecular Geometry
Stoichiometry and Solution Chemistry Thermodynamics and Thermochemistry Chemical
Kinetics and Equilibrium Acids, Bases, and Electrochemistry
Introduction The purpose of this comprehensive final examination is to rigorously evaluate
candidates' mastery of core general chemistry principles, advanced problem-solving
methodologies, and laboratory safety protocols. The assessment measures essential skills
and knowledge, including quantitative reasoning, chemical reaction analysis,
thermodynamic calculations, and molecular property prediction. Designed with a robust
blend of traditional multiple-choice items and complex scenario-based challenges, the exam
tests the student's ability to apply theoretical chemical concepts to real-world laboratory and
industrial situations. Special emphasis is placed on critical thinking, ethical data reporting,
regulatory safety compliance, and effective decision-making under realistic constraints.
Section One: Questions 1–100
Question 1
A. 3.01 x 10^23 B. 6.022 x 10^23 C. 1.204 x 10^24 D. 1.505 x 10^23
B. 6.022 x 10^23 Explanation: Avogadro's number defines the number of constituent
particles, usually atoms or molecules, that are contained in one mole of a given substance,
exactly equal to 6.022 x 10^23 per mole.
Question 2
A. Mass is created or destroyed during chemical reactions. B. Energy is conserved in an
isolated system. C. The total mass of reactants equals the total mass of products in a closed
system. D. Volume remains constant during gas-phase reactions at constant temperature.
C. The total mass of reactants equals the total mass of products in a closed system.
Explanation: The law of conservation of mass dictates that matter cannot be created or
destroyed in a chemical reaction, meaning the total mass of all starting materials equals the
total mass of the resulting products in a closed container.
Question 3
A. Ionic bond B. Nonpolar covalent bond C. Polar covalent bond D. Metallic bond
C. Polar covalent bond Explanation: A polar covalent bond occurs when two atoms
with differing electronegativities share electrons unequally, creating a partial positive charge
on one atom and a partial negative charge on the other.
Question 4
,A. Temperature B. Catalyst C. Surface area D. Enthalpy of reaction
D. Enthalpy of reaction Explanation: While temperature, catalysts, and surface area
directly alter the rate of a chemical reaction by changing activation energy or collision
frequency, the overall enthalpy of reaction is a state function that dictates energy change,
not reaction speed.
Question 5
A. 1s^2 2s^2 2p^6 3s^1 B. 1s^2 2s^2 2p^5 C. 1s^2 2s^2 2p^6 3s^2 D. 1s^2 2s^2 2p^6 3s^2
3p^1
A. 1s^2 2s^2 2p^6 3s^1 Explanation: Sodium has an atomic number of 11, meaning
it possesses 11 electrons. The correct electron configuration fills orbitals sequentially up to
the 3s orbital with a single valence electron.
Question 6
A. Molarity B. Molality C. Mass percentage D. Mole fraction
B. Molality Explanation: Molality is defined as the number of moles of solute
dissolved per kilogram of solvent. Unlike molarity, it does not change with temperature
because mass does not fluctuate with thermal expansion.
Question 7
A. An increase in pressure shifts the equilibrium to the side with fewer moles of gas. B. An
increase in temperature shifts an exothermic equilibrium to the right. C. Adding a reactant
shifts the equilibrium to the left. D. A catalyst changes the equilibrium position of a
reversible reaction.
A. An increase in pressure shifts the equilibrium to the side with fewer moles of gas.
Explanation: According to Le Chatelier's principle, system stress caused by increased
pressure is mitigated by shifting equilibrium toward the side with fewer moles of gas to
reduce overall pressure.
Question 8
A. pH = -log[OH-] B. pOH = -log[H+] C. pH + pOH = 14 at standard conditions D. Kw =
[H+][OH-] = 1.0 x 10^-7
C. pH + pOH = 14 at standard conditions Explanation: At standard temperature, the
ion-product constant of water is 1.0 x 10^-14, which leads directly to the logarithmic
relationship that pH plus pOH equals 14.
Question 9
A. Anode B. Cathode C. Salt bridge D. External wire
, B. Cathode Explanation: By definition in electrochemistry, reduction always occurs at
the cathode, regardless of whether the electrochemical cell is galvanic or electrolytic.
Question 10
A. Fluorine B. Cesium C. Oxygen D. Nitrogen
B. Cesium Explanation: Atomic radius increases down a group and decreases across a
period from left to right. Cesium is located near the bottom left of the periodic table, giving
it the largest atomic radius among common elements.
Question 11
A. London dispersion forces B. Dipole-dipole interactions C. Hydrogen bonding D. Ionic
bonding
C. Hydrogen bonding Explanation: Hydrogen bonding is a particularly strong type of
intermolecular force that occurs when hydrogen is covalently bonded to highly
electronegative atoms such as nitrogen, oxygen, or fluorine.
Question 12
A. q = m x C x ΔT B. PV = nRT C. ΔG = ΔH - TΔS D. E = mc^2
A. q = m x C x ΔT Explanation: The specific heat capacity equation, q = mCΔT, is used
to calculate the heat absorbed or released by a substance when its temperature changes
without undergoing a phase change.
Question 13
A. Zero order B. First order C. Second order D. Third order
B. First order Explanation: For a first-order reaction, the half-life is independent of
the initial concentration of the reactant, a characteristic defined by the equation t_1/2 =
0.693 / k.
Question 14
A. Strong acid B. Weak acid C. Strong base D. Weak base
A. Strong acid Explanation: Strong acids, such as hydrochloric acid or nitric acid,
dissociate completely into their constituent ions when dissolved in an aqueous solution.
Question 15
A. Oxidation involves the gain of electrons. B. Reduction involves the loss of electrons. C. The
oxidizing agent is itself reduced during a redox reaction. D. The reducing agent gains
electrons in a chemical reaction.
, C. The oxidizing agent is itself reduced during a redox reaction. Explanation: In redox
chemistry, the oxidizing agent promotes oxidation in another species by accepting electrons,
which inherently causes the oxidizing agent to undergo reduction.
Question 16
A. Linear B. Bent C. Trigonal planar D. Tetrahedral
B. Bent Explanation: Water has two bonding pairs and two lone pairs around the
central oxygen atom, which repels the bonds downward according to VSEPR theory, resulting
in a bent molecular geometry with an angle near 104.5 degrees.
Question 17
A. Joule B. Pascal C. Kelvin D. Mole
B. Pascal Explanation: Pressure is defined as force per unit area, and its standard SI
unit is the pascal, equivalent to one newton per square meter.
Question 18
A. Sublimation B. Deposition C. Condensation D. Melting
A. Sublimation Explanation: Sublimation is the phase transition in which a substance
passes directly from a solid state to a gaseous state without passing through the
intermediate liquid phase.
Question 19
A. 22.4 liters B. 11.2 liters C. 44.8 liters D. 1.0 liter
A. 22.4 liters Explanation: According to ideal gas laws, one mole of any ideal gas
occupies a standard molar volume of 22.4 liters at standard temperature and pressure.
Question 20
A. Principal quantum number (n) B. Angular momentum quantum number (l) C. Magnetic
quantum number (m_l) D. Spin quantum number (m_s)
A. Principal quantum number (n) Explanation: The principal quantum number,
designated as n, primarily determines the overall energy level and average distance of the
electron orbital from the nucleus.
Question 21
A. Buffer solution B. Saturated solution C. Supersaturated solution D. Standard solution
A. Buffer solution Explanation: A buffer solution is specifically designed to resist
significant changes in pH when small amounts of strong acids or strong bases are
introduced, usually consisting of a weak conjugate acid-base pair.
