VIRGINIA STATE INSPECTION
TEST 2026 2027 UPDATED
QUESTIONS WITH CORRECT
ANSWERS AND DETAILED
RATIONALES 100 PERCENT
VERIFIED GRADED A+
1. Which statement best describes the law of conservation of mass?
A. Matter can be created but not destroyed in a chemical reaction
B. The total mass of reactants is always greater than the total mass of
products
C. The total mass of reactants equals the total mass of products in a
chemical reaction
D. Mass is conserved only in physical changes, not chemical changes
CORRECT ANSWER: C. The total mass of reactants equals the total
mass of products in a chemical reaction
RATIONALE: The law of conservation of mass states that matter is
neither created nor destroyed in a chemical reaction. Therefore, the total
mass of reactants must equal the total mass of products. Choice A
incorrectly states matter can be created, choice B violates conservation,
and choice D incorrectly limits conservation to physical changes.
,2. What is the correct electron configuration for oxygen (atomic number
8)?
A. 1s² 2s² 2p⁴
B. 1s² 2s² 2p⁶
C. 1s² 2s² 2p³
D. 1s² 2s¹ 2p⁵
CORRECT ANSWER: A. 1s² 2s² 2p⁴
RATIONALE: Oxygen has 8 electrons. The configuration fills 1s (2), 2s
(2), and then 2p with 4 electrons. Choice B is for neon, choice C has too
few p electrons, and choice D incorrectly distributes the electrons.
3. A solution contains 0.25 moles of NaCl dissolved in 0.500 L of water.
What is the molarity of the solution?
A. 0.125 M
B. 0.250 M
C. 0.500 M
D. 2.00 M
CORRECT ANSWER: C. 0.500 M
RATIONALE: Molarity = moles of solute / liters of solution = 0.25 mol /
0.500 L = 0.500 M. Choice A is incorrect due to dividing incorrectly,
choice B is the moles value, and choice D inverts the calculation.
,4. Which of the following molecules is polar?
A. CO₂
B. CH₄
C. H₂O
D. CCl₄
CORRECT ANSWER: C. H₂O
RATIONALE: Water is polar due to its bent molecular geometry and the
electronegativity difference between oxygen and hydrogen, resulting in a
net dipole moment. CO₂, CH₄, and CCl₄ are nonpolar because their
symmetrical geometries cancel out individual bond dipoles.
5. What is the oxidation state of chromium in K₂Cr₂O₇?
A. +3
B. +4
C. +6
D. +7
CORRECT ANSWER: C. +6
RATIONALE: Potassium is +1 (×2 = +2), oxygen is -2 (×7 = -14). The
sum must be zero, so 2(+1) + 2(Cr) + 7(-2) = 0, giving 2 + 2Cr - 14 = 0,
so 2Cr = +12, Cr = +6. Choice A is the oxidation state in Cr₂O₃, choice B
is incorrect, and choice D overestimates.
, 6. A gas occupies 5.00 L at 1.00 atm and 298 K. What volume will it
occupy at 2.00 atm and 298 K?
A. 2.50 L
B. 5.00 L
C. 10.00 L
D. 1.25 L
CORRECT ANSWER: A. 2.50 L
RATIONALE: At constant temperature, Boyle's law applies: P₁V₁ = P₂V₂.
V₂ = (1.00 atm × 5.00 L) / 2.00 atm = 2.50 L. Choice C results from
doubling instead of halving, choice B ignores the pressure change, and
choice D is incorrect.
7. Which of the following is a strong electrolyte?
A. Acetic acid
B. Glucose
C. Sodium chloride
D. Ammonia
CORRECT ANSWER: C. Sodium chloride
RATIONALE: Sodium chloride is an ionic compound that completely
dissociates into ions in aqueous solution, making it a strong electrolyte.
TEST 2026 2027 UPDATED
QUESTIONS WITH CORRECT
ANSWERS AND DETAILED
RATIONALES 100 PERCENT
VERIFIED GRADED A+
1. Which statement best describes the law of conservation of mass?
A. Matter can be created but not destroyed in a chemical reaction
B. The total mass of reactants is always greater than the total mass of
products
C. The total mass of reactants equals the total mass of products in a
chemical reaction
D. Mass is conserved only in physical changes, not chemical changes
CORRECT ANSWER: C. The total mass of reactants equals the total
mass of products in a chemical reaction
RATIONALE: The law of conservation of mass states that matter is
neither created nor destroyed in a chemical reaction. Therefore, the total
mass of reactants must equal the total mass of products. Choice A
incorrectly states matter can be created, choice B violates conservation,
and choice D incorrectly limits conservation to physical changes.
,2. What is the correct electron configuration for oxygen (atomic number
8)?
A. 1s² 2s² 2p⁴
B. 1s² 2s² 2p⁶
C. 1s² 2s² 2p³
D. 1s² 2s¹ 2p⁵
CORRECT ANSWER: A. 1s² 2s² 2p⁴
RATIONALE: Oxygen has 8 electrons. The configuration fills 1s (2), 2s
(2), and then 2p with 4 electrons. Choice B is for neon, choice C has too
few p electrons, and choice D incorrectly distributes the electrons.
3. A solution contains 0.25 moles of NaCl dissolved in 0.500 L of water.
What is the molarity of the solution?
A. 0.125 M
B. 0.250 M
C. 0.500 M
D. 2.00 M
CORRECT ANSWER: C. 0.500 M
RATIONALE: Molarity = moles of solute / liters of solution = 0.25 mol /
0.500 L = 0.500 M. Choice A is incorrect due to dividing incorrectly,
choice B is the moles value, and choice D inverts the calculation.
,4. Which of the following molecules is polar?
A. CO₂
B. CH₄
C. H₂O
D. CCl₄
CORRECT ANSWER: C. H₂O
RATIONALE: Water is polar due to its bent molecular geometry and the
electronegativity difference between oxygen and hydrogen, resulting in a
net dipole moment. CO₂, CH₄, and CCl₄ are nonpolar because their
symmetrical geometries cancel out individual bond dipoles.
5. What is the oxidation state of chromium in K₂Cr₂O₇?
A. +3
B. +4
C. +6
D. +7
CORRECT ANSWER: C. +6
RATIONALE: Potassium is +1 (×2 = +2), oxygen is -2 (×7 = -14). The
sum must be zero, so 2(+1) + 2(Cr) + 7(-2) = 0, giving 2 + 2Cr - 14 = 0,
so 2Cr = +12, Cr = +6. Choice A is the oxidation state in Cr₂O₃, choice B
is incorrect, and choice D overestimates.
, 6. A gas occupies 5.00 L at 1.00 atm and 298 K. What volume will it
occupy at 2.00 atm and 298 K?
A. 2.50 L
B. 5.00 L
C. 10.00 L
D. 1.25 L
CORRECT ANSWER: A. 2.50 L
RATIONALE: At constant temperature, Boyle's law applies: P₁V₁ = P₂V₂.
V₂ = (1.00 atm × 5.00 L) / 2.00 atm = 2.50 L. Choice C results from
doubling instead of halving, choice B ignores the pressure change, and
choice D is incorrect.
7. Which of the following is a strong electrolyte?
A. Acetic acid
B. Glucose
C. Sodium chloride
D. Ammonia
CORRECT ANSWER: C. Sodium chloride
RATIONALE: Sodium chloride is an ionic compound that completely
dissociates into ions in aqueous solution, making it a strong electrolyte.
