Questions on Molecular and Ionic Equations
Multiple-Choice Questions — Molecular and Ionic Equations
1. What does a molecular equation show?
A) Only ions in solution
B) All reactants and products as molecules or compounds
C) Only solids
D) Only gases
E) Only net ions
2. What is an ionic equation?
A) Shows only compounds
B) Shows all strong electrolytes as ions
C) Shows only solids
D) Shows only gases
E) Shows no ions
3. What is a net ionic equation?
A) Shows all species including spectator ions
B) Shows only species that undergo a chemical change
C) Shows only molecular compounds
D) Shows only solvents
E) Shows balanced electrons
4. In the reaction between AgNO₃ and NaCl, which ion is a spectator?
A) Ag⁺
B) NO₃⁻
C) Cl⁻
D) Na⁺
E) Both B and D
5. Which of the following is the net ionic equation for the precipitation of AgCl?
A) AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
B) Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
C) Na⁺(aq) + NO₃⁻(aq) → NaNO₃(aq)
D) Ag⁺(aq) + Na⁺(aq) → AgNa(s)
E) Cl⁻(aq) + NO₃⁻(aq) → ClNO₃(aq)
6. Which equation correctly shows a molecular equation?
A) NaCl(aq) → Na⁺(aq) + Cl⁻(aq)
B) HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
C) Na⁺(aq) + OH⁻(aq) → H₂O(l)
D) H⁺(aq) + OH⁻(aq) → H₂O(l)
E) Cl⁻(aq) + Ag⁺(aq) → AgCl(s)
7. Which of these is a spectator ion in acid-base neutralization?
A) H⁺
B) OH⁻
C) Na⁺
D) H₂O
E) None
8. What type of equation would include the complete dissociation of strong electrolytes?
A) Molecular
B) Ionic
C) Net ionic
D) Empirical
E) None of the above
9. What state symbol indicates a precipitate in an equation?
A) (aq)
B) (g)
C) (l)
D) (s)
E) (p)
10. Which is the correct ionic equation for the reaction of BaCl₂ with Na₂SO₄?
A) Ba²⁺(aq) + 2Cl⁻(aq) + 2Na⁺(aq) + SO₄²⁻(aq) → BaSO₄(s) + 2Na⁺(aq) + 2Cl⁻(aq)
B) BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2NaCl(aq)
C) Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)
D) Ba²⁺(aq) + 2Na⁺(aq) + SO₄²⁻(aq) + 2Cl⁻(aq) → BaSO₄(s) + 2NaCl(aq)
E) Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(aq)
11. What is the net ionic equation for the reaction of hydrochloric acid with sodium hydroxide?
A) HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
B) H⁺(aq) + OH⁻(aq) → H₂O(l)
C) Na⁺(aq) + Cl⁻(aq) → NaCl(aq)
D) HCl(aq) + NaOH(aq) → H₂O(l) + Na⁺(aq) + Cl⁻(aq)
E) H⁺(aq) + NaOH(aq) → Na⁺(aq) + H₂O(l)
12. Which ion is NOT a spectator ion in the reaction of AgNO₃ and KBr?
A) NO₃⁻
B) K⁺
C) Ag⁺
D) Both A and B
E) Both B and C
13. In the reaction Pb(NO₃)₂ + 2KI → PbI₂ + 2KNO₃, which is the precipitate?
A) Pb(NO₃)₂
B) KI
C) PbI₂
D) KNO₃
E) Pb
14. Which of these is a strong electrolyte that completely dissociates in water?
A) H₂O
B) NaCl
C) Glucose
D) Ethanol
E) CO₂
15. Which species would appear in the ionic equation for the reaction of magnesium sulfate with barium chloride?
A) MgSO₄(s)
B) Ba²⁺(aq)
C) Mg²⁺(aq)
D) SO₄²⁻(aq)
E) Both B, C, and D
16. What does the "(aq)" state symbol indicate in an equation?
A) Solid state
B) Gas state
C) Liquid state
D) Dissolved in water (aqueous)
E) None of the above
17. In writing net ionic equations, which ions are canceled out?
A) All positive ions
B) All negative ions
C) Spectator ions
D) Precipitates
E) Solvent molecules
18. Which of the following represents a molecular equation for a neutralization reaction?
A) HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
B) H⁺(aq) + OH⁻(aq) → H₂O(l)
C) Na⁺(aq) + Cl⁻(aq) → NaCl(aq)
D) Cl⁻(aq) + Na⁺(aq) → NaCl(aq)
E) H₂O(l) → H⁺(aq) + OH⁻(aq)
19. Which of these is the ionic equation for the reaction between calcium chloride and sodium carbonate?
A) Ca²⁺(aq) + 2Cl⁻(aq) + 2Na⁺(aq) + CO₃²⁻(aq) → CaCO₃(s) + 2Na⁺(aq) + 2Cl⁻(aq)
B) CaCl₂(aq) + Na₂CO₃(aq) → CaCO₃(s) + 2NaCl(aq)
C) Ca²⁺(aq) + CO₃²⁻(aq) → CaCO₃(s)
D) CaCO₃(s) + NaCl(aq) → CaCl₂(aq) + Na₂CO₃(aq)
E) Ca²⁺(aq) + Na⁺(aq) + CO₃²⁻(aq) + Cl⁻(aq) → CaCO₃(s) + NaCl(aq)
20. Why are net ionic equations useful?
A) They show only spectator ions
B) They simplify equations to show actual chemical change
C) They show the physical state of all species
D) They list all compounds in solution
E) They are used only for gases
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Answer Key with Explanations
1. B – Molecular equations show all reactants and products as intact molecules.
2. B – Ionic equations show strong electrolytes dissociated into ions.
3. B – Net ionic equations show only species that change during the reaction.
4. E – Nitrate (NO₃⁻) and sodium (Na⁺) ions do not participate and are spectators.
5. B – The precipitate formation is the reaction of Ag⁺ and Cl⁻ ions.
6. B – Molecular equations show all compounds as molecules without dissociation.
7. C – Sodium ions (Na⁺) are spectators in acid-base neutralization.
8. B – Ionic equations show dissociation of strong electrolytes.
9. D – Precipitates are indicated by (s) for solid.
10. A – Complete ionic form with all ions before and after reaction.
11. B – Net ionic equation for neutralization shows H⁺ + OH⁻ → H₂O.
12. D – Nitrate and potassium ions are spectators; silver ion reacts.
13. C – Lead iodide (PbI₂) is the solid precipitate formed.
14. B – NaCl dissociates completely in water.
15. E – Magnesium, barium, and sulfate ions are present as ions in solution.
16. D – (aq) indicates aqueous or dissolved in water.
17. C – Spectator ions cancel out in net ionic equations.
18. A – Molecular equation shows all species in molecular form.
19. A – Full ionic equation before canceling spectator ions.
20. B – Net ionic equations focus on actual chemical changes.
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