Questions on Net Ionic Equations
Multiple-Choice Questions — Net Ionic Equations
1. What is a net ionic equation?
A) An equation showing all reactants and products as molecules
B) An equation showing only ions involved in the chemical change
C) An equation showing only solids formed
D) An equation showing all spectator ions
E) An equation showing all reactants and products as gases
2. Which ions are typically omitted from a net ionic equation?
A) Reacting ions
B) Spectator ions
C) Precipitates
D) Gaseous products
E) All ions are included
3. In the reaction between NaCl and AgNO₃, what is the net ionic equation?
A) Na⁺ + NO₃⁻ → NaNO₃
B) Ag⁺ + Cl⁻ → AgCl(s)
C) NaCl + AgNO₃ → AgCl + NaNO₃
D) AgNO₃ → Ag⁺ + NO₃⁻
E) NaCl → Na⁺ + Cl⁻
4. What does the (s) symbol represent in net ionic equations?
A) Aqueous solution
B) Solid precipitate
C) Gas
D) Liquid
E) Spectator ion
5. Why do we write net ionic equations?
A) To include all compounds
B) To simplify equations by removing spectator ions
C) To show only the molecular formulas
D) To balance the equation only
E) To show all physical states
6. Which of the following is a spectator ion in the reaction of BaCl₂ with Na₂SO₄?
A) Ba²⁺
B) SO₄²⁻
C) Na⁺
D) BaSO₄
E) CO₃²⁻
7. What happens to spectator ions in net ionic equations?
A) They react and form products
B) They remain unchanged and are omitted
C) They form precipitates
D) They change oxidation state
E) They form gases
8. Which is the correct net ionic equation for the neutralization of HCl with NaOH?
A) HCl + NaOH → NaCl + H₂O
B) H⁺ + OH⁻ → H₂O
C) Na⁺ + Cl⁻ → NaCl
D) HCl → H⁺ + Cl⁻
E) NaOH → Na⁺ + OH⁻
9. What must be done before writing a net ionic equation?
A) Write the balanced molecular equation
B) Write the ionic equation including all ions
C) Identify and cancel spectator ions
D) All of the above
E) None of the above
10. In the precipitation reaction between Pb(NO₃)₂ and KI, which species appear in the net ionic equation?
A) Pb²⁺ and NO₃⁻
B) Pb²⁺ and I⁻
C) K⁺ and NO₃⁻
D) KI and Pb(NO₃)₂
E) K⁺ and I⁻
11. What is the net ionic equation for the reaction of calcium chloride and sodium carbonate?
A) CaCl₂ + Na₂CO₃ → CaCO₃ + 2NaCl
B) Ca²⁺ + CO₃²⁻ → CaCO₃(s)
C) Ca²⁺ + 2Cl⁻ + 2Na⁺ + CO₃²⁻ → CaCO₃ + 2NaCl
D) CaCl₂ → Ca²⁺ + 2Cl⁻
E) Na₂CO₃ → 2Na⁺ + CO₃²⁻
12. What does it mean if an ion does not appear in the net ionic equation?
A) It is a reactant
B) It is a product
C) It is a spectator ion
D) It is a precipitate
E) It is a gas
13. Which of the following is NOT part of the net ionic equation?
A) Ions that form a precipitate
B) Ions that react to form a gas
C) Spectator ions
D) Ions that form a liquid product
E) Ions that undergo oxidation
14. The net ionic equation for a gas-forming reaction always includes:
A) Spectator ions
B) The gaseous product
C) All dissolved ions
D) Only reactants
E) Only solids
15. Which reaction shows a correct net ionic equation?
A) HNO₃ + NaOH → NaNO₃ + H₂O
B) H⁺ + OH⁻ → H₂O
C) Na⁺ + NO₃⁻ → NaNO₃
D) HNO₃ → H⁺ + NO₃⁻
E) NaOH → Na⁺ + OH⁻
16. How do you identify the precipitate in a net ionic equation?
A) It remains dissolved in solution
B) It is indicated by (aq)
C) It is indicated by (s)
D) It is a gas
E) It is always water
17. When writing a net ionic equation for a reaction in aqueous solution, what form do strong electrolytes take?
A) Intact molecules
B) Dissociated ions
C) Solids
D) Gases
E) None
18. Which of the following is a correct net ionic equation for the reaction of hydrochloric acid and silver nitrate?
A) HCl + AgNO₃ → AgCl + HNO₃
B) Ag⁺ + Cl⁻ → AgCl(s)
C) H⁺ + NO₃⁻ → HNO₃
D) AgNO₃ → Ag⁺ + NO₃⁻
E) HCl → H⁺ + Cl⁻
19. Why are net ionic equations important in chemistry?
A) They show all chemical species in detail
B) They highlight only the species involved in the chemical change
C) They simplify molecular formulas
D) They list all reactants and products
E) They show physical states
20. What is the first step in writing a net ionic equation?
A) Write the balanced molecular equation
B) Write the ionic equation
C) Cancel spectator ions
D) Identify products
E) Write formulas for solids
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Answers with Explanations
1. B – Net ionic equations show only ions involved in the chemical change.
2. B – Spectator ions do not participate and are omitted.
3. B – Ag⁺ and Cl⁻ combine to form solid AgCl.
4. B – (s) denotes a solid precipitate.
5. B – To simplify by removing ions that do not change.
6. C – Na⁺ is a spectator ion in this reaction.
7. B – Spectator ions stay unchanged and are left out of the net ionic equation.
8. B – Neutralization is H⁺ + OH⁻ → H₂O.
9. D – You must write, dissociate, and cancel before finalizing.
10. B – Pb²⁺ and I⁻ form the precipitate PbI₂.
11. B – Calcium ion reacts with carbonate ion to form precipitate calcium carbonate.
12. C – Missing ions are spectators.
13. C – Spectator ions are not part of net ionic equations.
14. B – The gaseous product appears in the net ionic equation.
15. B – Net ionic equation for neutralization is H⁺ + OH⁻ → H₂O.
16. C – (s) indicates a solid precipitate.
17. B – Strong electrolytes dissociate into ions in ionic equations.
18. B – Silver ion and chloride ion form the solid precipitate silver chloride.
19. B – Net ionic equations highlight the actual chemical change.
20. A – Start with a balanced molecular equation.
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