AP Chemistry Flashcards: Net Ionic Equations

What this deck covers

This deck focuses on Net Ionic Equations, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: Identify the spectator ions in the reaction: $NaCl + AgNO_3 \rightarrow NaNO_3 + AgCl$?

Answer: $Na^+$ and $NO_3^-$ are spectator ions. These ions appear unchanged on both sides of the equation.

Flashcard 2: Identify the precipitate in the reaction: $Pb(NO_3)_2 + 2KI \rightarrow PbI_2 + 2KNO_3$.

Answer: $PbI_2$ is the precipitate. Lead iodide is insoluble and forms as a solid.

Flashcard 3: Which ions are typically not included in net ionic equations?

Answer: Spectator ions. They remain unchanged and don't participate in the reaction.

Flashcard 4: Identify the spectator ions in the reaction: $Na_2S + 2HCl \rightarrow 2NaCl + H_2S$.

Answer: $Na^+$ and $Cl^-$ are spectator ions. These ions remain in solution and don't react.

Flashcard 5: What is the net ionic equation for $H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O$?

Answer: $2H^+ + 2OH^- \rightarrow 2H_2O$. Diprotic acid neutralized by two hydroxide ions.

Flashcard 6: What is the net ionic equation for $2HCl + Mg \rightarrow MgCl_2 + H_2$?

Answer: $Mg + 2H^+ \rightarrow Mg^{2+} + H_2$. Active metal displaces hydrogen from acid.

Flashcard 7: Identify the spectator ions in the reaction: $Ca(NO_3)_2 + Na_2SO_4 \rightarrow CaSO_4 + 2NaNO_3$.

Answer: $Na^+$ and $NO_3^-$ are spectator ions. These ions don't participate in the precipitation.

Flashcard 8: What is the net ionic equation for $AgNO_3 + NaCl \rightarrow AgCl + NaNO_3$?

Answer: $Ag^+ + Cl^- \rightarrow AgCl$. Shows formation of insoluble silver chloride precipitate.

Flashcard 9: What is the net ionic equation for $K_2SO_4 + Ba(NO_3)_2 \rightarrow BaSO_4 + 2KNO_3$?

Answer: $Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Formation of insoluble barium sulfate from ionic reactants.

Flashcard 10: Write the net ionic equation for $CaCO_3 \rightarrow CaO + CO_2$.

Answer: No net ionic equation; no ions in the reaction. No ionic compounds are involved in this decomposition.

Flashcard 11: Write the net ionic equation for $NH_4Cl + NaOH \rightarrow NH_3 + NaCl + H_2O$.

Answer: $NH_4^+ + OH^- \rightarrow NH_3 + H_2O$. Base removes proton from ammonium to form ammonia.

Flashcard 12: What is the net ionic equation for $2NaOH + FeCl_2 \rightarrow Fe(OH)_2 + 2NaCl$?

Answer: $Fe^{2+} + 2OH^- \rightarrow Fe(OH)_2$. Iron hydroxide precipitates from solution.

Flashcard 13: What is the net ionic equation for $Zn + 2HCl \rightarrow ZnCl_2 + H_2$?

Answer: $Zn + 2H^+ \rightarrow Zn^{2+} + H_2$. Metal displacement reaction producing hydrogen gas.

Flashcard 14: What is the net ionic equation for $FeCl_3 + 3NaOH \rightarrow Fe(OH)_3 + 3NaCl$?

Answer: $Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3$. Iron hydroxide forms as an insoluble precipitate.

Flashcard 15: Identify the precipitate in the reaction: $Ca(OH)_2 + 2HCl \rightarrow CaCl_2 + 2H_2O$.

Answer: No precipitate; only water forms. This is an acid-base reaction, not precipitation.

Flashcard 16: What is the net ionic equation for $2NaOH + CuSO_4 \rightarrow Cu(OH)_2 + Na_2SO_4$?

Answer: $Cu^{2+} + 2OH^- \rightarrow Cu(OH)_2$. Hydroxide ions precipitate copper as insoluble hydroxide.

Flashcard 17: What is the net ionic equation for $2HCl + CaCO_3 \rightarrow CaCl_2 + CO_2 + H_2O$?

Answer: $2H^+ + CO_3^{2-} \rightarrow CO_2 + H_2O$. Carbonate reacts with acid to form gas and water.

Flashcard 18: Write the net ionic equation for $Na_2S + 2HCl \rightarrow 2NaCl + H_2S$.

Answer: $S^{2-} + 2H^+ \rightarrow H_2S$. Sulfide ion is protonated by acid to form gas.

Flashcard 19: Identify the precipitate in the reaction: $Mg(NO_3)_2 + 2NaOH \rightarrow Mg(OH)_2 + 2NaNO_3$.

Answer: $Mg(OH)_2$ is the precipitate. Magnesium hydroxide is insoluble in water.

Flashcard 20: State the definition of an acid-base reaction.

Answer: A reaction where an acid and a base react to form water and a salt. Proton transfer from acid to base forms neutral products.

Flashcard 21: Explain the role of spectator ions in a reaction.

Answer: They do not participate in the chemical change. They appear on both sides unchanged during reaction.

Flashcard 22: Identify the precipitate in the reaction: $AgNO_3 + NaBr \rightarrow AgBr + NaNO_3$.

Answer: $AgBr$ is the precipitate. Silver bromide is insoluble and precipitates.

Flashcard 23: Identify the spectator ions in the reaction: $KCl + AgNO_3 \rightarrow AgCl + KNO_3$.

Answer: $K^+$ and $NO_3^-$ are spectator ions. These ions are present but don't participate in reaction.

Flashcard 24: State the definition of a precipitation reaction.

Answer: A reaction where an insoluble solid forms and separates from solution. Soluble salts combine to form an insoluble product.

Flashcard 25: What is the net ionic equation for $K_2CO_3 + 2HNO_3 \rightarrow 2KNO_3 + CO_2 + H_2O$?

Answer: $CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate ion reacts with acid to produce gas.

Flashcard 26: Write the net ionic equation for $HCl + NaOH \rightarrow NaCl + H_2O$.

Answer: $H^+ + OH^- \rightarrow H_2O$. Shows only the acid-base neutralization, omitting spectators.

Flashcard 27: Write the net ionic equation for $2HCl + Mg(OH)_2 \rightarrow MgCl_2 + 2H_2O$.

Answer: $2H^+ + 2OH^- \rightarrow 2H_2O$. Acid-base reaction producing water from ions.

Flashcard 28: Write the net ionic equation for $Na_2CO_3 + 2HCl \rightarrow 2NaCl + CO_2 + H_2O$.

Answer: $CO_3^{2-} + 2H^+ \rightarrow CO_2 + H_2O$. Carbonate reacts with acid to produce gas and water.

Flashcard 29: What is a net ionic equation?

Answer: An equation showing only the species that change during the reaction. Shows only species that actually react or are produced.

Flashcard 30: Write the net ionic equation for $2NaCl + Pb(NO_3)_2 \rightarrow PbCl_2 + 2NaNO_3$.

Answer: $Pb^{2+} + 2Cl^- \rightarrow PbCl_2$. Lead chloride forms as an insoluble precipitate.

Flashcard 31: What does a complete ionic equation include?

Answer: All ions present in the reaction, including spectator ions. Shows both reacting and non-reacting ions in solution.

Flashcard 32: What is the net ionic equation for $BaCl_2 + Na_2SO_4 \rightarrow BaSO_4 + 2NaCl$?

Answer: $Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4$. Shows formation of insoluble barium sulfate precipitate.

Flashcard 33: Identify the precipitate in the reaction: $CaCl_2 + Na_2CO_3 \rightarrow CaCO_3 + 2NaCl$.

Answer: $CaCO_3$ is the precipitate. Calcium carbonate is insoluble in water.

Flashcard 34: Write the net ionic equation for $Al_2(SO_4)_3 + 3BaCl_2 \rightarrow 3BaSO_4 + 2AlCl_3$.

Answer: $3Ba^{2+} + 3SO_4^{2-} \rightarrow 3BaSO_4$. Three equivalents of precipitation reaction occur.