Oxidation-Reduction Reactions, Oxidation States, and Ionic Equations

Vocabulary practice flashcards covering assigning oxidation states, identifying redox reactions, determining oxidizing and reducing agents, and formulating balanced complete and net ionic equations for acid-base reactions.

Reducing Agent in $Al_{(s)} + 3Ag^+_{(aq)} \rightarrow Al^{3+}_{(aq)} + 3Ag_{(s)}$

$Al_{(s)}$, which is oxidized from an oxidation state of $0$ to $+3$ by donating electrons.

Oxidizing Agent in $Al_{(s)} + 3Ag^+_{(aq)} \rightarrow Al^{3+}_{(aq)} + 3Ag_{(s)}$

$Ag^+_{(aq)}$, which is reduced from an oxidation state of $+1$ to $0$ by accepting electrons.

Oxidizing Agent in $Ba_{(s)} + Cl_{2(g)} \rightarrow BaCl_{2(s)}$

$Cl_{2(g)}$, which gains electrons to undergo reduction, oxidizing barium metal.

Oxidizing Agent in $Mg_{(s)} + Br_{2(l)} \rightarrow MgBr_{2(s)}$

$Br_{2(l)}$, which is reduced to bromide ions by accepting electrons from magnesium.

Reaction Classification of $SO_{3(g)} + H_2O_{(l)} \rightarrow H_2SO_{4(aq)}$

A non-redox acid anhydride hydration reaction in which no element changes its oxidation state ($S = +6$, $O = -2$, $H = +1$ on both sides).

Oxidation State of Nitrogen in $N_2$

$0$, because the oxidation state of any pure, uncombined elemental form is zero.

Oxidation State of Lithium in $Li^+$

$+1$, identical to the ionic charge of the monoatomic cation.

Oxidation States in $Fe_2O_3$

$+3$ for $Fe$ and $-2$ for $O$, yielding a neutral compound ($2(+3) + 3(-2) = 0$).

Oxidation States in $MnO_4^-$

$+7$ for $Mn$ and $-2$ for $O$, adding up to the overall ion charge of $-1$ ($+7 + 4(-2) = -1$).

Oxidation States in $HCO_3^-$

$+1$ for $H$, $+4$ for $C$, and $-2$ for $O$, totaling the overall ion charge of $-1$ ($+1 + (+4) + 3(-2) = -1$).

Complete Ionic Equation for $HC_2H_3O_{2(aq)} + LiOH_{(aq)}$

HC_2H_3O_{2(aq)} + Li^+_{(aq)} + OH^-_{(aq)} \rightarrow H_2O_{(l)} + Li^+_{(aq)} + C_2H_3O_2^-_{(aq)}, representing the weak acid in undissociated form and the soluble strong electrolytes as separate ions.

Net Ionic Equation for $HC_2H_3O_{2(aq)} + LiOH_{(aq)}$

HC_2H_3O_{2(aq)} + OH^-_{(aq)} \rightarrow H_2O_{(l)} + C_2H_3O_2^-_{(aq)}, determined by eliminating the spectator ion ($Li^+_{(aq)}$) from the complete ionic equation.