Oxidation-Reduction (Redox) Reactions - AP Chemistry
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What happens to the oxidation state of an element during oxidation?
What happens to the oxidation state of an element during oxidation?
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Increases. Oxidation involves loss of electrons.
Increases. Oxidation involves loss of electrons.
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What is the oxidation state of sulfur in $H_2SO_4$?
What is the oxidation state of sulfur in $H_2SO_4$?
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+6. Calculate using: 2(+1) + S + 4(-2) = 0, so S = +6.
+6. Calculate using: 2(+1) + S + 4(-2) = 0, so S = +6.
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Identify the element reduced in the reaction: $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$.
Identify the element reduced in the reaction: $Fe + CuSO_4 \rightarrow FeSO_4 + Cu$.
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$Cu$. Copper's oxidation state decreases from +2 to 0.
$Cu$. Copper's oxidation state decreases from +2 to 0.
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What is the role of the oxidizing agent in a redox reaction?
What is the role of the oxidizing agent in a redox reaction?
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Accepts electrons. It gains electrons and gets reduced itself.
Accepts electrons. It gains electrons and gets reduced itself.
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Identify the element oxidized: $2K + Br_2 \rightarrow 2KBr$.
Identify the element oxidized: $2K + Br_2 \rightarrow 2KBr$.
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$K$. Potassium's oxidation state increases from 0 to +1.
$K$. Potassium's oxidation state increases from 0 to +1.
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What is the oxidation state of aluminum in $Al_2O_3$?
What is the oxidation state of aluminum in $Al_2O_3$?
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+3. Calculate using: 2(Al) + 3(-2) = 0, so Al = +3.
+3. Calculate using: 2(Al) + 3(-2) = 0, so Al = +3.
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Define 'redox reaction'.
Define 'redox reaction'.
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A reaction involving electron transfer. Involves oxidation and reduction occurring simultaneously.
A reaction involving electron transfer. Involves oxidation and reduction occurring simultaneously.
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Identify the reducing agent in the reaction: $2H_2 + O_2 \rightarrow 2H_2O$.
Identify the reducing agent in the reaction: $2H_2 + O_2 \rightarrow 2H_2O$.
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$H_2$. $H_2$ loses electrons, so it's the reducing agent.
$H_2$. $H_2$ loses electrons, so it's the reducing agent.
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Identify the reducing agent: $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$.
Identify the reducing agent: $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$.
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$Zn$. $Zn$ loses electrons and gets oxidized.
$Zn$. $Zn$ loses electrons and gets oxidized.
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Find the oxidation state of nitrogen in $NO_3^-$.
Find the oxidation state of nitrogen in $NO_3^-$.
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+5. Calculate using: N + 3(-2) = -1, so N = +5.
+5. Calculate using: N + 3(-2) = -1, so N = +5.
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What is reduction in a redox reaction?
What is reduction in a redox reaction?
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Gain of electrons. Reduction involves gaining electrons from another species.
Gain of electrons. Reduction involves gaining electrons from another species.
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What is the oxidation state of phosphorus in $H_3PO_4$?
What is the oxidation state of phosphorus in $H_3PO_4$?
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+5. Calculate using: 3(+1) + P + 4(-2) = 0, so P = +5.
+5. Calculate using: 3(+1) + P + 4(-2) = 0, so P = +5.
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What is the oxidation state of carbon in $CO_2$?
What is the oxidation state of carbon in $CO_2$?
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+4. Calculate using: C + 2(-2) = 0, so C = +4.
+4. Calculate using: C + 2(-2) = 0, so C = +4.
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What happens to the oxidation state of an element during reduction?
What happens to the oxidation state of an element during reduction?
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Decreases. Reduction involves gain of electrons.
Decreases. Reduction involves gain of electrons.
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State the oxidation state of chlorine in $Cl_2$.
State the oxidation state of chlorine in $Cl_2$.
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- Diatomic chlorine is in its elemental state.
- Diatomic chlorine is in its elemental state.
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What is the oxidation state of nitrogen in $NH_3$?
What is the oxidation state of nitrogen in $NH_3$?
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-3. Calculate using: 3(+1) + N = 0, so N = -3.
-3. Calculate using: 3(+1) + N = 0, so N = -3.
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What is the change in oxidation state for iron in $Fe_2O_3$ during reduction?
What is the change in oxidation state for iron in $Fe_2O_3$ during reduction?
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Decreases from +3 to 0. Reduction decreases oxidation state by gaining electrons.
Decreases from +3 to 0. Reduction decreases oxidation state by gaining electrons.
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What is the oxidation state of oxygen in most compounds?
What is the oxidation state of oxygen in most compounds?
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-2. Oxygen typically has -2 oxidation state in compounds.
-2. Oxygen typically has -2 oxidation state in compounds.
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What is oxidation in a redox reaction?
What is oxidation in a redox reaction?
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Loss of electrons. Oxidation involves losing electrons to another species.
Loss of electrons. Oxidation involves losing electrons to another species.
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What is the oxidation state of sulfur in $SO_2$?
What is the oxidation state of sulfur in $SO_2$?
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+4. Calculate using: S + 2(-2) = 0, so S = +4.
+4. Calculate using: S + 2(-2) = 0, so S = +4.
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In redox terminology, what is a half-reaction?
In redox terminology, what is a half-reaction?
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Reaction showing either oxidation or reduction alone. Shows one part of the complete redox process.
Reaction showing either oxidation or reduction alone. Shows one part of the complete redox process.
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What is the change in oxidation state for copper in $CuO$ during reduction?
What is the change in oxidation state for copper in $CuO$ during reduction?
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Decreases from +2 to 0. Reduction decreases oxidation state by gaining electrons.
Decreases from +2 to 0. Reduction decreases oxidation state by gaining electrons.
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Identify the reducing agent in the reaction: $2H_2 + O_2 \rightarrow 2H_2O$.
Identify the reducing agent in the reaction: $2H_2 + O_2 \rightarrow 2H_2O$.
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$H_2$. $H_2$ loses electrons, so it's the reducing agent.
$H_2$. $H_2$ loses electrons, so it's the reducing agent.
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What is the role of the oxidizing agent in a redox reaction?
What is the role of the oxidizing agent in a redox reaction?
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Accepts electrons. It gains electrons and gets reduced itself.
Accepts electrons. It gains electrons and gets reduced itself.
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Identify the element oxidized: $2K + Br_2 \rightarrow 2KBr$.
Identify the element oxidized: $2K + Br_2 \rightarrow 2KBr$.
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$K$. Potassium's oxidation state increases from 0 to +1.
$K$. Potassium's oxidation state increases from 0 to +1.
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What is the oxidation state of sulfur in $H_2SO_4$?
What is the oxidation state of sulfur in $H_2SO_4$?
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+6. Calculate using: 2(+1) + S + 4(-2) = 0, so S = +6.
+6. Calculate using: 2(+1) + S + 4(-2) = 0, so S = +6.
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What happens to the oxidation state of an element during oxidation?
What happens to the oxidation state of an element during oxidation?
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Increases. Oxidation involves loss of electrons.
Increases. Oxidation involves loss of electrons.
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State the oxidation state of chlorine in $NaCl$.
State the oxidation state of chlorine in $NaCl$.
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-1. Chlorine gains one electron to form chloride ion.
-1. Chlorine gains one electron to form chloride ion.
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What is the oxidation state of carbon in $CH_4$?
What is the oxidation state of carbon in $CH_4$?
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-4. Calculate using: C + 4(+1) = 0, so C = -4.
-4. Calculate using: C + 4(+1) = 0, so C = -4.
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Find the oxidation state of chromium in $Cr_2O_7^{2-}$.
Find the oxidation state of chromium in $Cr_2O_7^{2-}$.
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+6. Calculate using: 2(Cr) + 7(-2) = -2, so Cr = +6.
+6. Calculate using: 2(Cr) + 7(-2) = -2, so Cr = +6.
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