9.1 Oxidation and reduction

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Directly related questions

20N.2.sl.TZ0.1b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.sl.TZ0.1b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.sl.TZ0.b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.sl.TZ0.4d(ii):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
20N.2.sl.TZ0.4d(ii):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
20N.2.sl.TZ0.d(ii):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
20N.2.hl.TZ0.1b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.hl.TZ0.1b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.hl.TZ0.b(vi):
Deduce, referring to oxidation states, whether ${MnO}_{2}$ is an oxidizing or reducing agent.
20N.2.hl.TZ0.4d(iv):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
20N.2.hl.TZ0.4d(iv):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
20N.2.hl.TZ0.d(iv):
Suggest a metal that could replace nickel in a new half-cell and reverse the electron flow. Use section 25 of the data booklet.
17N.2.hl.TZ0.7d:
Identify the best reducing agent in the table above.
17N.2.hl.TZ0.7d:
Identify the best reducing agent in the table above.
17N.2.hl.TZ0.d:
Identify the best reducing agent in the table above.
17N.1.sl.TZ0.21:
What are the oxidation states of chromium in (NH₄)₂Cr₂O₇ (s) and Cr₂O₃ (s)?
17N.1.sl.TZ0.21:
What are the oxidation states of chromium in (NH₄)₂Cr₂O₇ (s) and Cr₂O₃ (s)?
21M.1.sl.TZ2.21: What is the oxidation state of oxygen in H2O2? A. −2 B. −1 C. +1 D. +2
21M.1.sl.TZ2.21: What is the oxidation state of oxygen in H2O2? A. −2 B. −1 C. +1 D. +2
21M.2.sl.TZ1.1d(ii): Deduce the change in the oxidation state of sulfur.
21M.2.sl.TZ1.d(ii): Deduce the change in the oxidation state of sulfur.
21M.2.sl.TZ1.1d(ii): Deduce the change in the oxidation state of sulfur.
21M.2.sl.TZ1.3d(i):
Write the half-equation for the reduction of hydrogen peroxide to water in acidic solution.
21M.2.sl.TZ1.3d(i):
Write the half-equation for the reduction of hydrogen peroxide to water in acidic solution.
21M.2.sl.TZ1.d(i):
Write the half-equation for the reduction of hydrogen peroxide to water in acidic solution.
21M.2.sl.TZ1.4b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21M.2.sl.TZ1.4b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21M.2.sl.TZ1.b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21M.2.hl.TZ1.1e(ii): Deduce the change in the oxidation state of sulfur.
21M.2.hl.TZ1.1e(ii): Deduce the change in the oxidation state of sulfur.
21M.2.hl.TZ1.e(ii): Deduce the change in the oxidation state of sulfur.
18M.2.hl.TZ2.4a:
In acidic solution, bromate ions, BrO₃⁻(aq), oxidize iodide ions, I⁻(aq).

BrO₃⁻(aq) + 6H⁺(aq) + 6e⁻ $\rightleftharpoons$ Br⁻(aq) + 3H₂O(l)

2I⁻(aq) $\rightleftharpoons$ I₂(s) + 2e⁻

Formulate the equation for the redox reaction.
18M.2.hl.TZ2.4a:
In acidic solution, bromate ions, BrO₃⁻(aq), oxidize iodide ions, I⁻(aq).

BrO₃⁻(aq) + 6H⁺(aq) + 6e⁻ $\rightleftharpoons$ Br⁻(aq) + 3H₂O(l)

2I⁻(aq) $\rightleftharpoons$ I₂(s) + 2e⁻

Formulate the equation for the redox reaction.
18M.2.hl.TZ2.a:
In acidic solution, bromate ions, BrO₃⁻(aq), oxidize iodide ions, I⁻(aq).

BrO₃⁻(aq) + 6H⁺(aq) + 6e⁻ $\rightleftharpoons$ Br⁻(aq) + 3H₂O(l)

2I⁻(aq) $\rightleftharpoons$ I₂(s) + 2e⁻

Formulate the equation for the redox reaction.
18M.1.sl.TZ2.22: Which can describe oxidation? A. Loss of hydrogen B. Decrease in oxidation number C. ...
18M.1.sl.TZ2.22: Which can describe oxidation? A. Loss of hydrogen B. Decrease in oxidation number C. ...
21N.2.hl.TZ0.6a: Outline what is measured by BOD.
21N.2.hl.TZ0.6a: Outline what is measured by BOD.
21N.2.hl.TZ0.a: Outline what is measured by BOD.
21N.2.hl.TZ0.6c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
21N.2.hl.TZ0.c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
21N.2.hl.TZ0.6c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
18N.2.hl.TZ0.3d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
18N.2.hl.TZ0.d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
18N.2.hl.TZ0.3d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
22M.1.sl.TZ1.21: In which of the following species would sulfur be reduced if converted to SCl2? A. S2O32– B. ...
22M.1.sl.TZ1.21: In which of the following species would sulfur be reduced if converted to SCl2? A. S2O32– B. ...
18N.2.hl.TZ0.3d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
18N.2.hl.TZ0.d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
18N.2.hl.TZ0.3d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
22M.1.sl.TZ1.23:
How many electrons are needed when the following half-equation is balanced using the lowest possible whole numbers?

__ NO₃^– (aq) + __ H⁺(aq) + __ e^– → __ NO (g) + __ H₂O (l)

A. 1

B. 2

C. 3

D. 5
22M.1.sl.TZ1.23:
How many electrons are needed when the following half-equation is balanced using the lowest possible whole numbers?

__ NO₃^– (aq) + __ H⁺(aq) + __ e^– → __ NO (g) + __ H₂O (l)

A. 1

B. 2

C. 3

D. 5
22M.1.sl.TZ2.21: Which species could be reduced to form NO2? A. N2 B. NO3− C. HNO2 D. NO
22M.1.sl.TZ2.21: Which species could be reduced to form NO2? A. N2 B. NO3− C. HNO2 D. NO
22M.2.hl.TZ1.1d(iii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.hl.TZ1.1d(iii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.hl.TZ1.d(iii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.hl.TZ1.1d(iv):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.hl.TZ1.1d(iv):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.hl.TZ1.d(iv):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.sl.TZ2.5a:
Deduce the half-equations for the reaction at each electrode.
22M.2.sl.TZ2.5a:
Deduce the half-equations for the reaction at each electrode.
22M.2.sl.TZ2.a:
Deduce the half-equations for the reaction at each electrode.
22M.2.hl.TZ2.5b:
Calculate the oxidation state of sulfur in iron(II) disulfide, FeS₂.
22M.2.hl.TZ2.5b:
Calculate the oxidation state of sulfur in iron(II) disulfide, FeS₂.
22M.2.hl.TZ2.b:
Calculate the oxidation state of sulfur in iron(II) disulfide, FeS₂.
19M.2.hl.TZ1.2g:
The combustion reaction in (f)(ii) can also be classed as redox. Identify the atom that is oxidized and the atom that is reduced.
19M.2.hl.TZ1.2g:
The combustion reaction in (f)(ii) can also be classed as redox. Identify the atom that is oxidized and the atom that is reduced.
19M.2.hl.TZ1.g:
The combustion reaction in (f)(ii) can also be classed as redox. Identify the atom that is oxidized and the atom that is reduced.
19M.2.hl.TZ1.4b(v):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.hl.TZ1.4b(v):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.hl.TZ1.b(v):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.hl.TZ2.1d(ii):
Deduce the average oxidation state of carbon in product B.
19M.2.hl.TZ2.1d(ii):
Deduce the average oxidation state of carbon in product B.
19M.2.hl.TZ2.d(ii):
Deduce the average oxidation state of carbon in product B.
19M.2.hl.TZ2.4e(ii):
Deduce the coefficients required to complete the half-equation.

ReO₄⁻ (aq) + ____H⁺ (aq) + ____e⁻ ⇌ [Re(OH)₂]²⁺ (aq) + ____H₂O (l) E^θ = +0.36 V
19M.2.hl.TZ2.e(ii):
Deduce the coefficients required to complete the half-equation.

ReO₄⁻ (aq) + ____H⁺ (aq) + ____e⁻ ⇌ [Re(OH)₂]²⁺ (aq) + ____H₂O (l) E^θ = +0.36 V
19M.2.hl.TZ2.4e(ii):
Deduce the coefficients required to complete the half-equation.

ReO₄⁻ (aq) + ____H⁺ (aq) + ____e⁻ ⇌ [Re(OH)₂]²⁺ (aq) + ____H₂O (l) E^θ = +0.36 V
19M.2.hl.TZ2.4d(i):
State the name of this compound, applying IUPAC rules.
19M.2.hl.TZ2.4d(i):
State the name of this compound, applying IUPAC rules.
19M.2.hl.TZ2.d(i):
State the name of this compound, applying IUPAC rules.
19M.2.sl.TZ1.4b(iv):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.sl.TZ1.4b(iv):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.sl.TZ1.b(iv):
MnO₂ is another possible catalyst for the reaction. State the IUPAC name for MnO₂.
19M.2.sl.TZ2.1d(ii):
Deduce the average oxidation state of carbon in product B.
19M.2.sl.TZ2.1d(ii):
Deduce the average oxidation state of carbon in product B.
19M.2.sl.TZ2.d(ii):
Deduce the average oxidation state of carbon in product B.
19M.1.sl.TZ2.21: Which species contains nitrogen with the highest oxidation state? A. NO3− B. NO2− C. NO2 D. N2O
19M.1.sl.TZ2.21: Which species contains nitrogen with the highest oxidation state? A. NO3− B. NO2− C. NO2 D. N2O
19M.1.sl.TZ1.22:
Which is the species oxidized and the oxidizing agent in the reaction?

MnO₂ (s) + 4HCl (aq) → MnCl₂ (aq) + Cl₂ (g) + 2H₂O (l)
19M.1.sl.TZ1.22:
Which is the species oxidized and the oxidizing agent in the reaction?

MnO₂ (s) + 4HCl (aq) → MnCl₂ (aq) + Cl₂ (g) + 2H₂O (l)
22N.1.sl.TZ0.22:
Which substance is the reducing agent in the given reaction?

H⁺ (aq) + 2H₂O (l) + 2MnO₄⁻ (aq) + 5SO₂ (g) → 2Mn²⁺ (aq) + 5HSO₄⁻ (aq)

A. H⁺

B. H₂O

C. MnO₄⁻

D. SO₂
22N.1.sl.TZ0.22:
Which substance is the reducing agent in the given reaction?

H⁺ (aq) + 2H₂O (l) + 2MnO₄⁻ (aq) + 5SO₂ (g) → 2Mn²⁺ (aq) + 5HSO₄⁻ (aq)

A. H⁺

B. H₂O

C. MnO₄⁻

D. SO₂
17N.1.sl.TZ0.22:
Which of the following is a redox reaction?

A. 3Mg (s) + 2AlCl₃ (aq) → 2Al (s) + 3MgCl₂ (aq)

B. SiO₂ (s) + 2NaOH (aq) → Na₂SiO₃ (aq) + H₂O (l)

C. KCl (aq) + AgNO₃ (aq) → AgCl (s) + KNO₃ (aq)

D. 2NaHCO₃ (aq) → Na₂CO₃ (aq) + CO₂ (g) + H₂O (l)
17N.1.sl.TZ0.22:
Which of the following is a redox reaction?

A. 3Mg (s) + 2AlCl₃ (aq) → 2Al (s) + 3MgCl₂ (aq)

B. SiO₂ (s) + 2NaOH (aq) → Na₂SiO₃ (aq) + H₂O (l)

C. KCl (aq) + AgNO₃ (aq) → AgCl (s) + KNO₃ (aq)

D. 2NaHCO₃ (aq) → Na₂CO₃ (aq) + CO₂ (g) + H₂O (l)
17N.1.hl.TZ0.30:
Consider the following half-equations:

I₂ (s) + 2e^– $\rightleftharpoons$ 2I^– (aq) E^θ = +0.54 V
(brown) (colourless)

MnO₄^– (aq) + 8H⁺ (aq) + 5e^– $\rightleftharpoons$ Mn²⁺ (aq) + 4H₂O (l) E^θ = +1.51 V
(purple) (colourless)

Which statement is correct for the reaction between KMnO₄ (aq) and KI (aq) in acidic conditions?

A. MnO₄^– reduces I^– to I₂.

B. I^– reduces MnO₄^– to Mn²⁺.

C. The colour changes from brown to purple.

D. MnO₄^– is oxidized to Mn²⁺.
17N.1.hl.TZ0.30:
Consider the following half-equations:

I₂ (s) + 2e^– $\rightleftharpoons$ 2I^– (aq) E^θ = +0.54 V
(brown) (colourless)

MnO₄^– (aq) + 8H⁺ (aq) + 5e^– $\rightleftharpoons$ Mn²⁺ (aq) + 4H₂O (l) E^θ = +1.51 V
(purple) (colourless)

Which statement is correct for the reaction between KMnO₄ (aq) and KI (aq) in acidic conditions?

A. MnO₄^– reduces I^– to I₂.

B. I^– reduces MnO₄^– to Mn²⁺.

C. The colour changes from brown to purple.

D. MnO₄^– is oxidized to Mn²⁺.
17N.2.sl.TZ0.2e.i: Identify the strongest reducing agent in the given list.
17N.2.sl.TZ0.2e.i: Identify the strongest reducing agent in the given list.
17N.2.sl.TZ0.e.i: Identify the strongest reducing agent in the given list.
18M.1.sl.TZ1.21:
Which equation shows oxygen undergoing reduction?

A. 2F₂ + O₂ → 2F₂O

B. Na₂O + H₂O → 2NaOH

C. H₂O₂ + 2HI → 2H₂O + I₂

D. 2CrO₄²⁻ + 2H⁺ $\rightleftharpoons$ Cr₂O₇²⁻ + H₂O
18M.1.sl.TZ1.21:
Which equation shows oxygen undergoing reduction?

A. 2F₂ + O₂ → 2F₂O

B. Na₂O + H₂O → 2NaOH

C. H₂O₂ + 2HI → 2H₂O + I₂

D. 2CrO₄²⁻ + 2H⁺ $\rightleftharpoons$ Cr₂O₇²⁻ + H₂O
18M.1.sl.TZ1.23:
Which coefficients correctly balance this redox equation?

aFe²⁺(aq) + MnO₄⁻(aq) + bH⁺(aq) → cFe³⁺(aq) + Mn²⁺(aq) + dH₂O(l)
18M.1.sl.TZ1.23:
Which coefficients correctly balance this redox equation?

aFe²⁺(aq) + MnO₄⁻(aq) + bH⁺(aq) → cFe³⁺(aq) + Mn²⁺(aq) + dH₂O(l)
18M.1.sl.TZ2.21: Which element has the same oxidation number in both species? A. C in C2H4 and CO2 B. H...
18M.1.sl.TZ2.21: Which element has the same oxidation number in both species? A. C in C2H4 and CO2 B. H...
18N.1.sl.TZ0.21:
Which is correct for the reaction?

P₄ (s) + 3H₂O (l) + 3OH⁻ (aq) → PH₃ (g) + 3H₂PO₂⁻ (aq)
18N.1.sl.TZ0.21:
Which is correct for the reaction?

P₄ (s) + 3H₂O (l) + 3OH⁻ (aq) → PH₃ (g) + 3H₂PO₂⁻ (aq)
18N.1.sl.TZ0.23: Which represents a reduction? A. SO3 to SO42− B. Mn2O3 to MnO2 C. H2O2 to OH− D. ...
18N.1.sl.TZ0.23: Which represents a reduction? A. SO3 to SO42− B. Mn2O3 to MnO2 C. H2O2 to OH− D. ...
18N.2.sl.TZ0.2d.ii: Deduce the average oxidation state of carbon in propan-2-ol.
18N.2.sl.TZ0.2d.ii: Deduce the average oxidation state of carbon in propan-2-ol.
18N.2.sl.TZ0.d.ii: Deduce the average oxidation state of carbon in propan-2-ol.
18N.2.sl.TZ0.3d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
18N.2.sl.TZ0.3d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
18N.2.sl.TZ0.d.i:
Bromate(V) ions act as oxidizing agents in acidic conditions to form bromide ions.

Deduce the half-equation for this reduction reaction.
18N.2.sl.TZ0.3d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
18N.2.sl.TZ0.3d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
18N.2.sl.TZ0.d.ii:
Bromate(V) ions oxidize iron(II) ions, Fe²⁺, to iron(III) ions, Fe³⁺.

Deduce the equation for this redox reaction.
18N.2.hl.TZ0.6a.iii: Deduce the average oxidation state of carbon in butanoic acid.
18N.2.hl.TZ0.6a.iii: Deduce the average oxidation state of carbon in butanoic acid.
18N.2.hl.TZ0.a.iii: Deduce the average oxidation state of carbon in butanoic acid.
19M.2.hl.TZ1.3k:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.hl.TZ1.3k:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.hl.TZ1.k:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.hl.TZ2.4c:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.2.hl.TZ2.4c:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.2.hl.TZ2.c:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.3.hl.TZ1.1b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19M.3.hl.TZ1.1b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19M.3.hl.TZ1.b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19M.1.hl.TZ2.28: Which compound contains sulfur with an oxidation state of +6? A. SO2 B. H2S C. H2SO3 D. H2SO4
19M.1.hl.TZ2.28: Which compound contains sulfur with an oxidation state of +6? A. SO2 B. H2S C. H2SO3 D. H2SO4
19M.2.sl.TZ1.3e:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.sl.TZ1.3e:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.sl.TZ1.e:
State the oxidation number of carbon in sodium carbonate, Na₂CO₃.
19M.2.sl.TZ2.4b:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.2.sl.TZ2.4b:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.2.sl.TZ2.b:
Describe how the relative reactivity of rhenium, compared to silver, zinc, and copper, can be established using pieces of rhenium and solutions of these metal sulfates.
19M.2.sl.TZ2.4c(i):
State the name of this compound, applying IUPAC rules.
19M.2.sl.TZ2.4c(i):
State the name of this compound, applying IUPAC rules.
19M.2.sl.TZ2.c(i):
State the name of this compound, applying IUPAC rules.
19M.3.sl.TZ1.1b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19M.3.sl.TZ1.1b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19M.3.sl.TZ1.b(iii):
Compare the ease of oxidation of s-block and d-block metals to their melting points and densities. Use section 25 of the data booklet.
19N.3.sl.TZ0.2a(ii): Determine the change in the average oxidation state of carbon. From ethanol to ethanal: From...
19N.3.sl.TZ0.2a(ii): Determine the change in the average oxidation state of carbon. From ethanol to ethanal: From...
19N.3.sl.TZ0.a(ii): Determine the change in the average oxidation state of carbon. From ethanol to ethanal: From...
19N.3.sl.TZ0.2a(iii): List the three products at the anode from the least to the most oxidized.
19N.3.sl.TZ0.2a(iii): List the three products at the anode from the least to the most oxidized.
19N.3.sl.TZ0.a(iii): List the three products at the anode from the least to the most oxidized.
19N.3.sl.TZ0.2b: Deduce, giving your reason, which catalyst is most effective at fully oxidizing ethanol.
19N.3.sl.TZ0.2b: Deduce, giving your reason, which catalyst is most effective at fully oxidizing ethanol.
19N.3.sl.TZ0.b: Deduce, giving your reason, which catalyst is most effective at fully oxidizing ethanol.
19N.3.sl.TZ0.5a:
Discuss why different methods of reduction are needed to extract metals.
19N.3.sl.TZ0.5a:
Discuss why different methods of reduction are needed to extract metals.
19N.3.sl.TZ0.a:
Discuss why different methods of reduction are needed to extract metals.
19N.1.sl.TZ0.22: In which species does sulfur have the same oxidation state as in SO32–? A. S2O32– B. ...
19N.1.sl.TZ0.22: In which species does sulfur have the same oxidation state as in SO32–? A. S2O32– B. ...
19N.1.sl.TZ0.23:
The following occurs when metal X is added to Y sulfate solution and Z sulfate solution. (X, Y and Z represent metal elements but not their symbols.)

X (s) + YSO₄ (aq) → XSO₄ (aq) + Y (s)
X (s) + ZSO₄ (aq): no reaction

What is the order of increasing reactivity?

A. X < Y < Z

B. Y < X < Z

C. Z < Y < X

D. Z < X < Y
19N.1.sl.TZ0.23:
The following occurs when metal X is added to Y sulfate solution and Z sulfate solution. (X, Y and Z represent metal elements but not their symbols.)

X (s) + YSO₄ (aq) → XSO₄ (aq) + Y (s)
X (s) + ZSO₄ (aq): no reaction

What is the order of increasing reactivity?

A. X < Y < Z

B. Y < X < Z

C. Z < Y < X

D. Z < X < Y
20N.1.sl.TZ0.23: What are the oxidation states of oxygen?
20N.1.sl.TZ0.23: What are the oxidation states of oxygen?
20N.2.sl.TZ0.1b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
20N.2.sl.TZ0.1b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
20N.2.sl.TZ0.b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
20N.2.hl.TZ0.1b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
20N.2.hl.TZ0.1b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
20N.2.hl.TZ0.b(v):
State the oxidation state of manganese in ${MnO}_{2}$ and ${MnCl}_{2}$ .
21M.1.sl.TZ1.21: A student performed displacement reactions using metals W and X and solutions of salts of metals...
21M.1.sl.TZ1.21: A student performed displacement reactions using metals W and X and solutions of salts of metals...
21M.1.sl.TZ1.22:
What is correct for this redox reaction?

MnO₂(s) + 2 $I$ ⁻ (aq) + 4H⁺(aq) → Mn²⁺(aq) + $I$ ₂(aq) + 2H₂O (l)
21M.1.sl.TZ1.22:
What is correct for this redox reaction?

MnO₂(s) + 2 $I$ ⁻ (aq) + 4H⁺(aq) → Mn²⁺(aq) + $I$ ₂(aq) + 2H₂O (l)
21M.2.sl.TZ1.3d(ii):
Deduce a balanced equation for the oxidation of Fe2+ by acidified hydrogen peroxide.
21M.2.sl.TZ1.3d(ii):
Deduce a balanced equation for the oxidation of Fe2+ by acidified hydrogen peroxide.
21M.2.sl.TZ1.d(ii):
Deduce a balanced equation for the oxidation of Fe2+ by acidified hydrogen peroxide.
21M.2.hl.TZ1.4b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21M.2.hl.TZ1.4b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21M.2.hl.TZ1.b: The hydrogen peroxide could cause further oxidation of the methanol. Suggest a possible oxidation...
21N.1.sl.TZ0.22:
What is the change in the oxidation state of oxygen?

2Fe²⁺(aq) + H₂O₂(aq) + 2H⁺(aq) → 2H₂O (l) + 2Fe³⁺(aq)

A. +1

B. 0

C. −1

D. −2
21N.1.sl.TZ0.22:
What is the change in the oxidation state of oxygen?

2Fe²⁺(aq) + H₂O₂(aq) + 2H⁺(aq) → 2H₂O (l) + 2Fe³⁺(aq)

A. +1

B. 0

C. −1

D. −2
21N.2.sl.TZ0.6a: Outline what is measured by BOD.
21N.2.sl.TZ0.6a: Outline what is measured by BOD.
21N.2.sl.TZ0.a: Outline what is measured by BOD.
21N.2.sl.TZ0.6c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
21N.2.sl.TZ0.6c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
21N.2.sl.TZ0.c(iv):
The three steps of the Winkler Method are redox reactions.

Deduce the reduction half-equation for step II.
22M.1.sl.TZ2.11:
What is the name of the compound with formula Ti₃(PO₄)₂?

A. Titanium phosphate

B. Titanium(II) phosphate

C. Titanium(III) phosphate

D. Titanium(IV) phosphate
22M.1.sl.TZ2.11:
What is the name of the compound with formula Ti₃(PO₄)₂?

A. Titanium phosphate

B. Titanium(II) phosphate

C. Titanium(III) phosphate

D. Titanium(IV) phosphate
22M.1.sl.TZ2.22:
Which combination best describes what is happening to chloromethane, CH₃Cl, in the equation below?

CH₃Cl (g) + H₂(g) $⇌$ CH₄(g) + HCl (g)

A. Oxidation and addition

B. Oxidation and substitution

C. Reduction and addition

D. Reduction and substitution
22M.1.sl.TZ2.22:
Which combination best describes what is happening to chloromethane, CH₃Cl, in the equation below?

CH₃Cl (g) + H₂(g) $⇌$ CH₄(g) + HCl (g)

A. Oxidation and addition

B. Oxidation and substitution

C. Reduction and addition

D. Reduction and substitution
22M.2.sl.TZ1.1d(ii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.sl.TZ1.1d(ii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.sl.TZ1.d(ii): Determine the oxidation state of nitrogen in Mg3N2 and in NH3.
22M.2.sl.TZ1.1d(iii):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.sl.TZ1.1d(iii):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.sl.TZ1.d(iii):
Deduce, giving reasons, whether the reaction of magnesium nitride with water is an acid–base reaction, a redox reaction, neither or both.
22M.2.sl.TZ1.3b:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.sl.TZ1.3b:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.sl.TZ1.b:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.hl.TZ1.2a:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.hl.TZ1.2a:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.hl.TZ1.a:
Suggest an experiment that shows that magnesium is more reactive than zinc, giving the observation that would confirm this.
22M.2.sl.TZ2.1c: The reaction of lithium with water is a redox reaction. Identify the oxidizing agent in the...
22M.2.sl.TZ2.1c: The reaction of lithium with water is a redox reaction. Identify the oxidizing agent in the...
22M.2.sl.TZ2.c: The reaction of lithium with water is a redox reaction. Identify the oxidizing agent in the...
22M.2.sl.TZ2.5b:
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
22M.2.sl.TZ2.5b:
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
22M.2.sl.TZ2.b:
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
22M.2.hl.TZ2.3b(i):
Molten zinc chloride undergoes electrolysis in an electrolytic cell at 450 °C.

Deduce the half-equations for the reaction at each electrode.
22M.2.hl.TZ2.3b(i):
Molten zinc chloride undergoes electrolysis in an electrolytic cell at 450 °C.

Deduce the half-equations for the reaction at each electrode.
22M.2.hl.TZ2.b(i):
Molten zinc chloride undergoes electrolysis in an electrolytic cell at 450 °C.

Deduce the half-equations for the reaction at each electrode.
22M.2.hl.TZ2.3b(ii):
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
22M.2.hl.TZ2.3b(ii):
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
22M.2.hl.TZ2.b(ii):
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
23M.2.HL.TZ2.3a:
An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).
23M.2.HL.TZ2.3a:
An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).
23M.2.HL.TZ2.a:
An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).

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9.1 Oxidation and reduction

Description

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