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Redox Processes

Each subtopic includes About section, revision page link, 10 preview questions, and practice CTAs.

Oxidation and reduction

Subtopic

Oxidation and reduction under Redox Processes for Grade 12 IB.

About Topic & Revision

Preview questions (no answers)

  1. 1.

    Which half-equation represents a reduction process?

    A.

    Zn→Zn2++2e−Zn \rightarrow Zn^{2+} + 2e^{-}

    B.

    2Cl−→Cl2+2e−2Cl^{-} \rightarrow Cl_{2} + 2e^{-}

    C.

    Fe2+→Fe3++e−Fe^{2+} \rightarrow Fe^{3+} + e^{-}

    D.

    Cu2++2e−→CuCu^{2+} + 2e^{-} \rightarrow Cu

  2. 2.

    In the reaction Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g)Mg(s) + 2HCl(aq) \rightarrow MgCl_{2}(aq) + H_{2}(g), which species acts as the reducing agent?

    A.

    Cl−Cl^{-}

    B.

    Mg(s)Mg(s)

    C.

    H+(aq)H^{+}(aq)

    D.

    MgCl2(aq)MgCl_{2}(aq)

  3. 3.

    What is the oxidation state of sulfur in the sulfate ion, SO42−SO_{4}^{2-}?

    A.

    +2

    B.

    +4

    C.

    +6

    D.

    -2

Download the worksheet for Redox Processes - Oxidation and reduction to practice offline. It includes additional chapter-level practice questions.

Electrochemical cells

Subtopic

Electrochemical cells under Redox Processes for Grade 12 IB.

About Topic & Revision

Preview questions (no answers)

  1. 1.

    Consider the following diagram of a voltaic cell consisting of Zinc and Copper half-cells. In which direction do the electrons flow through the external circuit?

    A.

    From the Cu electrode to the Zn electrode

    B.

    From the Zn electrode to the Cu electrode

    C.

    From the salt bridge to the Cu electrode

    D.

    From the Zn electrode into the salt bridge

  2. 2.

    Which statement correctly describes an electrolytic cell?

    A.

    It converts chemical energy into electrical energy.

    B.

    It involves a spontaneous redox reaction.

    C.

    It requires an external source of electrical energy to drive a non-spontaneous reaction.

    D.

    Oxidation occurs at the negative electrode.

  3. 3.

    What is the primary function of a salt bridge in a voltaic cell?

    A.

    To allow the flow of electrons between the two half-cells

    B.

    To provide a path for ions to move and maintain electrical neutrality

    C.

    To increase the overall cell potential (E⊖E^{\ominus})

    D.

    To act as a catalyst for the redox reaction

Download the worksheet for Redox Processes - Electrochemical cells to practice offline. It includes additional chapter-level practice questions.

Redox Processes - IB Grade 12 Chemistry Notes & Revision | Krit.club