Question

which of the following statements is true?
oxidation is the loss of electrons. when oxidized, charge becomes more negative.
reduction is the loss of electrons. when reduced, charge becomes more positive.
reduction is the loss of electrons. when reduced, charge becomes more negative.
oxidation is the gain of electrons. when oxidized, charge becomes more negative.
reduction is the gain of electrons. when reduced, charge becomes more negative.
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question 6
what chemical reaction is represented by the following half - reaction?
$i_2(g) + 2e^- \
ightarrow 2i^-(aq)$
oxidation
decomposition
reduction
replacement
combination

Explanation:

First Question (Which statement is TRUE?):

To determine the true statement, we recall the definitions of oxidation and reduction:

• Oxidation: Loss of electrons. When a species is oxidized, it loses electrons (negative charge), so its overall charge becomes more positive (e.g., \( \text{Fe}

ightarrow \text{Fe}^{2+} + 2e^- \), charge goes from 0 to +2).

• Reduction: Gain of electrons. When a species is reduced, it gains electrons (negative charge), so its overall charge becomes more negative (e.g., \( \text{Cl}_2 + 2e^-

ightarrow 2\text{Cl}^- \), charge goes from 0 to -1 per Cl).

Now, analyze each option:

• Option 1: "Oxidation is the loss of electrons. When oxidized, charge becomes more negative." → Incorrect (oxidation increases positive charge).
• Option 2: "Reduction is the loss of electrons. When reduced, charge becomes more positive." → Incorrect (reduction is gain of electrons, and charge becomes more negative).
• Option 3: "Reduction is the loss of electrons. When reduced, charge becomes more negative." → Incorrect (reduction is gain of electrons).
• Option 4: "Oxidation is the gain of electrons. When oxidized, charge becomes more negative." → Incorrect (oxidation is loss of electrons).
• Option 5: "Reduction is the gain of electrons. When reduced, charge becomes more negative." → Correct (matches the definitions: reduction = gain of electrons, and gaining electrons makes charge more negative).

Second Question (Half - reaction \( \boldsymbol{\text{I}_2(g) + 2e^-

ightarrow 2\text{I}^-(aq)} \)):

Recall:

• Oxidation: Loss of electrons (electrons are a product, e.g., \( \text{X}

ightarrow \text{X}^{+} + e^- \)).

• Reduction: Gain of electrons (electrons are a reactant, e.g., \( \text{Y} + e^-

ightarrow \text{Y}^- \)).

In the given half - reaction \( \text{I}_2(g) + 2e^-
ightarrow 2\text{I}^-(aq) \), electrons (\( e^- \)) are a reactant, meaning \( \text{I}_2 \) is gaining electrons. Thus, this is a reduction reaction.

Answer:

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First Question: