Question

identify whether each change represents an oxidation or reduction. then determine how many electrons were involved and which side of the reaction they should appear on in the half-reaction.

Answer 1

• Al ⇒ Al³⁺ is an oxidation and 3 electrons on the right side are needed.

• Cu²⁺ ⇒ Cu is a reduction and 2 electrons on the left side are needed.

• 2 F⁻ ⇒ F₂ is an oxidation and 2 electrons on the right side are needed.

In a redox reaction, we can identify 2 kinds of half-reactions:

• Oxidation: the oxidation number increases.
• Reduction: the oxidation number decreases.

Let's consider the following half-reactions.

• Al ⇒ Al³⁺

This is an oxidation because the oxidation number increases from 0 to 3+. To balance it, we need 3 electrons on the right side.

• Cu²⁺ ⇒ Cu

This is a reduction because the oxidation number decreases from 2+ to 0. To balance it, we need 2 electrons on the right side.

• 2 F⁻ ⇒ F₂

This is an oxidation because the oxidation number increases from -1 to 0. To balance it, we need 2 electrons on the right side.

• Al ⇒ Al³⁺ is an oxidation and 3 electrons on the right side are needed.

• Cu²⁺ ⇒ Cu is a reduction and 2 electrons on the left side are needed.

• 2 F⁻ ⇒ F₂ is an oxidation and 2 electrons on the right side are needed.

Learn more: https://brainly.com/question/2671074

Identify whether each change represents an oxidation or reduction. then determine how many electrons were involved and which side of the reaction they should appear on in the half-reaction.

Al ⇒ Al³⁺

Cu²⁺ ⇒ Cu

2 F⁻ ⇒ F₂