Question
Which best describes the electron transfer that occurs during this oxidation-reduction reaction?
4Al+3O
2
→2Al
2
O
3
A. Each oxygen atom gained four electrons, and each aluminum atom lost three electrons.
B. Each oxygen atom gained three electrons, and each aluminum atom lost two electrons.
C. Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.
D. Each oxygen atom gained three electrons, and each aluminum atom lost four electrons.
4Al+3O
2
→2Al
2
O
3
A. Each oxygen atom gained four electrons, and each aluminum atom lost three electrons.
B. Each oxygen atom gained three electrons, and each aluminum atom lost two electrons.
C. Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.
D. Each oxygen atom gained three electrons, and each aluminum atom lost four electrons.
Answers
Answered by
GPT-4o mini
To analyze the oxidation-reduction reaction given:
\[ 4 \text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3 \]
we can identify the changes in oxidation states for the reactants and products.
1. **Aluminum (Al)**: In the elemental form, aluminum has an oxidation state of 0. In aluminum oxide (\(\text{Al}_2\text{O}_3\)), aluminum has an oxidation state of +3. Therefore, each aluminum atom loses 3 electrons when going from 0 to +3.
2. **Oxygen (O)**: In the elemental form (\(\text{O}_2\)), oxygen has an oxidation state of 0. In aluminum oxide, oxygen has an oxidation state of -2. Therefore, each oxygen atom gains 2 electrons when going from 0 to -2.
Given this understanding, we can summarize the electron transfer as:
- Each aluminum atom loses 3 electrons.
- Each oxygen atom gains 2 electrons.
Now, let's review the options:
A. Each oxygen atom gained four electrons, and each aluminum atom lost three electrons.
B. Each oxygen atom gained three electrons, and each aluminum atom lost two electrons.
C. Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.
D. Each oxygen atom gained three electrons, and each aluminum atom lost four electrons.
The correct description is **C**: Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.
\[ 4 \text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3 \]
we can identify the changes in oxidation states for the reactants and products.
1. **Aluminum (Al)**: In the elemental form, aluminum has an oxidation state of 0. In aluminum oxide (\(\text{Al}_2\text{O}_3\)), aluminum has an oxidation state of +3. Therefore, each aluminum atom loses 3 electrons when going from 0 to +3.
2. **Oxygen (O)**: In the elemental form (\(\text{O}_2\)), oxygen has an oxidation state of 0. In aluminum oxide, oxygen has an oxidation state of -2. Therefore, each oxygen atom gains 2 electrons when going from 0 to -2.
Given this understanding, we can summarize the electron transfer as:
- Each aluminum atom loses 3 electrons.
- Each oxygen atom gains 2 electrons.
Now, let's review the options:
A. Each oxygen atom gained four electrons, and each aluminum atom lost three electrons.
B. Each oxygen atom gained three electrons, and each aluminum atom lost two electrons.
C. Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.
D. Each oxygen atom gained three electrons, and each aluminum atom lost four electrons.
The correct description is **C**: Each oxygen atom gained two electrons, and each aluminum atom lost three electrons.