Answered

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Explain why or why not.

5. Think Critically: In the reaction [tex]2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl}[/tex], which atom is reduced and which atom is oxidized?

Sagot :

GinnyAnswer
Certainly! Let's analyze the reaction step-by-step to determine which atom is oxidized and which is reduced in the given chemical reaction:

[tex]\[ 2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl} \][/tex]

### Step 1: Identify the Oxidation States of Reactants and Products

- Sodium (Na):
- In its elemental form, sodium (Na) has an oxidation state of 0.

- Chlorine (Cl2):
- In its elemental molecular form, chlorine (Cl2) has an oxidation state of 0.

- Sodium in NaCl:
- In sodium chloride (NaCl), sodium (Na) typically has an oxidation state of +1.

- Chlorine in NaCl:
- In sodium chloride (NaCl), chlorine (Cl) typically has an oxidation state of -1.

### Step 2: Determine Changes in Oxidation States

- Sodium (Na) changes from an oxidation state of 0 to +1.

- Chlorine (Cl2) changes from an oxidation state of 0 to -1.

### Step 3: Identify Reduction and Oxidation

- Oxidation involves the loss of electrons and an increase in oxidation state.
- Here, sodium (Na) goes from 0 to +1, indicating that it loses one electron.
- Therefore, sodium (Na) is oxidized.

- Reduction involves the gain of electrons and a decrease in oxidation state.
- Here, chlorine (Cl2) goes from 0 to -1, indicating that it gains one electron.
- Therefore, chlorine (Cl2) is reduced.

### Step 4: Conclusion

In the reaction [tex]\(2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl}\)[/tex]:

- The atom oxidized is Sodium (Na).
- The atom reduced is Chlorine (Cl2).

This is because sodium loses electrons and is oxidized, whereas chlorine gains electrons and is reduced.
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