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.
