In the reaction: $3Cl_{2}+6NaOH\rightarrow NaClO_{3}+5NaCl+3H_{2}O$ the element which loses as well as gains electrons is :

Q: In the reaction: $3Cl_{2}+6NaOH\rightarrow NaClO_{3}+5NaCl+3H_{2}O$ the element which loses as well as gains electrons is :

In the given chemical reaction: \[ 3Cl_{2} + 6NaOH \rightarrow NaClO_{3} + 5NaCl + 3H_{2}O \] we need to identify the element that both loses and gains electrons. According to the correct answer, Option 2 (Cl) is the element that undergoes both oxidation and reduction. Let's explore why this is the case: ### Explanation for Option 2 (Cl): 1. **Oxidation and Reduction of Chlorine:** - In the reaction, chlorine ($Cl_2$) is present in its elemental form with an oxidation state of 0. - Chlorine is converted into two different products: sodium chloride ($NaCl$) and sodium chlorate ($NaClO_3$). - In sodium chloride ($NaCl$), chlorine has an oxidation state of -1. This indicates that chlorine has gained electrons (reduction). - In sodium chlorate ($NaClO_3$), chlorine has an oxidation state of +5. This indicates that chlorine has lost electrons (oxidation). - Therefore, chlorine undergoes both oxidation and reduction in this reaction, a process known as disproportionation. ### Explanation for why other options are incorrect: 1. **Option 1 (Na):** - Sodium ($Na$) in sodium hydroxide ($NaOH$) and in the products ($NaCl$ and $NaClO_3$) remains in the +1 oxidation state throughout the reaction. - There is no change in the oxidation state of sodium, meaning it neither gains nor loses electrons. 2. **Option 3 (O):** - Oxygen ($O$) in sodium hydroxide ($NaOH$) and in the products ($NaClO_3$ and $H_2O$) remains in the -2 oxidation state. - There is no change in the oxidation state of oxygen, meaning it neither gains nor loses electrons. 3. **Option 4 (H):** - Hydrogen ($H$) in sodium hydroxide ($NaOH$) and in water ($H_2O$) remains in the +1 oxidation state. - There is no change in the oxidation state of hydrogen, meaning it neither gains nor loses electrons. In conclusion, chlorine (Cl) is the only element in this reaction that undergoes both oxidation and reduction, making Option 2 the correct answer.

Question

Accepted Answer

In the given chemical reaction:

$$ 3Cl_{2} + 6NaOH \rightarrow NaClO_{3} + 5NaCl + 3H_{2}O $$

we need to identify the element that both loses and gains electrons. According to the correct answer, Option 2 (Cl) is the element that undergoes both oxidation and reduction. Let's explore why this is the case:

### Explanation for Option 2 (Cl):

1. **Oxidation and Reduction of Chlorine:**
   - In the reaction, chlorine ($Cl_2$) is present in its elemental form with an oxidation state of 0.
   - Chlorine is converted into two different products: sodium chloride ($NaCl$) and sodium chlorate ($NaClO_3$).
   - In sodium chloride ($NaCl$), chlorine has an oxidation state of -1. This indicates that chlorine has gained electrons (reduction).
   - In sodium chlorate ($NaClO_3$), chlorine has an oxidation state of +5. This indicates that chlorine has lost electrons (oxidation).
   - Therefore, chlorine undergoes both oxidation and reduction in this reaction, a process known as disproportionation.

### Explanation for why other options are incorrect:

1. **Option 1 (Na):**
   - Sodium ($Na$) in sodium hydroxide ($NaOH$) and in the products ($NaCl$ and $NaClO_3$) remains in the +1 oxidation state throughout the reaction.
   - There is no change in the oxidation state of sodium, meaning it neither gains nor loses electrons.

2. **Option 3 (O):**
   - Oxygen ($O$) in sodium hydroxide ($NaOH$) and in the products ($NaClO_3$ and $H_2O$) remains in the -2 oxidation state.
   - There is no change in the oxidation state of oxygen, meaning it neither gains nor loses electrons.

3. **Option 4 (H):**
   - Hydrogen ($H$) in sodium hydroxide ($NaOH$) and in water ($H_2O$) remains in the +1 oxidation state.
   - There is no change in the oxidation state of hydrogen, meaning it neither gains nor loses electrons.

In conclusion, chlorine (Cl) is the only element in this reaction that undergoes both oxidation and reduction, making Option 2 the correct answer.