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Oxidation number of S in S2Cl2 , is...

Oxidation number of S in `S_2Cl_2` , is

A

`+1`

B

`+6`

C

0

D

`-1`

Text Solution

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The correct Answer is:
To find the oxidation number of sulfur (S) in the compound \( S_2Cl_2 \) (disulfur dichloride), we can follow these steps: ### Step 1: Identify the oxidation states of known elements In \( S_2Cl_2 \), we have two elements: sulfur (S) and chlorine (Cl). We know that chlorine typically has an oxidation state of -1. ### Step 2: Set up the equation for oxidation states Let the oxidation state of sulfur be \( x \). Since there are two sulfur atoms in the compound, the contribution from sulfur will be \( 2x \). For chlorine, since there are two chlorine atoms, the contribution will be \( 2 \times (-1) = -2 \). ### Step 3: Write the equation based on the overall charge The compound \( S_2Cl_2 \) is neutral, meaning the sum of the oxidation states must equal 0. Therefore, we can set up the equation: \[ 2x + (-2) = 0 \] ### Step 4: Solve for \( x \) Rearranging the equation gives: \[ 2x - 2 = 0 \] Adding 2 to both sides: \[ 2x = 2 \] Dividing both sides by 2: \[ x = 1 \] ### Conclusion The oxidation number of sulfur in \( S_2Cl_2 \) is \( +1 \).
To find the oxidation number of sulfur (S) in the compound \( S_2Cl_2 \) (disulfur dichloride), we can follow these steps: ### Step 1: Identify the oxidation states of known elements In \( S_2Cl_2 \), we have two elements: sulfur (S) and chlorine (Cl). We know that chlorine typically has an oxidation state of -1. ### Step 2: Set up the equation for oxidation states Let the oxidation state of sulfur be \( x \). Since there are two sulfur atoms in the compound, the contribution from sulfur will be \( 2x \). For chlorine, since there are two chlorine atoms, the contribution will be \( 2 \times (-1) = -2 \). ...
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