Question:
What are the oxidation numbers on S atoms in \(S_4O_6^{2-}\)?
What are the oxidation numbers on S atoms in \(S_4O_6^{2-}\)?
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In sulphur oxyanions, sulphur atoms bonded directly to oxygen usually have positive oxidation states, while sulphur atoms connected only through \(S-S\) bonds often have oxidation number zero.
Updated On: Jun 22, 2026
- \(6,\,-1,\,-1,\,6\)
- \(5,\,0,\,0,\,5\)
- \(2.5,\,2.5,\,2.5,\,2.5\)
- \(7,\,-2,\,-2,\,7\)
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The Correct Option is B
Solution and Explanation
Step 1: Write the structure of tetrathionate ion.
The ion \[ S_4O_6^{2-} \] contains a chain of four sulphur atoms.
Its structure can be represented as \[ O_3S-S-S-SO_3^{2-} \] The two terminal sulphur atoms are bonded to oxygen atoms, while the two middle sulphur atoms are connected only with sulphur atoms.
Step 2: Find oxidation state of terminal sulphur atoms.
Each terminal sulphur atom is attached to three oxygen atoms.
Since oxygen has oxidation number \[ -2 \] the total contribution from oxygen atoms attached to one terminal sulphur is \[ 3\times (-2)=-6 \] The sulphur atom balances this and effectively has oxidation state \[ +5 \] Thus, the two terminal sulphur atoms have oxidation number \[ +5 \]
Step 3: Find oxidation state of middle sulphur atoms.
The two middle sulphur atoms are connected only through \[ S-S \] bonds.
Since bonds between identical atoms contribute zero to oxidation number, each middle sulphur atom has oxidation number \[ 0 \]
Step 4: Verify the total charge.
Adding all oxidation numbers: \[ (+5)+0+0+(+5)=+10 \] For six oxygen atoms: \[ 6\times (-2)=-12 \] Total charge: \[ +10-12=-2 \] which matches the charge on the ion.
Step 5: Final conclusion.
Therefore, the oxidation numbers on the sulphur atoms are \[ \boxed{5,\,0,\,0,\,5} \]
The ion \[ S_4O_6^{2-} \] contains a chain of four sulphur atoms.
Its structure can be represented as \[ O_3S-S-S-SO_3^{2-} \] The two terminal sulphur atoms are bonded to oxygen atoms, while the two middle sulphur atoms are connected only with sulphur atoms.
Step 2: Find oxidation state of terminal sulphur atoms.
Each terminal sulphur atom is attached to three oxygen atoms.
Since oxygen has oxidation number \[ -2 \] the total contribution from oxygen atoms attached to one terminal sulphur is \[ 3\times (-2)=-6 \] The sulphur atom balances this and effectively has oxidation state \[ +5 \] Thus, the two terminal sulphur atoms have oxidation number \[ +5 \]
Step 3: Find oxidation state of middle sulphur atoms.
The two middle sulphur atoms are connected only through \[ S-S \] bonds.
Since bonds between identical atoms contribute zero to oxidation number, each middle sulphur atom has oxidation number \[ 0 \]
Step 4: Verify the total charge.
Adding all oxidation numbers: \[ (+5)+0+0+(+5)=+10 \] For six oxygen atoms: \[ 6\times (-2)=-12 \] Total charge: \[ +10-12=-2 \] which matches the charge on the ion.
Step 5: Final conclusion.
Therefore, the oxidation numbers on the sulphur atoms are \[ \boxed{5,\,0,\,0,\,5} \]
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