sweetescobar
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Can anyone help me with this question:

Explain, in terms of electron transfer, why bromine is the oxidant (oxidising agent) in this reaction
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DSKE
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(Original post by sweetescobar)
Can anyone help me with this question:

Explain, in terms of electron transfer, why bromine is the oxidant (oxidising agent) in this reaction
What’s the reaction/equation?
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sweetescobar
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(Original post by DSKE)
What’s the reaction/equation?
Br2(aq) + S2–(aq) → 2Br –(aq) + S(s)
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DSKE
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(Original post by sweetescobar)
Br2(aq) + S2–(aq) → 2Br –(aq) + S(s)
Okay so the oxidation state of bromine went from 0 to -2 whereas the oxidation state of sulfur went from -2 to 0. Therefore, bromine is the oxidising agent because it’s the one being reduced and accepts electrons
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charco
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(Original post by DSKE)
Okay so the oxidation state of bromine went from 0 to -2 whereas the oxidation state of sulfur went from -2 to 0. Therefore, bromine is the oxidising agent because it’s the one being reduced and accepts electrons
Not quite correct.

Each bromine atom changed from 0 to -1.
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DSKE
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(Original post by charco)
Not quite correct.

Each bromine atom changed from 0 to -1.
Oh yeahhh true, sorry lol - it’s early in the morning 😅
Last edited by DSKE; 1 month ago
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sweetescobar
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But hasn't the bromine lost electrons and the sulfur the one gaining electrons?
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(Original post by sweetescobar)
But hasn't the bromine lost electrons and the sulfur the one gaining electrons?
No, oxidation numbers of elemental atoms are always zero.

Bromide ions are in the -1 oxidation state.

0 to -1 is gain of one electron.
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sweetescobar
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But then how is Sulfur not gaining electrons. Sorry this is confusing me. I now understand the part about bromine, but not sulfur
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DSKE
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(Original post by sweetescobar)
But then how is Sulfur not gaining electrons. Sorry this is confusing me. I now understand the part about bromine, but not sulfur
Because sulfur went from -2 to 0 which means it’s being oxidised, and oxidation is loss of electrons
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sweetescobar
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oh ok. Thank you both for your help!
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