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Chemistry - oxidising agent

Can anyone help me with this question:

Explain, in terms of electron transfer, why bromine is the oxidant (oxidising agent) in this reaction
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?
Original post by DSKE
What’s the reaction/equation?

Br2(aq) + S2–(aq) → 2Br –(aq) + S(s)
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
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.
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 😅
(edited 3 years ago)
But hasn't the bromine lost electrons and the sulfur the one gaining electrons?
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.
But then how is Sulfur not gaining electrons. Sorry this is confusing me. I now understand the part about bromine, but not sulfur
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
oh ok. Thank you both for your help!

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