[student8607]

Does it matter what state the reactants are in for the redox reaction to occur?
I know for precipitation reactions, you need to have both reactants in (aq).

How about having 2 atoms instead of 3?

EX:
Cl2(g) + 2 NaBr(aq) --> Br2(aq) + 2 NaCl(aq)
Cl2=0, Na=+1, Br=-1 --> Br=0, Na=+1, Cl=-1…Br is reducing agent --> oxidized, Cl is oxidizing agent --> reduced

[Borek]

Please elaborate, I have no idea what you are asking about.

[student8607]

Does it matter what chemical state (solid, liquid, gas, aqueous) that the reactants are in?

In class, we had an example similar to this:
EX:Cl2(s) + 2 NaBr(g) --> Br2(aq) + 2 NaCl(aq)
Cl2=0, Na=+1, Br=-1 --> Br=0, Na=+1, Cl=-1…Br is reducing agent --> oxidized, Cl is oxidizing agent --> reduced

Would there still be a redox reactions if we had this:
Cl2(g) + 2 NaBr(aq) --> Br2(aq) + 2 NaCl(aq)
Cl2=0, Na=+1, Br=-1 --> Br=0, Na=+1, Cl=-1…Br is reducing agent --> oxidized, Cl is oxidizing agent --> reduced


In precipitate reactions, it has to be
A(aq) + B(aq) ... they both have to be in aqueous form

Is that true for redox reactions? Or does there just need to be an electron transfer?