oxidation-reduction question...?

Question

A colorless solution of NaCl is added to an orange solution containing Br_2 (assume aq solutions).

What's the balanced net ionic equation for this? (no spectator ions)... assuming the reaction occurs. and what's the oxidizing agent? and how do you know it's the oxidizing agent? so confused by this concept...

Thanks so much for the help!!

Answer 1

There is no reaction.

Cl is more electronegative than Br and thus Br2 cannot steal the electrons from Cl- in order for the redox reaction to occur.

Oxidizing agent is the reactant that will oxidize something else. In order to do that it will take electrons from the other compound so itself is reduced.

Answer 2

Net ionic equation

2Cl- + Br2 --> 2 Br- + Cl2.

The oxidizing agent is Br2 because it oxidizes Cl-. You know the latter gets oxidized because its oxidation number increases from -1 (in chloride) to 0 (in chlorine). For the same reason, Cl- is the reducing agent because it reduces Br2 (oxidation number 0) to Br- (oxidation number -1)

Answer 3

No no longer all reaction are redox. reaction between metals and non-metals are merely redox reaction Redox skill help and oxidation, it truly is the benefit or lack of electron forming and ionic bond. Oxidation=lack of electrons help= benefit of electrons e.g.a rection between a nonmetal and metallic is time-honored as redox reaction. Metals are oxidized Non-metasl are decreased there is replace in oxidation state. although in non-metals there's a covalent bonding, electrons are not any more received or lost yet quite is shared. this isn't a redox reaction. submit to in ideas : Redox ought to contain metals. Metals are resposible for any redox reaction