For the following reaction, identify the element that was oxidized, the element that was reduced, and the reducing agent. Give an explanation for each answer.

SnCl2 + PbCl4 yields SnCl4 + PbCl2

Question

For the following reaction, identify the element that was oxidized, the element that was reduced, and the reducing agent. Give an explanation for each answer. 

SnCl2 + PbCl4 yields SnCl4 + PbCl2

anonymous · Answer

SnCl is the reducing agent because it reduced PbCl right? So then SnCl is the one that got oxidized, correct?

abmon98 · Answer

Cl oxidation state is usually -1 except in compound of F or O(more electronegative elements). in this case Cl is -1
-1*2 (because there are 2 atoms of Cl present in Sncl2)=-2
The sum of the oxidation states of all the atoms or ions in a neutral compound is zero therefore Sn has to be +2
Pb is +4 on the reactant side as the reaction proceeds and products are formed. Sn is oxidized from +2 to +4 and Pb is reduced from +4 to +2

anonymous · Answer

And the reducing agent is Pb? or Cl?

anonymous · Answer

@Abmon98

abmon98 · Answer

Reducing agent reduced another substance and is oxidised so the reducing agent here is SnCl2

anonymous · Answer

Oh okay, thank you for explaining!

abmon98 · Answer

your welcome :)