What is the first step to balance a redox equation using the half-reaction method?
Redox reactions are conceived to occur on the basis of electron transfer, which requires the assignment of formal oxidation states. The oxidation state is the charge left on the central atom when all the bonding pairs of electrons are distributed on the basis of a few predetermined rules.
And thus for, say
And once you have assigned the oxidation numbers, the difference between such numbers is the number of electrons transferred during the redox equation.
Are charge and mass balanced here?
And for every reduction, there is a corresponding oxidation:
And in the overall redox reaction, we cross-multiply the individual redox equations to eliminate the electrons:
.........to give finally,
Which is, as far as I know, balanced with respect to mass and charge, as indeed it must be if we purport to model a chemical process.
What we would see in this reaction, if we mixed stoichiometric reagents, was the disappearance of the deep purple colour of potassium permanganate to give almost colourless
What are the oxidation numbers of the central atom in