What makes balancing redox reactions different from balancing other reactions?

Answer 1

Balancing redox reactions is different from balancing other reactions because both the number of atoms and the amount of charge must be balanced.

Answer 2

Because when one thing is oxidized, another thing is reduced; hence, being complementary processes. Oxidation means the process of losing an electron. Reduction means gaining an electron. You can't just create and destroy electrons, so if an element loses one of its electrons, another element must therefore gain that electron. For example, consider the equation:

Cu(2+) + Mg --> Cu + Mg(2+)

Answer 3

A redox reaction consists of two half reactions which relate a compound or element's oxidation number before and after a reaction. These consist not only of elements and compounds but of electrons. Thus the difference is that redox reactions involve balancing elements AND electrons not just elements like other reactions.

Answer 4

Balancing redox reactions involves accounting for both the mass balance of atoms and the charge balance of ions. This typically requires adding electrons to ensure that the total charge is conserved. In contrast, balancing other reactions may only involve adjusting coefficients to balance the number of atoms on each side.