Electrochemical processes are written with the oxidation half-reaction on the left and the reduction reaction on the right; whereas, oxidation-reduction reactions are represented by equations that group the reaction participants into reactants and products.

a. true
b. false

B) FALSE.

Explanation:

First off, its important to understand the following concepts;

A half reaction is either the oxidation or reduction reaction component of a redox (Oxidation - Reduction) reaction. A half reaction is obtained by considering the change in oxidation states of individual substances involved in the redox reaction.

Often, the concept of half-reactions is used to describe what occurs in an electrochemical cell, such as a Galvanic cell battery. Half-reactions can be written to describe both the metal undergoing oxidation (known as the anode) and the metal undergoing reduction (known as the cathode).

Half equations simply much just breaks the reaction into oxidation and reduction steps (irrespective of the order, whether left or right).

An example of half equation is given below;

Mg → Mg2+ + 2e− (Oxidation)

Cu2+ + 2e− → Cu (Reduction)

The answer is false because; oxidation-reduction reactions are NOT represented by equations that group the reaction participants into reactants and products. Rather they are

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.