Question

What is the difference between:

Modern explanation and Arrhenius explanation for the theory of electrolysis.

Answer 1

Arrhenius considered that water ionizes electrolytes but Modern theory explained that electrolytes are ionic even in solid state and their ions are held by strong electrostatic forces which make them immobile. Water renders these ions mobility by breaking the electrostatic forces.

Answer 2

	Arrhenius Theory of Ionisation	Modem Theory of Ionisation
(1)	When an electrolyte dissolves in water, it dissociates into (+ve ions) and (−ve ions), known as cations and anions, respectively.	The electrolytes can be purely ionic, such as NaCl, KCI, or covalent compounds with polar properties, such as HCl, HBr, etc.
(2)	All ions have an electric charge and are responsible for the current flow through the solution.	Ionic compounds are made up of ions that are bound together by strong attractive forces. When such a substance is dissolved in water or melted, the force of attraction between the ions decreases, and the ions begin to move freely.
(3)	The conductivity of the electrolyte is determined by the concentration of ions in the solution.	In solution, ions are surrounded by solvent molecules. Hydrated ions are those formed when water is utilised as a solvent.
(4)	The number of (+ve) charges equals the number of (−ve) charges in the solution, indicating that it is in electrolytic equilibrium. The equilibrium is created between the unionised molecules and the ions generated.	Polar covalent compounds, such as hydrogen chloride, create ions in solution. Ions are formed by the attraction of polar chemicals and water molecules, which have opposite charges.
(5)	Non-electrolytes lack ionisation and so contain only molecules in solution. Examples include sugar solution and benzene.	A strong electrolyte ionises almost completely even at moderate concentrations.
(6)	The degree of dissociation is the amount to which an electrolyte dissociates or breaks into ions.	Diluting the solution decreases the inter-ionic forces that hold the ions, leading to increased ionisation. Because of the increasing quantity of ions, the solution's electrical conductivity increases.