the difference between ionic reaction and redox reaction
Below is a summary to explain the difference between a redox reaction and an ionic reaction. This will also help you understand the part that oxidation and reduction take in chemistry.
Ionic reaction - a chemical reaction where oppositely charged atoms (ions) are attracted to each other.
Key ionic = attracted atoms.
An ionic reaction can occur without first having one atom transfer an electron to another (an ionic reaction can occur without redox).
When two ionic compounds dissolve in water and are mixed a new ionic compound can form out of solution. This can occur without any of them changing their charge. There has been no transfer of electrons. This is a non-redox reaction.
Redox reaction - A transfer of an electron between atoms has occurred.
Key redox = transfer of an electron.
A redox reaction means a transfer of electrons has occurred between one atom and another. A bond mostly then occurs because one atom is +ve and the other is -ve and they attract each other. This is a very strong bond. Sometimes bonds do not occur, the electron is simply transferred.
A classic redox reaction occurs between metals and non-metals where an electron is transferred from the metal to the non-metal forming +ve and -ve ions they then bond together with a very strong electrostatic attracting force called ionic bonding.
A redox reaction is one in which electrons are transferred between substances. One substance loses electrons (oxidation) and another gains electrons (reduction).
Reference here to the acronym OILRIG - Oxidation Is Loss Reduction Is Gain.
Example
Iron + copper sulphate → Iron sulphate + copper
Fe + CuSO4 → FeSO4 + Cu
Iron is oxidised (loses electrons) Fe to Fe²+
Copper is reduced (gain electrons) Cu²+ to Cu
