Question

Which is incorrect about oxidation? (1) deelectronation (2) inereased electron density (3) increase in oxidation state (4) loss of hydrogen

Short answer

(2) increased electron density

Step-by-step solution

Define Oxidation

Oxidation is a chemical process where an atom, ion, or molecule loses electrons. This process is often characterized by an increase in the oxidation state of the element.

Identify Terms

Each option should be examined to see if it accurately describes aspects of oxidation. The terms are: deelectronation, increased electron density, increase in oxidation state, and loss of hydrogen.

Analyze Each Option

Option (1), deelectronation (loss of electrons), is a correct description of oxidation. Option (2), increased electron density, suggests gain of electrons which is actually reduction, not oxidation. Option (3), increase in oxidation state, is also a characteristic of oxidation. Option (4), loss of hydrogen, is another way to describe oxidation.

Conclusion

The option that is incorrect about oxidation is increased electron density because this describes reduction.

Key concepts

Oxidation State

Oxidation state, also known as oxidation number, is a concept used to keep track of electrons in chemical reactions. It helps in determining whether an atom is being oxidized or reduced. When an atom loses electrons, its oxidation state increases. For example, if a sodium atom loses one electron, its oxidation state goes from 0 to +1.
In a neutral molecule, the sum of the oxidation states of all atoms must be zero. In an ion, the sum must be equal to the charge of the ion. This concept is crucial for balancing redox reactions and understanding electron transfer in a chemical reaction.

Electron Transfer

Electron transfer is the movement of electrons from one atom or molecule to another. This is a fundamental part of redox (reduction-oxidation) reactions.

In oxidation, an atom or molecule loses electrons, transferring them to another species. For example, in a simple reaction of magnesium and oxygen, magnesium loses electrons and oxygen gains them. The transfer can be direct, or it might involve a series of intermediate carriers, especially in biological systems.
Understanding electron transfer is essential for grasping how batteries work, how plants photosynthesize, and how various other chemical reactions proceed.

Deelectronation

Deelectronation is a term referring to the loss of electrons by an atom, ion, or molecule. This is essentially another way to describe oxidation. For instance, when iron rusts, it loses electrons and forms iron oxide.
Deelectronation plays a crucial role in many industrial processes, including battery operation, metal refining, and even biological systems like respiration and photosynthesis. It's vital to note that the electrons lost by one substance are typically gained by another in a corresponding reduction process.

Chemical Reaction

A chemical reaction involves the breaking and forming of bonds between atoms. In redox reactions, which include oxidation and reduction processes, electrons are transferred between reactants.
These reactions are everywhere: in the rusting of metal, combustion of fuels, and in our very cells where energy production happens. The correct understanding of this dynamic is crucial for numerous applications, from energy storage technologies to metabolic engineering.
Breaking down a chemical reaction into steps, such as identifying changes in oxidation states and tracking electron transfer, helps in understanding the overall transformation occurring during the reaction.