Question

What are the oxidation numbers in the compound $ KCl $ ?

Answer 1

Hint :We can define oxidation state as the degree of loss of an electron in a chemical compound. The oxidation state by an element in a compound can be calculated using the rules of oxidation numbers. Oxidation number is also known as an oxidation state. It is defined as the total number of electrons that an atom either gains or losses, in order to form chemical bonds with another atom.

Complete Step By Step Answer:
We will check the oxidation states in all the given molecules in in the compound $ KCl $
Oxidation state of $ Cl $ in can be determined as $ -1 $ for Potassium has an Oxidation state of $ +1. $ This is demonstrated by the following diagram of $ KCl $ compound and with equations proving the oxidation state of chlorine to be $ -1. $ The important rules for this problem are:
The oxidation number of a monatomic ion equals the charge of the ion.
The oxidation number of a Group $ 1 $ element in a compound is $ +1. $
The oxidation number of a Group $ 17 $ element in a binary compound is $ -1. $
The sum of the oxidation numbers of all the atoms in a neutral compound is $ 0. $
The compound can be rewritten as; $ K-Cl\text{ } $ thus for $ KCl, $ we have $ \therefore \left[ \left( K \right)\left( Cl \right) \right]=0\Rightarrow \left[ \left( +1 \right)\left( +Y \right) \right]=0 $ here it is equal to zero because it’s a stable molecule and stability factor equates with zero.
On further solving we get $ Y=-1. $ Oxidation number of chlorine is $ -1. $
Therefore, $ KCl $ is a neutral compound. It has no charge.

Note :
We must remember that the reduction is an opposite process of oxidation. If there is gain of electrons by a molecule, atom or ion then it is called as reduction it occurs when the oxidation state of the species is decreased. Reducing agent is one which is oxidized in a reaction. Reducing agent reduces the oxidizing agent.