Question

Calculate the oxidation number in \[N{a_2}[CO{(N{O_2})_6}]\] .
A) +3
B) +2
C) +1
D) 0

Answer 1

Hint: The oxidation state or oxidation number is defined as the total number of electrons that an atom can either gain or lose in order to form a chemical bond with another atom. By knowing the oxidation state of the other elements present, we can know the oxidation state of the central snippet of the emulsion.

Complete Step by Step Solution:
Oxidation number can also be defined as the degree of oxidation of an atom that is present in an emulsion.
The oxidation number can be positive, negative, or zero and is an integer. A coordination complex consists of a central atom or ion clicked to ligands by coordinated covalent bonds. The ligands and the central atom together form the coordination sphere.
In the central complex of \[CO\] :
The coordination sphere consists of 6 nitro ligands with a charge of -1 each. The coordination sphere carries a -3 charge as the coordination sphere is electrically neutral. The oxidation state of the sodium ligands is equal to +3
Let’s assume that the oxidation state of \[CO\] is equal to \[x\] .
The oxidation state of the nitro ligands is equal to -1, and sodium ligands is equal to +3
Therefore, after putting the values, we get
\[3( + 1) + x + 6( - 1) = 0\]
\[x = 6 - 3 = + 3\]
So, the oxidation state in \[N{a_2}[CO{(N{O_2})_6}]\] is equal to \[ + 3\] .
Hence, option A is the correct answer

Note: While calculating the oxidation state of an emulsion, we can move a step backward and multiply the number to coefficient with the oxidation state of the same atom that is present in the emulsion. For example, in the complex mentioned above, there are 4 \[CO\] ligands that are multiplied by its oxidation state of 0 while calculating the oxidation state of cobalt.