Question

How does the oxidation state of the element differ as compared to its place in the periodic table?

Answer 1

Oxidation state:

• The oxidation number is also known as the oxidation state, is the total number of electrons that an atom either gains or losses in order to form a chemical bond with another atom.
• The more electronegative element in a substance will be having a negative oxidation state and the less electronegative element will be having a positive oxidation state.

s-block oxidation state:

• The general electronic configuration of s-block elements is ${\mathrm{ns}}^{1-2}$.
• s-block contains 2 groups, that is group 1 and group 2.
• The general electronic configuration of group 1 is ${\mathrm{ns}}^1$ and the oxidation state is $+1$.
• The general electronic configuration of group 2 is ${\mathrm{ns}}^2$ and the oxidation state is $+2$.
• Therefore, the number of electrons that an atom either gains or loses is $+1$ and $+2$.

p-block oxidation state:

• The general electronic configuration of p-block elements is ${\mathrm{ns}}^2{\mathrm{np}}^{1-6}$.
• p-block contains 6 groups, that is group 13 to group 18.
• The general electronic configuration of group 13 is ${\mathrm{ns}}^2{\mathrm{np}}^1$ and the oxidation state is $+3$.
• The general electronic configuration of group 14 is ${\mathrm{ns}}^2{\mathrm{np}}^2$ and the oxidation states will be $+4,+2,-2,$ and $-4$ .
• The general electronic configuration of group 15 is ${\mathrm{ns}}^2{\mathrm{np}}^3$ and the oxidation state will be $+5,+3$ and $-3$.
• The general electronic configuration of group 16 is ${\mathrm{ns}}^2{\mathrm{np}}^4$ and the oxidation state will be $+4,+2$ and $-2$.
• The general electronic configuration of group 17 is ${\mathrm{ns}}^2{\mathrm{np}}^5$ and the oxidation state will be $+5,+3,+1$ and $-1$.
• The general electronic configuration of group 18 is ${\mathrm{ns}}^2{\mathrm{np}}^6$ and the oxidation state will be zero since this is the noble gas family and they do not want to lose or gain electrons.

d-block oxidation state:

• The general electronic configuration of d-block elements is $(\mathrm{n}-1){\mathrm{d}}^{1-10}{\mathrm{ns}}^{0-2}$
• d-block contains 10 groups, that is group 3 to group 12.
• The transition metals are having variable oxidation states, since their valence electrons are in two different sets of orbitals, that is $(\mathrm{n}-1)\mathrm{d}$ and $\mathrm{ns}$.
• The energy difference between these orbitals is very less and therefore, these energy levels can be used for bond formation.
• For example, Vanadium ( $\mathrm{V}$) shows $+2,+3,+4$ and $+5$ oxidation states.

f-block oxidation state:

• The general electronic configuration of f-block elements is $(\mathrm{n}-2){\mathrm{f}}^{0-14}(\mathrm{n}-1){\mathrm{d}}^{0-2}{\mathrm{ns}}^2$.
• The f-block elements are in two rows at the bottom of the periodic table and are known as inner transition metals.
• f-block elements show oxidation $+3$ state, and some elements also show $+4,+5,+6,$and $+7$ oxidation states.