Question

Justify the position of hydrogen in the periodic table on the basis of its electronic configuration.

Answer 1

Hint:
Hydrogen is the lightest element which is the first member of the periodic table. As hydrogen has an unique electronic configuration of \[1{s^1}\] it shows unique properties making its chemistry quite interesting.

Step-by-step explanation:
Step 1:
Hydrogen possesses unique properties as it has only one electron in the valence shell.
As it has one electron in the valence shell so it resembles the alkali metals in various ways:
They have similar valence shell electronic configuration.
They form mono-positive cations.
They exhibit electropositive character.
They have similar oxidation states.
They have a strong affinity for non-metals.
Like alkali metals, hydrogen is also a very good reducing agent.
So, it should be placed with alkali metals in Group 1.
Step 2:
Hydrogen, like halogen the group 17 elements has only one electron less to attain stable inert gas configuration and shows similarity in characters in the following ways:
They are diatomic in nature.
They form mono-negative anions.
They have a comparable ionisation energy.
They are non-metallic in nature.
They have similar oxidation states.
They combine similarly with metals and non-metals.
So, Hydrogen can be placed with halogens in Group 17.

Hence, the position of hydrogen is debatable in the periodic table.

Note: Hydrogen can form a \[{H^ + }\] ion by releasing an electron and thereby its oxidation state matches with the alkali metals and it can also form \[{H^ - }\] ion by accepting an electron and thereby its oxidation state matches with the halogens.