Justify the place

The elements of group 16 are collectively called chalcogens.

[i]. Elements of group 16 have six valence electrons each. The general electronic configuration of these elements is ns² np⁴, where n varies from 2 to 6.

[ii]. Oxidation state: As these elements have six valence electrons [ns²np⁴], they should display an oxidation state of -2. However, only oxygen predominantly shows the oxidation state of -2 owing to its high Electronegativity. It also exhibits the oxidation state of -1 [H₂O₂], zero [O₂], and +2 [OF₂]. However, the stability of the -2 oxidation state decreases on moving down a group due to a decrease in the Electronegativity of the elements. The heavier elements of the group show an oxidation state of +2, +4, and +6 due to the availability of d-orbitals.

[iii]. Formation of hydrides: These elements form hydrides of formula H₂E, where E = O, S, Se, Te, PO. Oxygen and sulphur also form hydrides of type H₂E_2. These hydrides are quite volatile in nature.