In case of oxygen family (group -16) (a) The tendency for...

In case of oxygen family (group -16) (a) The tendency for catenation decreases markedly as we go down the group (b) Maximum coordination of oxygen is four due to lack of d-orbital but that of other elements is six due to presence of d-orbitals (c) The tendency to form multiple bonds with $\mathrm{C}, \mathrm{N}$ and $O$ decreases as going down the group from $\mathrm{S}$ to $\mathrm{Te}$. (d) All are correct

In case of oxygen family (group -16)
(a) The tendency for catenation decreases markedly as we go down the group
(b) Maximum coordination of oxygen is four due to lack of d-orbital but that of other elements is six due to presence of d-orbitals
(c) The tendency to form multiple bonds with $\mathrm{C}, \mathrm{N}$ and $O$ decreases as going down the group from $\mathrm{S}$ to $\mathrm{Te}$.
(d) All are correct

Key Concepts

Multiple Bond Formation

Multiple bonding involves the sharing of more than one pair of electrons between two atoms, such as double or triple bonds. In the oxygen family, the ability to form strong multiple bonds with elements like carbon and nitrogen is most pronounced in the lighter congeners. As one goes down the group from sulfur to tellurium, the tendency to form these multiple bonds decreases because the larger atomic size and the involvement of d-orbitals weaken the overlap necessary for the formation of robust ? bonds.

Catenation

Catenation refers to the ability of atoms of the same element to bond with each other to form chains or rings. In the oxygen family, this ability decreases as one moves down the group, primarily due to the increasing atomic size and the corresponding decrease in bond strength between the atoms. This makes the formation of extensive networks or chains less favorable for the heavier elements compared to oxygen or sulfur.

Coordination Number and Role of d-Orbitals

The coordination number of an element is often related to the number of available orbitals that can participate in bonding. Due to the absence of low-lying d-orbitals in oxygen, its coordination number is limited (typically maxing out at four). In contrast, heavier chalcogens, like sulfur, selenium, and tellurium, have accessible d-orbitals which can accommodate additional bonding, thereby allowing these atoms to achieve higher coordination numbers, such as six.

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