Question

why S and p block elements do not form carbonyl compound ​

Answer 1

Answer:

Complexes of Ca, Sr and Ba adopt a transition metal-like 18-electron configuration, rather than the octet more usually found in main group compounds

The heavier group 2 elements appear to involve their empty d-orbitals more in bonding than previously suspected. Calcium, strontium and barium can all form 18-electron octacarbonyl complexes with carbon monoxide, more akin to those formed by transition metals than other main group elements. The new results challenge previous notions of coordination chemistry and expand the limits of a widely accepted rule.

Elements are classified into main group elements, which include the s- and p-blocks of the periodic table, transition metals (d-block) and lanthanides and actinides (f-block). As main group elements, Ca, Sr and Ba normally form bonds using their s and p valence orbitals, following the ‘octet rule’, which states that atoms tend to combine in such a way that they have eight electrons in their valence shell. Transition metals bring in a further five d orbitals that must be filled to achieve such a stable configuration, resulting in a similar 18-electron rule for these elements.

Explanation:

Answer 2

even elements of carbon family such as silicon , lead does not form covalent bonds with oxygen because catenation property which is excessively present in carbon is not in other compounds and speaking about S block elements they try to form ionic compounds more often.... because of their low ionization enthalpy