Question

why overlapping is not applicable on polyatomic molecules explain with the example of methane​

Answer 1

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Simply beginning with the original atomic orbitals and ground electronic states of the atom cannot explain the observed geometry for molecules as simple as methane, CH4. Since 2 of the 2p orbitals of C are half-filled, two of the H 1s orbitals can overlap with these, (one for each half filled 2p orbital.

Answer 2

Answer:

Molecular orbital diagram

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A molecular orbital diagram, or MO diagram, is a qualitative descriptive tool explaining chemical bonding in molecules in terms of molecular orbital theory in general and the linear combination of atomic orbitals (LCAO) method in particular.[1][2][3] A fundamental principle of these theories is that as atoms bond to form molecules, a certain number of atomic orbitals combine to form the same number of molecular orbitals, although the electrons involved may be redistributed among the orbitals. This tool is very well suited for simple diatomic molecules such as dihydrogen, dioxygen, and carbon monoxide but becomes more complex when discussing even comparatively simple polyatomic molecules, such as methane. MO diagrams can explain why some molecules exist and others do not. They can also predict bond strength, as well as the electronic transitions that can take place.