Question

Why $C{H_4}$ cannot adopt square planar geometry?

Answer 1

Any central atom having four atoms attached to it, can arrange in two shapes, square planar and tetrahedral on the basis of repulsion between those atoms, or lone pair on the central atom and the atom. Methane is a molecule with a carbon central atom and four hydrogen atoms attached to it.

Complete step-by-step answer:
Carbon is an element that belongs to group 13 of periodic table and has atomic number 6.
The Ground state electronic configuration of carbon is $1{s^2}2{s^2}2p_x^12p_y^1$.
Excited state electronic configuration of carbon is $1{s^2}2{s^1}2p_x^12p_y^12p_z^1$.
As four vacant orbitals can occupy four hydrogen atoms and form $s{p^3}$ hybridised molecule,
commonly known as methane. $s{p^3}$ hybridised molecules are tetrahedral in geometry and so is methane.
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For square planar geometry, the hybridisation has to be $ds{p^2}$. But in methane, there is no involvement of d-orbitals as it has less electrons. So, it cannot have square planar geometry.
As per valence shell electron pair repulsion theory (VSEPR), we can't determine the structure of any molecule with the help of its hybridisation.
Therefore, we say that $C{H_4}$ cannot adopt square planar geometry.

Note: Methane molecule is tetrahedral with ${109.5^ \circ }$ bond angle (H-C-H), although the $2p$ orbitals are all at $90^0$ to each other and four equal bond lengths with no dipole moment because the electronegativity difference between carbon and hydrogen is very less.