The methane (CH4) molecule is tetrahedral, with each of the hydrogen atoms connected by a single bond to the central C atom. What type of orbital hybridization exists around the C atom

The type of orbital hybridization around the C atom is sp3 hybridization.

Explanation:

The electron configuration of carbon is 1s² 2s² 2p². According to this configuration, carbon only has two semi-occupied orbitals that can form a covalent bond.

But a process called hybridization occurs, where the "s" and "p" orbitals at the (2s² 2p²) level combine and generate new orbitals. So this hybridization process where one "s" orbital is combined with three "p" orbitals forms four new sp³ hybrid orbitals (remember that there is 1 s orbital and 3 p orbitals for each layer or energy level). These four hybrid orbitals are half full, having only one electron and being capable of forming four covalent bonds.

So, the type of orbital hybridization around the C atom is sp³ hybridization.

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

c, liquids evaporate, creating a gas