Orbitals that play a role in bonding to C atoms are sp³ hybridization orbitals, while O atoms, the orbitals used for binding are 2p orbitals
and the H atom, the orbitals used are 1s
<h3>Further explanation </h3>Hybridization is a term used in the formation of chemical bonds or the determination of the geometric shape of a molecule. Hybridization is generally used to describe molecules that have C, N and O atoms
In the formation of bonds between 2 atoms, the valence electrons of the two atoms will play a role in the filling of empty orbitals that are shared and filled with electrons from both atoms.
Hybridization itself is merging of orbitals that have different energy levels so that it is expected to explain the resulting geometric shape according to the length, angle or bond energy
In the compound CH₃OH (methanol) which is one of the alcohols there are 3 atoms in it namely C, H, and O
The electron configurations of each of these atoms are:
C: 1s² 2s² 2p2²
H: 1s1¹
O: 1s² 2s² 2p⁴
In an atom, C hybridization occurs where the electrons in the 2s orbitals are excited into the 2p orbitals to form sp³ hybridization orbitals so that 4 single electrons can bind to other atoms
Whereas on the O atom there are 2 single electrons in the 2p orbitals so that they can bind with 2 other electron atoms to form bonds
Whereas the H atom, there is 1 single electron in 1s orbitals that can bind to 1 electron from another atom
<h3>Learn more </h3>
statement about electrons and atomic orbitals
the formation of a bond.
the hybridization and bonding scheme for xef4
Keywords: the electron configuration, orbitals, hybridization
