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Hybridization of ##"HCl"##?
##"HCl"## has no orbital hybridization. Chlorine's ##3s## is too low in energy to interact with hydrogen's ##1s##, but chlorine's ##3p_z## can interact with hydrogen's ##1s## atomic orbital just fine.
A good general rule is that being less than about ##12## ##eV## apart in energy is required for orbitals to be close enough in energy.
The ##3s## and ##3p## orbitals of ##"Cl"## are apparently too far apart in energy to interact for orbital hybridization.
Based on these atomic orbital energies (Inorganic Chemistry, Miessler et al., Table 5.2):
##"E"_(1s)^"H" = -"13.61 eV"##
##"E"_(3s)^"Cl" = -"25.23 eV"##
##"E"_(3p)^"Cl" = -"13.67 eV"##
... here is the MO diagram for ##"HCl"##:
- ##1b_1## and ##1b_2## are nonbonding because the ##3p_x## and ##3p_y## atomic orbitals of chlorine weren't compatible with hydrogen's ##1s##, and the ##1a_1## is nonbonding because the ##3s## of chlorine is too low in energy to interact with hydrogen's ##1s##.
- ##2a_1## and ##3a_1## are the ##sigma_z## and ##sigma_z^"*"## bonding and antibonding MOs, respectively. They form because the ##1s## of hydrogen is compatible and close enough in energy to the ##3p_z## of chlorine.
It would contradict the Lewis structure to say that there is orbital hybridization in ##"HCl"##. Here's why:
- Nonbonding orbitals arise when two orbitals are NOT compatible and/or NOT close enough in energy.
- Although the ##3s## and ##3p## atomic orbitals are less than ##"12 eV"## apart, if they were to be able to interact, then given the closeness in energy to the ##1s## atomic orbital of ##"H"##, that ##1s## of ##"H"## would be able to interact with the ##3s## of ##"Cl"## too.
- The ##3s## and ##1s## are compatible (just know that they are compatible; the why is outside the scope of your level of education).
- So, if they were close enough in energy, they would interact, and then there would not be one nonbonding orbital from the ##3s## to hold one of the three lone pairs of electrons on ##"Cl"##, when we know that lone pair should be accounted for by the Lewis dot structure.
Therefore, there is no orbital hybridization in ##"HCl"##.