Mixing of s and p orbitals can lead to some strange effects and
very unstable structures that
cannot be accurately described using Lewis structures. For each
part, name the (n = 2)
homonuclear diatomic (e.g. Li2, N2, Ne2, etc.) that each statement
represents.
(c) A molecule with eight electrons in bonding orbitals but has a bond order of zero.
in a molecular orbital theory, filling orbitals with increasing energy levels,so using that if total no of electrons <14
for a homogeneous diatomic molecules order is
1s < *1s < 2s < * 2s< 2py=2pz<2px<-------------
bond order = 1 /2 ( Nb - Na), where Nb = bonding no of electrons, Na =antibonding no of electrons
if it is 8 electrons ,bonding =4, antibonding =4
bond order = 1/2 ( 4 -4) = 0, it shows that bonding does not exist.
thank u
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