A few years ago, an organic chemistry teaching lab professor told me one of the reasons dichloromethane is unsurprisingly unreactive is because of the symmetry ( degeneracy ) of the C-Cl antibonding orbitals ( in addition to the fact that C-Cl bonds are hard to displace ).
42.
The C-C triple bond length ranges from 119.2 pm in CaC 2 ( similar to ethyne ), to 130.3 pm in LaC 2 has been described in terms of La III with the extra electron delocalised into the antibonding orbital on C 2 2 ", explaining the metallic conduction.
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As expected from the fact that an electron is removed from the antibonding orbital when X 2 is ionized to [ X 2 ] +, the bond order as well as the bond strength in [ X 2 ] + gets higher, consequently the interatomic distances in the molecular ion is less than those in X 2.
44.
In such structures, the principal frontier electronic states are bonding and antibonding orbitals resulting from bonding between boron 2p orbitals and metal d orbitals; before group ( IV ), the number of available electrons in a unit cell is insufficient to fill all bonding orbitals, and beyond it they begin to fill the antibonding orbitals.
45.
In such structures, the principal frontier electronic states are bonding and antibonding orbitals resulting from bonding between boron 2p orbitals and metal d orbitals; before group ( IV ), the number of available electrons in a unit cell is insufficient to fill all bonding orbitals, and beyond it they begin to fill the antibonding orbitals.
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In the first excited state of O 2, a 22 kcal / mol energy increase from the ground state, both electrons in the antibonding orbitals occupy a degenerate ? * orbital, and oxygen is now in a singlet state ( indicated as 1 O 2 ) . 1 O 2 is very reactive with a lifetime between 10-100�s.
47.
However because Xe and O are electron rich both the bonding and antibonding orbitals will tend to be filled-this the'pi'system, if it existed wouldn't contribute much to bonding, if at all . . . Yet another reason to expect sp3 on oxygen . talk ) 14 : 09, 3 September 2009 ( UTC)
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This would give ( per atom ) one sp orbital occupied ( 2e ) giving a lone pair, one sp orbital bonding between atoms ( 1e per atom ) and the remaining 3 electrons per atom being placed on the doubly degenerate p orbitals ( this is how they will probably do it in text books note the third electron goes into an antibonding orbital ).
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:I imagine that it's easier for a base to deprotonate the OH than to do S N 2 on the Cl, because ( 1 ) deprotonation is less sterically hindered in this case, and ( 2 ) the OH probably already has some sort of interaction with the Cl, with an oxygen lone pair donating into the C-Cl ? * antibonding orbital to stabilise the molecule.
50.
For example, in the MO diagram provided for the [ Ti ( H 2 O ) 6 ] 3 + the " n " s orbital which is placed above ( " n " " 1 ) d in the representation of atomic orbitals ( AOs ) is used in a linear combination with the ligand orbitals, forming a very stable bonding orbital with significant ligand character as well as an unoccupied high energy antibonding orbital which is not shown.
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