Molecular Orbital Diagrams

Bond Oder must be

above 0 in order for the bond to be stable.

Antibonding I higher energy

because the energy in bonding is lower since it’s more favorable (think of the couple)

Antibonding means

electrons that are not in bonds, ie in Lewis they would be lone pair electrons

for s orbitals, the only possible bonding is

sigma

Sigma bonds are

hybridized to hybridized (explain)

Pi bonds are

unhybridized to unhbyrdized (explain)

Constructive interference is why

we have bonding orbitals

Destructive interference is why

we have antibonding orbitals

Draw bonding and anti bonding orbitals

Ok!

Bonding an UdAntibonding is product of

orbital being in phase and out of phase

Orbital Mixing happens

when the 2s and 2p orbitals are I close in energy, causing there to be repulsion between sigma bonds. The pi 2p is then higher.

In homonuclear diatomic orbital mixing happens when

Z is less than or equal to 7

MO gives us better information about

paramagnetism

In heteronuclear diatomics,

mixing happens when Zsum is less than or equal to 15

With heteronucelar diatomic MO’s we don’t have

Sigma 2p, 2s anymore rather we count up since the orbitals interacting don’t necessarily have to be the same.

Bond order equals

bonding - anti/nonbonding /2

In heteronucelar atoms, energy levels differ

due to difference in electronegativity, atomic radii, and Zeffective

In heteronucelar atoms, electron cloud distortion happens because

difference in electronegativity, atomic radii, and Zeffective

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Nana Asare Osei-Agyei