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For each of the following species: C2+ & O2- Write the molecular orbital energy diagram and fill in the electrons Hint: in each case, the number of valence electrons in the species is determined first; this is followed by the valence molecular orbital diagram for each species. Find the bond order and state whether the species is stable or unstable Hint: Bond order = (# of bonding e- - # of antibonding e-) ¸ 2 Determine if the species is diamagnetic or paramagnetic Hint: indicate the number of unpaired electrons

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Molecular orbital energy is the energy associated with each electron in an atom or molecule.

It is expressed in electron volts (eV) and is determined by the electron's position in the atom or molecule. The molecular orbital energy diagram and fill-in the electrons are given here in each case, the number of valence electrons in the species is determined first; this is followed by the valence molecular orbital diagram for each species.

C2+: Molecular Orbital Energy Diagram

1s2 2s2 2p2

σ2s*  ← 0 e-  

σ2s   ← 2 e-

σ2p*  ← 0 e-  

σ2p   ← 0 e-

π2p*  ← 0 e-  

π2p   ← 0 e-

Bond Order: 0

Stability: Unstable

Magnetism: Diamagnetic (no unpaired electrons)

O2-: Molecular Orbital Energy Diagram

1s2 2s2 2p4

σ2s*  ← 0 e-  

σ2s   ← 2 e-

σ2p*  ← 0 e-  

σ2p   ← 2 e-

π2p*  ← 0 e-  

π2p   ← 2 e-

Bond Order: 1

Stability: Stable

Magnetism: Paramagnetic (2 unpaired electrons)

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