Apply molecular orbital theory to predict which species has the
strongest bond.
Apply molecular orbital theory to predict which species has the
strongest bond.
O+2
O−2
O2
All bonds are equivalent according to molecular orbital
theory.
Molecular Orbital Theory -- Homodiatomics Use the molecular
orbital model to fully describe the bonding in O2+, O2, O2-, and
O22-. Determine which of the following statements are true and
which are false.
The electron configuration of O2- is
(σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)
The electron configuration of O2+ is
(σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)
The number of unpaired electrons in O2+ and O22- is,
respectively, 1 and 2.
The bond lengths increase in the order: O2+ < O2 < O2-
< O22-.
The bond order in O2+...
Subject: Physical Chemistry
Topic: Molecular Orbital Theory
Explain why the energy stabilization for bonding orbitals is
less than the destabilization energy for antibonding orbitals.
Molecular Orbital Theory
1.1 Which model, the Lewis electron dot
structure or the MO energy level diagram, better describes the
bonding in O2? Remember that liquid O2 is
attracted into the magnetic field of a large magnet.
True or False.
_____ MO theory allows us to avoid the use of resonance.
_____ Resonance is a concept which arises from the limitations
of Lewis electron dot structures
1.2 As we go from Li2 to
Li3 to Li4 to Lin, the number...
After thoroughly reviewing atomic orbital theory and molecular
orbital theory, respond to the following:
Explain how atomic orbitals interact and give rise to molecular
orbitals.
written in 250 words minimum
Prepare a molecular orbital diagram for the BeH2 molecule.
Assume in orbital potential energy of 4.0 eV for the 2p orbitals of
Be and -9.3eV for the 2s orbital. Assume that both the 2p and the
2s of Be interact with the two group orbitals of the hydrogens.