Valence and MO Theories Flashcards
Valence Bond Theory
A covalent bond forms when orbital of two atoms overlap, and a pair of electrons is localized in the region between the atoms
3 Principles of Valence Bond Theory
- The pair of electrons has opposite spins
- Good, in-phase overlap leads to strong bonding interactions
- Orbitals can hybridize to more appropriate shapes and orientations, to maximize overlap.
Molecular Orbital Theory and basic principle
A bonding approach in which quantum mechanics is applied to molecules
The Schrödinger equation is solved for electrons in a molecule, resulting in molecular orbitals
Molecular Orbitals Similarities to Atomic Orbitals
They can each hold two electrons w/ opposite spins
The square of the molecular orbital wave function gives the probability function
Features of MO diagrams
- Number of MOs = AOs
- Combining 2 AOs gives a bonding MO and an antibonding MO
- In ground state configurations, electrons occupy lowest energy MO upwards
- Bond strength can be measured by the calculated bond order
- Bond order = 1/2(no. of bonding es - no. of non-bonding es)
How do you calculate Bond Order?
Calculate from Molecular Order Theory
BO = 1/2(MO-MO*)
= 1/2 (bonding e - antibonding e)
Sigma Bond
End-to-end overlap of orbitals with electron density along axis of bond from MO Theory
single bonds and first overlap in multi-bonds
Pi bond
side-to-side overlap of orbitals, with electron density above and below axis of bond in MO theory
extra overlaps in multiple bonds
Limitations of Hybridization Schemes
- VBT does not always match experimental data
- Don’t work for d-orbitals
- Misleading when molecules have resonance
Hybridization
A hypothetical process so tetrahedral geometry can be modified to create hybrid orbitals when bonding occurs
MO Triangle shape and Nonmetals
Sigma
Pi pi
Sigma
Pi pi
B2 C2 N2
MO oval shape and Nonmetals
Sigma
Pi pi
Pi pi
Sigma
O2 F2
Hybridization Rules
Number of hybrid orbitals = number of orbitals mixed
Type of hybrid orbitals varies on the types of atomic orbitals mixed (s + p = sp)
Bond Order Trend
Positive ion = low bond order
Negative ion = high bond order
Fewest antibonding electrons
Bond Length Trend
Reverse of bond order trend
positive ion = longest bond length
negative ion = shortest bond length