Molecular Structure and Simple Covalent Bonding Models
Covalent bonding can be thought of as the situation when groups of atoms stay associated with each other independent of the phase
Valence Bond Theory: bonding occurs when pairs of electrons accumulate between nuclei
Paired electrons screen the nuclear charge, so nuclear-electron attraction overcomes electron-electron repulsion giving a net attraction of nuclei.
Lewis Dot structures
Electrons are distributed about atoms pictorially.
Only use valence electrons.
Lines represent an electron pair, either as a bond or a lone pair.
The formal charge about each atom should be minimized (neutral is best).
The octet "rule" works well for C, N, O, F but otherwise is merely advisory.
Resonance is a superposition of degenerate (equivalent) VB structures - this helps minimize charge distribution.
The net structure is a weighted average of all possible dot structures; the weighting is based on the relative energy of each resonance structure: low-energy structures contribute a lot and high-energy structures contribute little
Neutral structure perhaps contributes less than ionic structures (Why?)
Valence Shell Electron Pair Repulsion model (VSEPR)
A simple application of Coulombs Law to Lewis Dot structures - electron pairs distribute themselves to minimize electron-electron repulsion
1) Draw the best Lewis Dot structure with minimum formal charges
2) Count the number of lone pairs and bonds (sb=db=tb) about the center of interest
3) Distribute the electron density as follows:
Count Distribution Geometry 2 linear 180o angles 3 trigonal planar
4 tetrahedral 109o angles 5 trigonal bipyramid 120o and
6 octahedral 90o angles 7 pentagonal bipyramid 72o and
4) Distribute the lone pairs and bonds to minimize repulsions using the following:
lp-lp > lp-bp > bp-bp (tb > db > sb)
5) Fine geometry is dictated by lp-bp repulsions
Hybridization : one way to generate molecular orbitals to be used in VB theory
Wave interference can occur on-site (same atom) as well as between atoms: this costs energy but the energy is recovered upon bond formation.
Hybridization probably occurs because of atom-atom repulsions so is more prevalent among first row atoms than anywhere else on the Periodic Table.
Understanding the relative phases of orbitals is important because constructive interference (orbitals with the same phase) increases orbital size while destructive interference (orbitals of opposite phase) decreases the orbital size.
Some common types of hybrids:
(convention : the unique axis is defined as the z axis)
hybrid geometry orbitals used sp linear s + pz sp2 trigonal s + px + py sp3 tetrahedral s + px + py + pz sd3 tetrahedral s + dxy + dyz + dxz dsp2 square planar s + px + py + dx2-y2 dsp3 trigonal bipyramid s + px + py + pz + dz2 d2sp3 octahedral s + px + py + pz + dz2 + dx2-y2