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This overlap region has a high electron charge density. The more extensive the overlap between two orbitals, the stronger is the bond between two atoms.
account for shape in terms of quantum mechanics. determine the orbitals that are involved in bonding.
In order for these orbitals to mix they must: Have similar energy levels. Overlap well (similar orientation). Be close together.
It incorrectly assumes that electron are localized and so the concept of resonance must be added The model does not deal effectively with molecules containing unpaired electrons. The model gives no direct information about bonding energies
Bond strength (larger bond order means greater bond strength). Number of bonds that exist between two atoms. Existence of molecules or ions
As the bond order increases, the bond energy increases and the bond length decreases. Large bond energy associated with N2 molecule, which the MOT model predicts will have a bond order of 3, a triple bond.
Sigma (σ) bond pi (π)
Overlapping of one s orbital with another s orbital Overlapping of one s orbital with a p orbital Head on overlapping of one p with another p orbital
Electron-group geometry - determined by the locations of regions of high electron density around the central atom(s). Molecular geometry/shape of a molecule - determined by the arrangement of atoms around the central atom(s). (Electron pairs are not used in the molecular geometry determination. Just the positions of the atoms in the molecule are used.)
2: Linear (180°) 3: Trigonal planar (120°) 4: Tetrahedral (109.5°) 5: Trigonal bipyramidal (120°, 90°) 6: Octahedral (90°)
For example, the bond dipoles in CO2 cancel each other because CO2 is linear.
Chlorine generally forms one bond and has one unpaired electron. Oxygen, with two unpaired electrons, usually forms two bonds. However, carbon, with only two unpaired electrons, generally forms four bonds. For example, methane, CH4, is well known.
Four unpaired electrons are formed as an electron from the 2s orbital is promoted (excited) to the vacant 2p orbital. More than enough energy is supplied for this promotion from the formation of two additional covalent bonds.
A 3s electron can be promoted to a 3d subshell, which gives rise to a set of five sp3d hybrid orbitals
A 3s and a 3p electron can be promoted to the 3d subshell, which gives rise to a set of six sp3d2 hybrid orbitals
Write a plausible Lewis structure for the molecule or ion Use the VSEPR method to predict the electron-group geometry of the central atom Select the hybridization scheme that corresponds to the VSEPR prediction Describe the orbital overlap and molecular geometry
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