chapter 10 chemical bonding ii. lewis structure molecular structure structure determines chemical...
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Electron domain/group: area where electrons appear in Lewis structures.
It can be electron lone pairs, single bonds,
double bonds, triple bonds, or single electrons.
H2O, NH3, CH4, O2, N2, SCl2, CCl4, PCl3, NO+, NH4
+, CO, CO2
Valence Shell Electron Pair Repulsion (VSEPR) model
The lowest energy arrangement of a given number of electron
domains is the one that minimizes the repulsions among them.
The shape of ABn molecules or ions depend on the number of
electron domains surrounding the central A atom.
number of electron domains: 2 to 6
How to predict geometry of a molecule?
1) Draw the Lewis structure of the molecule or ion, and countthe number of electron domains around the central atom.
2) Determine the electron domain arrangement by arranging theelectron domains about the central atom so that the repulsionsamong them are minimized.
3) Use the arrangement of the bonded atoms to determine the molecular geometry.
CO2
Electron domains for multiple bonds exert a greaterrepulsion force on adjacent electron domains than do electron domains for single bonds.
lone pair-lone pair > lone pair-bonding pair > bonding pair- bonding pair
SO2
119°
Electron domain arrangement is not necessarily the same as the molecular structure.
Bent or V-shaped
SF4
To minimize repulsion, electron lone pairs are always placed in equatorial positions for trigonal bipyramidal geometry.
+ −Dipole
Dipole has a magnitude and a direction — vector
Magnitude (length) of a dipole — dipole moment
μ = qr
q — charge, r — distance between + and − charge
Polarity of a molecule
dipole moment of a molecule ≠ 0 ↔ polar molecule
dipole moment of a molecule = 0 ↔ nonpolar molecule
dipole of a molecule = sum of all the bond dipoles
EH
Atoms → atomic orbitals
Molecules → molecular orbitals
Molecular Orbital (MO)≈ Linear Combination of Atomic Orbitals (LCAO)
Bond order = ½ (number of bonding electrons − number of antibonding electrons)
If bond order > 0, the molecule is stable
If bond order = 0, the molecule is not stable
bond order = 1 → single bond
bond order = 2 → double bond
bond order = 3 → triple bond
O2, F2, Ne2: (σ2s) (σ2s*) (σ2p) (π2p) (π2p
*) (σ2p*)
B2, C2, N2: (σ2s) (σ2s*) (π2p) (σ2p) (π2p
*) (σ2p*)
1)Electron configuration.
2)Bond order → stable molecule/ion?
3)Paramagnetic or Diamagnetic?
O2, F2, N2, N2−, N2
+