Download Covalent Bonding

Strength of Bonds
Covalent Bonding
[Hybridization and Geometry]
Hybridization:
•In molecular compounds, orbital hybridization occurs.
•Valence Orbitals = ‘s’ & ‘p’ sublevels (4 total orbitals)
•S & P orbitals merge to form a hybrid orbital.
•Number of hybrid orbitals depends on locations of electron
density (# domains).
•Only Central Atoms experience hybridization.
•Bond dissociation energy: the amount of energy
required to break the bond between two covalently
bonded atoms.
•Single Bond < Double Bond < Triple Bond
Hybridization
• Site of electron density → “Steric Site” AKA Domain
• Both chemical bonds & lone pairs count as a steric site.
• 2 domains = sp hybrid.
• 3 domains = sp2 hybrid.
• 4 domains = sp3 hybrid.
• 5 domains = sp3d hybrid.
• With every increase in domains, you add another orbital to become
hybridized.
Valence Shell Electron Pair Repulsion Theory
(VSEPR)
•Structural formulas show relationships of atoms.
•They lack ability to show 3D shape.
•Atoms orient themselves as far apart from each other
•Molecules with zero lone pairs spread evenly 360°
•Lone pairs on the central atom will cause repulsion between
other lone pairs and bonds.
Structures: Draw structures & give VSEPR
(AXxEx) Classification
•CH4
VSEPR Classification:
Hybridization:
VSEPR Notation
•AXE Method:
•AXxEx
•A = Central Atom
•X = Number of bonded atoms off central atom
•E = Number of lone pairs on the central atom
•A certain AXE classification tells you → shape &
bonding angles.
Structures: Draw structures & give VSEPR
(AXxEx) Classification
•BHCl2
VSEPR Classification:
Hybridization:
Bond Angles:
Bond Angles:
Shape:
Shape:
Structures: Draw structures & give VSEPR
(AXxEx) Classification
VSEPR Classification:
•PCl5
Hybridization:
Bond Angles:
Shape:
HOMEWORK CHART:
structure, hybridization, AXE, shape, bond angles, show
partial charges (polarity) on bonds
1.
2.
3.
4.
5.
SF4
BH3
O3
CO2
CCl4
6.
7.
8.
9.
10.
SF6
OCl2
NF3
BF3
COF2