Bonding Where the magic of chemistry takes place!.

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Presentation transcript:

Bonding Where the magic of chemistry takes place!

Ionic Bonding

More Ionic Bonding

Molecular Bonding Nonpolar Covalent Polar Covalent

Metallic Bonding The electrons lost by the metal are now delocalized (not belonging to a single cation) and “swim” in the unfilled d orbitals. This mobility allows for metals to have special properties including malleability, ductility, conductivity & luster.

Ionic vs. Covalent Bonding Animations www www FPs FPs

Molecular Geometry Animations re/Chapter10/VSEPR.html

Valence Shell Electron Pair Repulsion Model (VSEPR) Helps us to make Lewis Structures. Dictates that most atoms form octets and that electrons want to be as far apart as possible (atoms with many unpaired electrons are surrounding the highly bonded middle atom). Does not describe geometry; can’t describe lone pairs.

Hybridization Orbitals of different energy levels combine to form orbitals with equal energy. S and P orbitals to form sp orbitals. sp = 2 orbitals (linear, Be) sp 2 = 3 orbitals (trigonal planar, B) sp 3 = 4 orbitals (tetrahedral, C) These are the orbitals that create bonds

Role of Unshared Electrons Unshared electron pairs exhibit the sp orbital shape. NH 3 and H 2 O are good examples. Both have extra electron pairs that contribute to the overall structure of the molecule. Hybridization Movie

Unpaired Electrons (Double Bonds) Single bonds involving shared electrons in overlapping orbitals are called sigma bonds. Electron density is between nuclei. When electrons in non-bonding sp 2 or sp orbitals combine a pi bond (double bond) is formed. A double bond is made up of one sigma bond and one pi bond. Double Bonds

Examples CO (hybridization of C) See board.

Hybridization Animations entialchemistry/flash/hybrv18.swf entialchemistry/flash/hybrv18.swf

Formation of Sigma & Pi Bonds Through Orbital Overlapping mations/chang_7e_esp/bom5s2_6.sw mations/chang_7e_esp/bom5s2_6.sw

Bonding Review Video Clips Electronegativity & Polarity Lewis Dot Structures Molecular Geometry Intermolecular Forces