Ionic Bonding, NaCl

NaCl - Crystal Lattice

Covalent Bond

Covalent Bond

Gilbert Lewis (1875 – 1946)

Steps for drawing Lewis Structures

Boron – Unfilled Octet

Rx of ammonia with Boron Trifluoride

Sulfur – overfilled octet

Coordinate Covalent Bonding

Linear – 180 bond angle

Trigonal planar – 120° bond angle

Tetrahedral – 109.5° bond angle

Trigonal bipyramidal – 90°,120°

Octahedral - 90° bond angles

Trigonal pyramidal – 107° bond angles

Bent – 104.5° bond angle

Square Pyramidal – bond angle 90°

VSEPR Theory 3D Shapes

VSEPR Shapes (cont’d)

Steps of VSEPR Theory

Non-polar and Polar Covalent Bonds

Hydrogen fluoride

Electronegativity Trends

Electronegativity Trends

Electronegativity Values

Bond dipole

Water dipoles orient themselves to an electric field

Net Negative Dipole

No net dipole, CO2

Molecular Shapes with No Net Dipole

Johannes van der Waals (1837 – 1923)

Dipole-Dipole Forces

Dipole-Dipole Force

Hydrogen Bonding in Water

Boiling Points of Covalent Hydrides

Fritz London (1900 – 1954)

London Dispersion Force

Noble Gases can freeze due to London Dispersion Forces

Boiling Point increases as Molar Mass Increases

Water Beading, Hydrogen Bonding

Surface Tension

Capillary Action

Capillary Action

Viscosity – resistance to flow

Composite Materials

Electron Sea Theory

Molecular Crystal - Snowflake

Covalent Network Crystals - Diamonds

Diamond vs. Graphite

Different Structures of Carbon

Semiconductors

n – type semiconductor