Ionic Bonding, NaCl
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Transcript of Ionic Bonding, NaCl
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