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Published byJewel Brooks Modified over 8 years ago
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Ionic Bonding, NaCl
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NaCl - Crystal Lattice
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Covalent Bond
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Gilbert Lewis (1875 – 1946)
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Steps for drawing Lewis Structures
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Boron – Unfilled Octet
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Rx of ammonia with Boron Trifluoride
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Sulfur – overfilled octet
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Coordinate Covalent Bonding
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Linear – 180 bond angle
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Trigonal planar – 120° bond angle
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Tetrahedral – 109.5° bond angle
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Trigonal bipyramidal – 90°,120°
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Octahedral - 90° bond angles
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Trigonal pyramidal – 107° bond angles
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Bent – 104.5° bond angle
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Square Pyramidal – bond angle 90°
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VSEPR Theory 3D Shapes
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VSEPR Shapes (cont’d)
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Steps of VSEPR Theory
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Non-polar and Polar Covalent Bonds
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Hydrogen fluoride
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Electronegativity Trends
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Electronegativity Values
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Bond dipole
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Water dipoles orient themselves to an electric field
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Net Negative Dipole
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No net dipole, CO 2
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Molecular Shapes with No Net Dipole
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Johannes van der Waals (1837 – 1923)
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Dipole-Dipole Forces
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Dipole-Dipole Force
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Hydrogen Bonding in Water
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Boiling Points of Covalent Hydrides
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Fritz London (1900 – 1954)
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London Dispersion Force
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Noble Gases can freeze due to London Dispersion Forces
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Boiling Point increases as Molar Mass Increases
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Water Beading, Hydrogen Bonding
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Surface Tension
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Capillary Action
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Viscosity – resistance to flow
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Composite Materials
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Electron Sea Theory
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Molecular Crystal - Snowflake
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Covalent Network Crystals - Diamonds
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Diamond vs. Graphite
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Different Structures of Carbon
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Semiconductors
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n – type semiconductor
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