1 / 19

Chemical Bonding: Types, Structures & Applications

Explore why atoms stick together through ionic, covalent, and metallic bonding. Learn about valence electrons, Lewis structures, and molecular properties. Practice drawing structures and understanding bond reactivity.

elmeri
Télécharger la présentation

Chemical Bonding: Types, Structures & Applications

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemical Bonding Why do atoms stick together, anyway? Who cares?

  2. Types of Bonding • Ionic • Covalent • Metallic Ionic Bonding: Covalent Bonding:

  3. Covalent Bonding Uses Valence Electrons

  4. Also called Lewis Dot Symbols

  5. How many valence electrons does a Si atom have? • 1 • 2 • 3 • 4 • 5 • 6 • 7 • 8

  6. Lewis Electron-Dot Structures:Describing Bonding in p-block compounds

  7. Interpreting Lewis Structures

  8. Drawing your own Lewis Structures

  9. How many total bonding electrons does an acetate ion have? 1. 3.5 • 7 • 8 • 10 • 12 • 13 • 14 • 15

  10. Why bother? Resonance Number of Bonds Molecular Structure Reactivity Lewis Structure Polarity Physical State and Properties Spectroscopy Hydrophilicity and phobicity

  11. Back to Drawing Lewis Structures I have an idea. Do what I say.

  12. Back to Drawing Lewis Structures

  13. Examples

  14. Examples with multiple bonds N2

  15. Examples: Exceptions to the Octet Rule ClF5

  16. Examples: Reading Organic Structures CH3CH3 CH3CN CHCCHCH2

  17. Draw the Lewis structure for SO3. How many lone pairs does it have? • 1 • 2 • 3 • 4 • 0

  18. Draw the Lewis structure for NO2-. How many lone pairs does it have? • 1 • 2 • 3 • 4 • 0

More Related