1 / 15

Mastering Lewis Structures: Hooking Atoms in Covalent Compounds

Learn how atoms in covalent compounds are bonded following rules for Lewis structures. Understand steps, hints, and practice problems with examples like CCl4, NH3, and SF6.

millerlisa
Download Presentation

Mastering Lewis Structures: Hooking Atoms in Covalent Compounds

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. Lewis Structures

  2. Lewis Structures • How the atoms in covalent compounds are hooked together. • Similar to Lewis Dot Diagrams • Must follow a set of rules to get the Lewis Structure

  3. The RULES 1. Add up the number of valence electrons in the compound 2. Guess at a structure and hook the atoms together using single bonds A) Usually the first element is in the middle B) Usually the most metallic element is in the middle 3. Give all atoms on the outside an octet 4. If you have electrons left over after step 3 then add all of them to the central atom 5. If you don’t have enough electrons to give the central atom an octet A) Check for deficient atoms (Be, B, Al) B) Try a double bond C) Try a triple bond

  4. HINTS • Leave a big gap in your notes for a list of hints

  5. Practice Problems • Carbon tetrachloride • CCl4 • HINT: Carbon is almost always in the middle

  6. Practice Problems • Ammonia • NH3 • HINT: Hydrogen only needs two electrons to get an “octet”

  7. Practice Problems • Sulfur hexafluoride • SF6 • HINT: Some central atoms can have more than an octet of electrons. S and P do this often.

  8. Practice Problems • Boron trihydride • BH3 • There is no way Boron can have an octet • HINT: Boron, Beryllium, and Aluminum very rarely have an octet of electrons.

  9. Practice Problems • Formaldehyde, CH2O • Which structure is correct? • HINT: The most symmetric structure is usually the correct one.

  10. Practice Problems • Hydrogen cyanide, HCN

  11. Practice Problems • Nitrate ion

  12. Practice Problems • Acetylene, C2H2

  13. Practice Problems • Carbon dioxide

  14. Practice Problems • R-134a, CF3CH2F

  15. Practice Problems • Nitrite ion

More Related