1 / 14

Understanding Chemical Bonding: Energy, Structures, and Molecular Nomenclature

Explore the intriguing world of chemical bonding in Chapters 6 and 7, focusing on the energy associated with bond formation, potential energy, and the stability of molecular compounds. Learn about Lewis structures, the octet rule, and the significance of bond energy and bond length. Discover how to name binary compounds using the prefix system, followed by practical examples such as carbon tetrachloride and dinitrogen monoxide. Delve into the properties of nonpolar and polar covalent bonds, as well as the seven diatomic elements essential to chemistry.

pello
Télécharger la présentation

Understanding Chemical Bonding: Energy, Structures, and Molecular Nomenclature

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. Ch. 6 & 7 - Chemical Bonding II. Molecular Compounds

  2. A. Energy of Bond Formation • Potential Energy • based on position of an object • low PE = high stability

  3. no interaction increased attraction A. Energy of Bond Formation • Potential Energy Diagram attraction vs. repulsion

  4. increased repulsion balanced attraction & repulsion A. Energy of Bond Formation • Potential Energy Diagram attraction vs. repulsion

  5. Bond Energy Bond Length A. Energy of Bond Formation • Bond Energy • Energy required to break a bond

  6. A. Energy of Bond Formation • Bond Energy • Short bond = high bond energy

  7. X 2s 2p B. Lewis Structures • Electron Dot Diagrams • show valence e- as dots • distribute dots like arrows in an orbital diagram • 4 sides = 1 s-orbital, 3 p-orbitals • EX: oxygen O

  8. Ne B. Lewis Structures • Octet Rule • Most atoms form bonds in order to obtain 8 valence e- • Full energy level stability ~ Noble Gases

  9. - + + B. Lewis Structures • Nonpolar Covalent - no charges • Polar Covalent - partial charges

  10. C. Molecular Nomenclature • Prefix System (binary compounds) 1. Less e-neg atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3. Change the ending of the second element to -ide.

  11. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 C. Molecular Nomenclature

  12. C. Molecular Nomenclature • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  13. C. Molecular Nomenclature • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  14. C. Molecular Nomenclature • The Seven Diatomic Elements Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

More Related