October 21, 2021, 06:12:28 PM
Forum Rules: Read This Before Posting


Topic: About Molecular Orbital!  (Read 14707 times)

0 Members and 1 Guest are viewing this topic.

Offline Donaldson Tan

  • Editor, New Asia Republic
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 3178
  • Mole Snacks: +261/-13
  • Gender: Male
    • New Asia Republic
Re:About Molecular Orbital!
« Reply #15 on: February 06, 2005, 08:49:05 AM »
overlapping and superimposing are kinda the same thing, except the latter emphasises more on wave mechanics.

in a region where two orbitals of both + signs overlap, electron density is higher than the mere sum of the electron density of the two seperate orbitals. More electrons density is shared between two atoms. the attraction of both nuclei for these electrons is greater than the mutual repulsion of the nuclei, and a net attractive fore aka bonding intereaction occurs.

in regions where two orbitals of both - signs overlap, there is effectively no electrons between the nuclei, Hence, there is only repulsion force between the 2 nuclei, hence no bonding occurs.

in regions where two orbitals of opposite signs overlap, the electron density present between two nuclei might not be sufficient to produce an attractive force stronger than the repulsion force between the nuclei. The electron density between the two nuclei in this molecular orbital is less than the sum of individual electron density of each orbitals. Hence, no bonding occurs.
"Say you're in a [chemical] plant and there's a snake on the floor. What are you going to do? Call a consultant? Get a meeting together to talk about which color is the snake? Employees should do one thing: walk over there and you step on the friggin� snake." - Jean-Pierre Garnier, CEO of Glaxosmithkline, June 2006

Sponsored Links