1 / 10

Lewis dot structures with atoms that break the octet rule

Learn about breaking the octet rule in Lewis dot structures, including odd electron compounds, electron deficient compounds, and expanded valence shells. Explore examples such as BCl3 and BeH2. Practice drawing Lewis dot structures for BF3 and SF6.

nathan-serrano
Download Presentation

Lewis dot structures with atoms that break the octet rule

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 dot structures with atoms that break the octet rule

  2. Breaking the octet rule • Some compounds have atoms with more or less than 8 electrons around them (breaking the octet rule) • There are 3 types • 1. odd numbered electrons • 2. electron deficient compounds • 3. expanded valence shells

  3. Odd electron • Although rare, it is possible to have compounds that have an odd number of electrons. • Obviously it is not possible to satisfy the octet rule with an odd number of electrons, ONE CANNOT BE A PAIR! • Two compounds are NO and NO2 • They will have a free electron.

  4. Lewis dot

  5. The formal charge is appropriate for each atom and the molecule • Compounds with a free electron, unpaired electron, are called free radicals. • They are highly reactive. • These two compounds are used in nitrous oxide systems in cars

  6. Electron deficient compounds • This is rare. It is only found Boron, Beryllium or Aluminum compounds. All are highly reactive. • Beryllium, aluminum are a metals, however, since its valence shell is so close to the nucleus it can form covalent bonds (rarely). • All atoms are electron deficient (have less than 4 electrons), and therefore when they form bonds they can’t make it all the way up to 8 electrons

  7. Examples • BCl3 • BeH2

  8. Expanded valance shells • One atom will have more than 8 valence electrons. • This requires a highly electronegative atoms (fluorine, oxygen, or chlorine) to bond with a nonmetal with its outer shell 3 p or higher. • Only the central atom will have more than 8 electrons. • C, N, O, F and Ne can’t have more than 8 electrons. There is no 2 d orbital so there is nowhere to put the extra electrons. • All nonmetals underneath them on the periodic table do have an used d orbital for the electrons.

  9. Examples • PF5 • XeF4 • ClF5 • NO3- • SO42-

  10. Homework • Draw the Lewis dot structure for • BF3 and SF6

More Related