1 / 19

COVALENT BONDING

COVALENT BONDING. Review of Ionic Bonding. Atoms always want to have their valence shells filled to make them stable Ionic bonds are between a metal and a nonmetal… In Ionic bonds: Anions TAKE ELECTRONS from Cations What happens if we have a combination of two non-metals?.

melvin-taylor
Download Presentation

COVALENT BONDING

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. COVALENT BONDING

  2. Review of Ionic Bonding • Atoms always want to have their valence shells filled to make them stable • Ionic bonds are between a metal and a nonmetal… • In Ionic bonds: • Anions TAKE ELECTRONS from Cations • What happens if we have a combination of two non-metals?

  3. Covalent Bonding • TwoNON-METALS can bond together in a COVALENT BOND • Let’s break this word down: • The prefix “Co” = to share • “Valent” comes from valence • So “COVALENT” means to SHARE VALENCE ELECTRONS when bonding

  4. Covalent Bonding • Many non-metals actually make covalent bonds in nature • Example: The oxygen we breathe is NOT just an individual oxygen ATOM… • It is actually an OXYGEN MOLECULE • Molecule = Atoms that are joined together

  5. Take 5 to summarize • LEFT SIDE OF NOTEBOOK • Look through the notes we just took • In your own words, explain key points or describe new information. • You may work on your own or discuss QUIETLY with your partner

  6. So let’s take a look at our dear friend Chlorine…

  7. UNPAIRED ELECTRONS Example:Chlorine Cl Cl

  8. Cl Cl - Cl2 This is a “single bond”

  9. So let’s take a look at our dear friend Oxygen…

  10. O O UNPAIRED ELECTRONS SHARE ELECTRONS TO MAKE PAIRS Lewis Diagrams of Oxygen

  11. The unpaired electrons from each oxygen are shared O O O O Shared electrons (new electron pairs) Are both electron shells happy now?

  12. O O They are now bound together by a covalent bond = O2 Each line represents a bond between 2 e- This is a “double bond”

  13. Covalent Bonds can be… • “Single Bonds” • “Double Bonds” • “Triple Bonds”

  14. Sometimes, more than two atoms are involved… Cl S Cl

  15. The unpaired electrons from S and Clare SHARED Cl S Cl

  16. EVERYBODY IS HAPPY!  Cl S Cl

  17. If there is no number, that means there is only 1 If there are more than one, we write the number like this All three are now bound together by covalent bonds SCl2

  18. Hydrogen • Acts like a nonmetal • Wants to have 2 electrons total (wants to look like Helium!) H

  19. Let’s Try Some

More Related