1. What you’ve learned so far….

2.  Atoms form bonds in more than one way  In IONIC bonding, atoms give up or gain electrons  In COVALENT bonding, atoms share electrons

3.  Valence electrons and bonding can be shown by using ELECTRON DOT DIAGRAMS (aka Lewis Structures)  Ionic bonds form due to the attraction of positive & negative ions  Ionic bonds are NEUTRAL because the opposite charges cancel each other out  Covalent bonds are held together by the attraction of each atom’s nucleus for the shared pair of electrons

4.  Ionic bonds occur between metals & non- metals; covalent bonds between non-metals & non-metals  Covalent bonds form MOLECULAR COMPOUNDS  Molecular compounds consist of electrically neutral molecules, NOT IONS, so they do not have charged particles to conduct electricity

5.  Ionic Bonding

6.  Covalent Bonds / Molecular Compounds Example of a single covalent bond CH 4

7. Double Bond Example Using O 2

8.  Polar molecules are covalent bonds in which electrons are shared unequally  Some atoms pull more strongly on the shared electrons than other atoms do.  This results in the electrons moving closer to one atom, causing the atoms to have slight electrical charges.

9. Water molecules are good examples of polar covalent bonds

10. Shared equally = non-polar bond Carbon Dioxide