1. Covalent Bonds Notes

2. Single Bonds A bond in which two or more atoms share a pair of electrons H + H  H-H Each hydrogen now achieves the electron configuration of the noble gas Helium. The dash represents a pair of electrons that are being shared Dashes are NOT used for ionic bonds!

3. Covalent bonding occurs between nonmetals. If it is a metal and a non-metal then it will be an ionic bond. F + F  F-F Each Fluorine atom shares one electron The electrons around the fluorine atoms are considered to be lone pairs or non- bonding pairs

4. What would the structural diagram of water look like? H + H + O  H-O-H

5. What happens when you form CH 4 (methane)?

6. Double bonds – atoms share 4 electrons Triple bonds – atoms share 6 electrons Double and Triple Bonds

7. Carbon dioxide: Nitrogen:

8. Coordinate Covalent Bonds A covalent bond in which one atom contributes both bonding electrons to form the bond. All polyatomic ions are Coordinate covalent bonds.

9. Resonance Structures that occur when it is possible to write more than one electron dot formula that have the same number of electron pairs. When electrons are all paired it is called diamagnetism. When electrons are NOT all paired, it is called paramagnetic.