1. Multiple Bonds Chemistry 11 Ms. McGrath

2. Multiple Bonds A nonmetal with 4, 5 or 6 valence electrons have more than one unpaired electron. This results in the sharing of more than one pair of electrons to achieve an octet. For example, oxygen has six valence electrons – two electron pairs and two unpaired electrons. Oxygen will then form oxygen molecules by sharing two electrons with another oxygen molecule.

3. Multiple Bonds For example, oxygen has six valence electrons – two electron pairs and two unpaired electrons. Oxygen will then form oxygen molecules by sharing two electrons with another oxygen molecule. Demonstrate how nitrogen atoms form nitrogen molecules?

4. Multiple Bonds One pair of shared electrons is considered one bond and is called a single covalent bond. Two pairs of shared electrons is considered two bonds and is called a double covalent bond. Six shared electrons or three pairs of shared electrons are triple covalent bonds.

5. Multiple Bonds Atoms of unlike elements can also form double and triple bonds. For example: carbon dioxide, CO 2. What would this look like?

6. Multiple Bonds Try page 170, #4, 5, 6

7. Multiple Bonds Lewis structures are important to understand atoms bonding together. There is a simplified structure called structural formulas. Single bonds are represented using one single line. Double bonds are represented using two lines. Triple bonds are represented using three lines.