1. November 11, 2015 Write 3 things you learned/know about ionic bonds.
Why does Oxygen commonly have a -2 charge?

2. Goals To explain the difference between the types of bonds.
To identify what bond is present in a chemical compound.
To draw chemical bonds

3. Agenda Items Common Assessment will be Thursday 11/19 Bell Work
Discuss Activity and Collect Packet
Return Practice Packet
Ionic Bond Racing
Notes on Covalent Bonds
Hand out Study Guide for Common Assessment
Homework: Study for tomorrow’s Ionic Bonding Quiz
Common Assessment will be
Thursday 11/19

4. Remember: Ionic Bonds Metals and nonmetals Give and take
Not always a 1:1 ratio
IONS are formed (opposites attract)

5. Covalent Bonds (sharing is caring!)
Formed when atoms SHARE valence e-
Occurs between nonmetals ONLY!
Two atoms can share electrons, and be held together by their mutual attraction to the shared electrons.

6. Covalent Bonds
Atoms with 1 unpaired valence e- share their unpaired e- as shown below

7. Covalent Bonds
A substance that is made of atoms with covalent bonds is called a covalent compound
Molecules – any group of atoms held together by covalent bonds.
This means anything that has ionic bonds cannot be called a molecule!

8. Covalent Bonds
A straight line is used to represent two electrons that are involved in a covalent bond
H H

9. Covalent Bonds O=O Sometimes, atoms need to share more than 2 e-.
If they share 4 e-, it’s called a double bond. (shown by 2 lines)
O=O

10. Covalent Bonds
If they share 6 e-, it’s called a triple bond. (shown by 3 lines)
N N

11. Covalent Bonds

12. Covalent Bonds
Covalent bonds can be POLAR (which means the e- are shared unequally) or NONPOLAR (which means the electrons are shared equally)

13. 3. Metallic Bonds Form between metals
Metals like to give up e- so a “net” of free e- is formed, making a sea of e- to hold atoms in place (attracted to + nuclei)
Strongest of all bonds
metallic  ionic  covalent