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

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

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

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

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.

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

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!

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

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

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

Covalent Bonds

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

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