1. Metallic Bonds Form between 2 metal atoms. (metal and metal) The atoms are unstable – they do not have full electron rings. Bond by sharing very loosely held valence electrons with each other. (The electrons “ flow ” between the atoms.) Metallic bonds are NOT the strongest bonds though… Ionic Bonds are the strongest bonds!

2. Properties of Metallic Bonds Metallic compounds are highly conductive. (They conduct energy (heat & electricity) easily!!!) They also have metallic luster (shine) They are malleable (able to be hammered into thin sheets.) They are ductile (can be rolled into wires.) Examples: CuZn, AlSb, GaSb, LaMg

3. What makes it easier for some atoms to bond than others? When you think about bonding, what do atoms need to gain or lose? VALENCE ELECTRONS!!! N -3 Li +1 Which one will bond the easiest? Li +1 Why? The LESS electrons an atom needs to gain or lose to have a full outer ring, the EASIER it is for that atom to bond!!!

4. Which groups on the periodic table will share or transfer electrons the easiest? (i.e. be most likely to form bonds?) ANSWER: Groups 1 and 17 b/c group 1 only needs to get rid of 1e- and group 17 only needs to gain 1e-.