1. ionic Bonds

2. Gaining electrons = negative charge
Losing electrons = positive charge
An atom which gains or loses electrons is called an ion

3. Ionic bonds occur when an atom gives electrons away
Ionic bonds occur between a metal and a non-metal

4. Anion = ion with a negative charge Cation = ion with a positive charge b
Cation = ion with a positive charge
Ionic bond = the attraction between anions and cations
Very easy to predict because they always work to neutralize the charges

6. Group #
Valence e-
Type of Ion 1
+1 cation 2
+2 cation 13 3
+3 cation 14 4
+ or -4 ion 15 5
-3 anion 16 6
-2 anion 17 7
-1 anion 18 8
Does not bond

7. Ionic compounds tend to form crystal lattice structures where the atoms are organized so the ions are balanced

8. In a crystal lattice, each positive ion is surrounded by negative ions and vice versa

10. Ionic bonds are strong and require a large amount of energy to break
Therefore, ionic compounds have high melting and boiling points.
Solid ionic compounds are nonconductors because of the balance of the ions’ charges

11. Liquid ionic compounds are conductors because their ions are free to move.
An electrolyte is an ionic compound in aqueous solution which conducts electricity.

12. Some ionic compounds contain polyatomic ions
Polyatomic ions are groups of elements which function as a single ion
NH C2H3O2

14. Metallic Bonds Metallic bonds occur between metal atoms
In metallic bonds, atoms do not give away or share electrons

15. In metallic bonding the valence shell of the atoms overlap creating an “electron sea”

16. The valence electrons move freely
These electrons are called “delocalized” electrons
A metallic bond is the attraction of a metal cation to delocalized electrons

18. Metallic properties can be contributed to the loose valence electrons.