1. Ionic and Metallic Bonds
Chapter 8 Section 3
Ionic and Metallic Bonds

2. Ions
An ion is an atom that is no longer electrically neutral because it has gained or lost electrons.
An ion that loses electrons becomes POSITIVE
The protons are in greater number
An ion that gains electrons becomes NEGATIVE
The electrons are in greater number

3. Losing Valence electrons
Example- Na
Sodium has 1 valence electron because it is in Group 1
If it loses that 1 electron then it would have 10 electrons which is the same as Neon
Neon is a Noble gas so it has 8 valence electrons and is chemically stable
Metals give up electrons

4. Gaining valence electrons
Non metals are both good at sharing electrons and receiving them from Metals
Example- Cl has 7 valence electrons
It just needs 1 more to become stable and have 8.
Na can give it 1 so that it can be like Argon- a noble gas
Na becomes Na¹ and Cl becomes Cl¹¯

5. Determining an ions charge
To determine the charge on an ion
Subtract the number of electrons from the number of protons

6. Ionic bonds Metals lose electrons to non metals
Metals become positively charged and the non metal becomes negatively charged
These ions attract each other to form an ionic compound and an ionic bond
The attraction between positively and negatively charged ions in an ionic compound is an Ionic bound.

7. Characteristics of ionic compounds
Solid and brittle at room temperature
Relatively high boiling and melting points
Usually dissolve in water to become a good conductor of electricity

8. Metallic bonds Metal atoms can bond to other metal atoms
They pool their valence electrons
A metallic bond is formed when many metal atoms share their pooled valence electrons

9. Properties of Metallic bonds
Good conductors of thermal energy and electricity
Can be hammered into sheets because the electrons can slide over each other
Shiny because the valence electrons reflect light