1. Ionic Bonding

2. Compounds on Earth.
All the compounds that exist on Earth are built from elements
118 elements are on the periodic table; only 80 commonly form compounds.
10 million known compounds; billions of possible compounds.
Figure 2.22: Hydrogen and carbon alone can be combined in millions of ways to make compounds with very different properties.

3. Discussion Questions Distinguish between elements and compounds.
Compare the number of elements with the number of compounds on Earth.

4. Ionic compounds are made of ions
Ionic compound: a compound made of oppositely charged ions – a bond between a metal and a non-metal.
Ions are held together with ionic bonds (a strong attraction between oppositely charged ions).
Ionic bonds are very strong.
ionic compound: a compound made of oppositely charged ions
ionic bond: a strong attraction that forms between oppositely charged ions

5. Ionic compounds are made of ions.
Binary ionic compounds:
Contain two elements - a metal and a non-metal.
Form when atoms of the metal element each lose one or more electrons to atoms of the non-metal element.
Results in the formation of ions that have full valence shells.
Full valence shell creates stability and that helps drive the formation of ionic compounds.

6. Sodium Chloride Example: Sodium chloride (salt)
Sodium (metal) reacts with chlorine (gas).
Forms when sodium atoms each transfer one electron to chlorine atoms.
Each sodium atom becomes positive ion (Na+).
Each chlorine atom becomes a negative ion (Cl−).

7. Sodium Chloride
Valence shells of both the sodium ion (Na+) and chlorine ion (Cl−) are full.
The stability of a full valence shell allows for the formation of ionic compounds.
Electrostatic attraction (forces) is the attraction between ions that have opposite charges and holds the ions together to form an ionic bond.

8. Lewis Dot Diagrams
Lewis Dot Diagrams is when we only examine/observe the valence shell of an element.
We can then easily see if the element will gain or lose an electron to produce an ion.
We use the Lewis Dot Diagrams to show how ionic bonds work.

9. Lewis Dot Diagrams

10. Na + Cl Na+ + Cl- NaCl Na+ + Cl- Lewis Dot Diagrams
Three steps to Lewis Dot Diagrams
1. Transfer of electrons.
2. Formation of cations and anions.
3. Formation of product. In our case the sodium ion combines with the chloride ion to produce sodium chloride.
Na + Cl
Na+ + Cl-
When an atom that tends to lose electrons is placed next to one that tends to gain electrons, the result is an electron transfer and the formation of to oppositely charged ions
All positive and negative charges must balance
NaCl
Na+ + Cl-

11. Lewis Dot Diagrams Draw Lewis Dot Diagrams for the following:
1. Lithium Bromide (LiBr)
2. Potassium Oxide (K2O)
3. Magnesium Nitride (Mg3N2)
4. Sodium Phosphide (Na3P)
5. Aluminum Chloride (AlCl3)

12. Structure of Ionic Compounds
Ionic compounds consist of positive and negative ions arranged in regular repeating patterns called lattices.
Example: Sodium chloride
Sodium chloride crystals consist of sodium and chloride ions arranged in a lattice.
Cubic structure of sodium chloride crystals.
Sodium chloride crystals consist of sodium and chloride ions arranged in a repeating pattern.

13. Properties of Ionic Compounds
Ionic compounds have high melting and boiling point
Melting requires breaking ionic bonds. That means you need to break the strong electrostatic forces that are holding the ions together in the lattice structure.
A large amount of energy is required to break ionic bonds.
Example: Melting point of sodium chloride is 801°C.

14. Properties of Ionic Compounds
Ionic compounds are hard and brittle.
Ionic solids are hard because ionic bonds are very strong.
When enough force is applied, ions will shift
This causes ions with the same charge to be close together.
Results in repulsive forces that break the solid apart.
When a force strong enough to overcome the strong forces of attraction between oppositely charged ions is applied, ions with like charges come close together. They repel one another and the solid cracks.

15. Properties of Ionic Compounds
Ionic compounds conduct electric current when in a liquid state or dissolved in liquid (aqueous solution)
Electric current: is the flow of charged particles.
Ionic compound in solid form: do not conduct electric current since ions are held rigidly in place.
Ionic Compound dissolved in liquid or in liquid form: ions are free to move and can conduct electric current.

16. Properties of Ionic Compounds

17. Assignment
Worksheet
differences