1. Chemistry
Chapter 8
Notes #2

2. Ionic Bonding/terms
Anions and cations are held together by opposite charges.
Many ionic compounds are referred to as salts or oxides.
Simplest ratio of elements in an ionic compound is called the formula unit.
The bond is formed through the transfer of electrons.
Electrons are transferred to achieve noble gas configuration.

3. Ionic Bonding Cation + Anion Formula Units (instead of molecules)
The cation is always written first
Formula Units (instead of molecules)
The ions come together to neutralize the charge (always have an overall charge of zero)
Structure: Positive ions are surrounded by negatives and vice versa

4. Ionic Bonding Na Cl
The metal (sodium) tends to lose its one electron from the outer level.
The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.

5. Ionic Bonding
Na+
Cl -
Note: Remember that NO DOTS are now shown for the cation!

7. Ionic Bonding
Lets do an example by combining calcium and phosphorus: Ca P
All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable).

8. Ionic Bonding Ca P

9. Ionic Bonding
Ca2+ P

10. Ionic Bonding
Ca2+ P Ca

11. Ionic Bonding
Ca2+
P 3- Ca P

12. Ionic Bonding
Ca2+
P 3- Ca

13. Ionic Bonding
Ca2+
P 3-
Ca2+ P

14. Ionic Bonding Ca
Ca2+
P 3-
Ca2+ P

15. Ionic Bonding Ca
Ca2+
P 3-
Ca2+ P

16. Ionic Bonding
Ca2+
Ca2+
P 3-
Ca2+
P 3-

17. = Ca3P2 Ionic Bonding Formula Unit
This is a chemical formula, which shows the kinds and numbers of atoms in the smallest representative particle of the substance.
For an ionic compound, the smallest representative particle is called a: Formula Unit

18. Naming Compounds Name Cation first, anion second
Monatomic cation – name of element
Monatomic anions – drop ending, add –ide
Ex. Oxygen = oxide
Polyatomic ions = name of polyatomic
Transition metals – the oxidation number is written as a roman numeral

19. Examples Sodium Chloride Magnesium Fluoride Potassium Nitride
Iron (III) oxide
Ammonium Sulfide
Lithium Carbonate
Strontium Phosphate
FeO
Fe2O3

20. Ionic Properties Ionic crystal = crystal lattice High melting points
3-dimensional geometric pattern of particles
High melting points
High boiling points
Hard, rigid, and brittle
Due to the high strength of the bonds
Energy to separate ions (1 mole) = lattice energy