Ionic compounds are formed through ionic bonding between metals and nonmetals. Electrons are transferred from the metal atoms to the nonmetal atoms, resulting in cations with positive charges and anions with negative charges. The electrostatic forces between the oppositely charged ions hold the compound together in a crystalline lattice structure. Common polyatomic ions like nitrate, sulfate, and phosphate are also present in ionic compounds. Ionic compounds have properties like being solid at room temperature, having high melting points, and being good conductors of electricity when molten or dissolved in water.

1. Ionic Compounds
and Bonding

2. Ionic Bonding
Ionic Bonding occurs between metals
and nonmetals.
Electrons are transferred from the metal
atoms to the nonmetal atoms.
The driving force behind ionic bonds is
that cations (+ ion) give up electrons
and anions (- ions) accept electrons to
make Noble Gas Configurations

3. Ionic Bond Formation
Check your Bohr models to see how
many electrons an element will
want to lose or gain. Mark each
family.
The resulting electrostatic forces are
what hold the two ions together.
Total charges on an ionic
compound are equal but opposite.

4. Ionic Bonding

5. Ionic Bond Formation

6. Draw what happens
when sodium reacts with
chlorine to form sodium
chloride
DRAW THE DOT AND CROSS DIAGRAM TOO.

7. Naming Ionic Compounds
1. Always name the cation (positively charged ion)
first, the anion (negatively charged ion) second
2. Use the name of the cation without any
alterations.
3. Use the root and “-ide” to the end for anions
4. For the transition metals, use brackets and
Roman Numerals after the name to denote its
charge

8. Examples
LiI
BeBr2
Aluminum Sulfide
FeCl2
Iron (III) Chloride
Lithium Iodide
Beryllium Bromide
Al2S3
Iron (II) Chloride
FeCl3

9. Polyatomic Ions
Poly – Many Atomic - Atoms
Ions formed of multiple atoms usually covalently
bonded together and should be treated as one
entity.
Nitrate: NO3
-

10. Polyatomic Ions
Pb2+
+ 2 NO3
-
→ Pb(NO3)2
The brackets tell
us that
everything inside
is doubled.

11. Common Polyatomic Ions
NH4
+
Ammonium
CO3
2-
Carbonate
HCO3
-
Hydrogen carbonate (Bicarbonate)
PO4
3-
Phosphate
ClO2
-
Chlorite
ClO3
-
Chlorate
ClO4
-
Perchlorate
NO2
-
Nitrite
NO3
-
Nitrate
SO3
2-
Sulfite
SO4
2-
Sulfate
MnO4
-
Permanganate
OH-
Hydroxide

12. Try These
Iron (III) Nitrate
Al2(CO3)3
KOH
Silver (II) Sulfate
Calcium Bicarbonate
Fe(NO3)3
Aluminum Carbonate
Potassium Hydroxide
Ag2SO4
Ca(HCO3)2

13. Ionic Bonding
Properties:
Solids at room temperature
Due to strong electrostatic
interactions between the cation (+
ion) and anion (- ion).
Tend to have high melting points
Typically quite hard

14. Ionic Bonding
Properties (cont’d)
Poor conductors in solid state
The electrons are being taken up in the
bonding
Great conductors when molten or
aqueous
When the ions dissociate the electrons are
free to move and pass the charge

15. Ionic Bonding
Properties (cont’d)
 Most dissolve or dissociate nicely in water
 Water has partial charges that interact with
the ions’ charges

16. Interaction with water:
Click here to watch video.

17. Ionic Structure
Ionic compounds join together to
form Crystal Lattice Structures
The atoms arrange themselves in
such a way that gives the structure
stability

18. NaCl Crystal Lattice
(Simple Cubic)
NaCl Crystals

19. Determining the Crystal
Structure
 We use a technique called X-Ray
Crystallography
 X-rays are shot at a sample and will
bounce off the atoms in a specific
pattern according to how they’re
arranged.

20. Click to watch video.

21. Crystal Structures
A lot depends on the size of the ions.
Na+
is relatively small compared to
Cl-
so it can slip in between the Cl-
ions and form a simple cubic
structure.
Cs+
, however, is about the same size
as Cl-
so it’s more like packing ping-
pong balls.