1. Ch. 7 Chemical Bonding

2. 7-1: Ionic Bonding
Ionic bond: occurs when a positively charged ion is attracted to a negatively charged ion.
In general, one atom takes electrons from another.
Ionic compound: composed entirely of ions
Cation: positively charged ion
Anion: negatively charged ion

3. Properties of Ionic Compounds
tend to dissolve in water
have high melting points due to strong bonds
are brittle
when molten (liquid), are good conductors

4. Octet Rule:
atoms tend to gain, lose or share electrons in order to acquire a full set of valence electrons
Lewis Dot Diagrams
Examples

5. Types of Ions Monatomic: have only one atom
If it is a cation, the name of the ion is the name of the atom.
Ex: Ca+2 = calcium ion
Transition metals can have more than one charge. If the cation is a transition metal, it will have a number to distinguish charge.
Ex: Fe can have a +2 or +3 charge, so ion names are iron (II) and iron (III)
If it is an anion it will end in –ide.
Ex: F-1 = fluoride (nor fluorine!)

6. Cations (fill in the missing info)
Atom
Ion Name
Ion
Rule #
Calcium
Ca+2 1
Lithium
Copper
Copper (I) 2
Cu+2
Iron
Iron (III)
Fe+3

7. Anions (fill in the missing info)
Atom
Ion Name
Ion
Rule
Oxygen
Oxide 3
Fluorine F-
S-2

8. Binary Ionic Compounds:
Form from the ions of only two elements.
To name them, just put the name of the cation and anion together.
Ex: BaCl2 = ions are barium and chloride, so the name is barium chloride
Ex: MnF2 = ions are manganese (II) and fluoride, so manganese (II) fluoride

9. Polyatomic Ions:
Ions that contain more than one atom

10. Polyatomic Ion Name
Ion symbol and charge
Ammonium
NH4+
Hydroxide
OH-
Acetate
C2H3O2-
Nitrate
NO3-
Carbonate
CO3-2
Sulfate
SO4-2
Phosphate
PO4-3
Hypochlorite
ClO-1
Bicarbonate
HCO3-

11. Naming using polyatomics
Again, just give the names of the ions
Ex: NH4Cl = ammonium and chloride, so ammonium chloride
Ex: MgSO4 = magnesium and sulfate, so magnesium sulfate
Ex: CuNO3 = copper (I) and nitrate, so copper (I) nitrate