Pre-AP Chemistry
Ionic Bonding Review Sheet
 PART 1: IONIC BONDING THEORY
- Chemical Bond: force holding two atoms together.
- Valence electrons participate in bonding.
- Atoms form ions by losing or gaining electrons. The number of electrons lost or gained depends
on the octet rule (=8 valence electrons). 1-3 valence electrons will lose electrons while 5-7
valence electrons will gain elections.
- Ionic bonding occurs between a metal (cation) and nonmetal (anion) and forms compounds.
- Electrostatic force holding two opposite charges together is an ionic bond.
- The total oxidation state (charge) of a compound is zero.
- Ionic compounds have high melting and boiling points (greater than room temperature) and can
conduct electricity (when aqueous).
- Ionic compounds adopt a low energy, stable crystal lattice structure.
- Lattice energy: amount of energy required to separate ions of an ionic compound (or separate
the crystalline solid into a gas).
- Ionic bond formation is overall exothermic (releases energy). Cation formation is endothermic,
anion formation is exothermic, and lattice formation is exothermic.
- Organizing Ideas:
Intramolecular
Force
Ionic
Compounds
Electrons
Transferred
Crystal Lattice
Structure
Exothermic
Overall
Electrostatic
Interaction
Metal
Nonmetal
Cation
Anion
Octet Rule
Noble gas
electron config.
Page 1 of 3
Stability
 PART 2: NOMENCLATURE
Type I: Ionic Bonding with FIXED oxidation states (charge)
-
How to identify: Metal is in the main groups (Group 1, 2, 3) and Ag+, Zn2+, Cd2+
-
SYMBOL  NAME
1) Write full name of the metal/cation.
2) Write name of the nonmental/anion with –ide ending.
-
NAME  SYMBOL
1) Write symbol for the metal/cation.
2) Write symbol for the nonmetal/anion.
3) Use the charge from the periodic table (based on element’s group #) to determine the
subscripts of the metal and nonmetal to give an overall charge of zero (pos = neg).
-
Examples:
1) Na2S
2) Calcium fluoride
sodium sulfide
CaF2
Type II: Ionic Bonding with VARIABLE oxidation states (charge)
-
How to identify: Metal is a transition metal except Ag, Zn, Cd
-
SYMBOL  NAME
1) Write full name of the metal/cation.
2) Write name of the nonmental/anion with –ide ending.
3) Use the fixed charge of the anion (from the periodic table) to determine the total
positive charge to give an overall compound charge of zero.
4) Divide the overall positive charge by the number of metal atoms to determine the
charge of EACH metal atom. Write this number as a Roman Numeral between the metal
and nonmetal in the chemical name.
-
NAME  SYMBOL
1) Write symbol for the metal/cation.
2) Write symbol for the nonmetal/anion.
3) The charge of the EACH metal cation comes from the Roman Numeral in the given
name.
4) The charge of the anion comes from the periodic table.
5) Determine the subscripts of the metal and nonmetal to give an overall charge of zero
(pos = neg).
Page 2 of 3
-
Examples:
1) Sn3P4
2) Cobalt(II) nitride
tin(IV) phosphide
Co3N2
Type III: Ionic Bonding with Polyatomic Ions
-
-
How to identify: A polyatomic ion will be present in the name or formula.
The list of polyatomic ions on Page 257 (textbook) MUST be memorized (name, formula, charge)
Consider the polyatomic ion as one large unit that does not change
NEVER touch or change the polyatomic ion --- use parentheses to denote multiple quantities
The charge of a polyatomic ion is the charge for the WHOLE unit/group of atoms. The sulfate ion
(SO42-) has a charge of 2- on the entire sulfate molecule…one SO4 has a charge of 2-.
Do NOT change the ending of the polyatomic anion to an –ide ending. Write the full name of the
ion.
1) If the metal/cation has a fixed charge, follow rules for Type I (except do not use –ide
ending).
2) If metal/cation has a variable charge, follow rules for Type II (except do not use –ide
ending.)
Examples:
1) Mn3(PO4)7
2) Barium acetate
permanganate(VII) phosphate
Ba(C2H3O2)2
Page 3 of 3