1. Chemical Bonding
Lesson 1 – Ionic Bonds & Compounds

2. Remember these??
They can be used to determine how atoms bond with each other.
Li: 1s2, 2s1
N: 1s2, 2s2, 2p3 Li N

3. The Octet Rule
Atoms are most stable when their outermost shell is full
Level 1 = 2 electrons
All other shells = 8 electrons
Noble gases have full outer shell so most do not bond with other atoms
Other atoms lose, gain, or share electrons to get a full outer shell

4. Ionic Bond * an electrostatic attraction between a cation and an anion
* electrons are lost by the cation
and gained by the anion
* usually involves a metal and a
nonmetal
* makes an ionic compound
animation

5. Metals lose electrons to get a stable outer shell (revert back to 8)
Nonmetals gain electrons to get a stable outer shell (add as many as needed until 8)
Ionic bond video

6. Properties of Ionic compounds
Most have high melting points and high boiling points.
Many dissolve in water (aqueous solution).
Good conductors of electricity (electrolyte) if melted (molten) or dissolved.
The greater the degree of ionization or dissociation the greater the conductivity of the solution

7. Form crystalline structures.
Ionic bonds are usually strong and stable. If stressed, the bonds will break along a cleave line.

8. Metal Cations Type I * metals whose ions can only have one possible
charge
Groups IA & IIA
Al, Ga, In, Zn, Cd, & Ag
* determine charge by position on the Periodic Table
IA = 1+; IIA = 2+
Al, Ga, and In = 3+; Zn & Cd = 2+; Ag = 1+

9. Type II * metals whose ions can have more than one possible charge
* Mostly transition (d-block) and
post transition metals

10. Polyatomic Ions * made of more than one atom.
* groups of atoms that travel together—never apart.
* The given charge is on the entire polyatomic ion—not on
individual atoms within the polyatomic ion.
A list can be found on page 7 of your reference packet. You are responsible for knowing:
ammonium (NH4+), cyanide (CN-), acetate (C2H3O2- or CH3COO-), nitrate (NO3-), nitrite (NO2-), hydroxide (OH-), carbonate (CO3 2-), sulfate (SO4 2-), sulfite (SO3 2-), and phosphate (PO4 3-)
You will have a quiz on the names, symbols and charges of these polyatomic ions.

11. Naming Ionic Compounds
* ALWAYS name the cation first and the anion second
* Cation – metal or polyatomic ion name
*** If the cation is a Type 2 metal, you must determine the charge of the metal and use that in the name***
* Anion – 1. if nonmetal change end of name to -ide
2. if polyatomic ion use the name

12. Name the following Potassium Chloride KCl NaCl MgO Sodium Chloride
Li3PO4
NH4Cl
Potassium Chloride
Sodium Chloride
Magnesium Oxide
Lithium Phosphate
Ammonium Chloride

13. Writing Formulas MgF2 Magnesium Fluoride Mg+2 F-1 F-1
Write the ions that make up the compound
Mg+2
F-1
Add ions as needed so the compound has a charge of zero
F-1
Write the number of each ion as a subscript and you have the formula
(DO NOT include charges & DO NOT write 1s)
MgF2
Simplest form = Formula unit

14. Zn(NO3)2 Zinc Nitrate Zn+2 NO3-1 NO3-1
Write the ions that make up the compound
Add ions as needed so the compound has a charge of zero
NO3-1
Write the number of each ion as a subscript and you have the formula
(DO NOT include charges & DO NOT write 1s)
*If you have more than 1 of a polyatomic ion,
you must put the ion in parenthesis*
Zn(NO3)2

15. Write the formula for the following
Calcium Oxide
Aluminum Chloride
Ammonium Nitrate
Ca O2-
CaO
Al Cl-
AlCl3
NH NO3-
NH4NO3

16. Copper (I) = Cu+ Copper (II) = Cu2+
When you have a Type II metal……
Type II metals are named like normal but with a Roman Numeral to indicate charge of the metal
Copper (I) = Cu+ Copper (II) = Cu2+
Name the following:
FeCl3
Each Chlorine has a charge of (-1). 3 chlorines would have a charge of (-3). To balance the compound to a charge of zero, Fe must have a charge of (+3); Iron (III)
Iron (III) Chloride

17. Name the following CuSO4 VCl5 Fe2O3 Cu?+ SO42- Copper (II) Sulfate
If there is one SO4 with a (-2) charge, the one Cu must have a (+2) to balance it
CuSO4
VCl5
Fe2O3
Cu?+ SO42-
Copper (II) Sulfate
If there are five Cl’s with a (-1) charge each, the one V must have a (+5) to balance the (-5) from Chlorine
V?+ Cl-
Vanadium (V) Chloride
Three O’s with a (-2) charge add up to -6. There are two Fe’s to cancel it out. Each Fe must have a (+3) to balance it.
Fe?+ O2-
Iron (III) Oxide