1. Ionic Bonding and Naming

2. What do we already know?
Protons determine the IDENTINTY of the element
Valance Electrons determine the CHEMICAL properties of an element.
Valance electrons are the electrons in the OUTER ENERGY level
For representative elements look at the group number to determine the number of valance electrons
Elements lose or gain electrons to achieve a full outer energy level (full OCTET)
Metals form CATIONS by losing electrons
Nonmetals form ANIONS by gaining electrons

3. The Octet Rule
Octet rule stated that in forming compounds atoms tend to achieve the electron configuration of a noble gas.
An octet is a set of eight electrons
Atoms of metals tend to lose their valence electrons leaving a complete octet in the next-lowest energy level.
Atoms of some nonmetals tend to gain electrons or to share electrons with another nonmetals to achieve a complete octet.

4. Lewis Structure
Electron dot structures (Lewis dot structure) are diagram that show the valence electrons at dots.
Each valance electron is represented with a dot
Put one dot on each side of the symbol before putting two on one side.
Examples
Carbon
Calcium
Chlorine
Argon
4 valance e-
2 valance e-
7 valance e-
8 valance e- C Ca Cl Ar

5. Formation of Ionic Compounds
Ionic compounds are compounds composed of cations and anions.
Although they are compounds of ions, ionic compounds are electrically neutral.
Ionic bonds are the electrostatic forces that hold ions together in ionic compounds. They occur due to the transfer of electrons
Chemical formula shows the kinds and numbers of atoms in the smallest representative unit of a substance.
Formula unit is the lowest whole-number ratio of ions in an ionic compound

6. Formula Writing
When writing formulas the MOST METALIC element is written first
Ionic bonds occur between METALS and NONMETALS so the metal is ALWAYS written FIRST.
Determine the ion that the elements will form
Balance charges
Can switch charges and reduce if necessary
Or can use the following equation:
# of metal x charge of metal + # of nonmetal x charge of nonmetal = 0
atoms atoms

7. Formula Writing Practice 1: Oxygen and Sodium
Sodium is metal so it MUST be written first
Na forms +1 ion and O forms -2 ion
Na+1 O-2 switching charges gives Na2O
(# metal) +1 +(#nonmetal) -2 = 0 solve
(2) +1 +(1) -2 = gives Na2O
NOTE: The subscript of 1 is NOT written
Practice 2: Nitrogen and Aluminum
Aluminum is metal so it MUST be written first
Al forms +3 ion and N forms -3 ion
Al+3 N-3 switching charges gives AlN (must reduce)
(# metal) +3 +(#nonmetal) -3 = 0 solve
(1) +3 +(1) -3 = gives AlN

8. Formula Writing Practice 3: Calcium and Carbon
Calcium is metal so it MUST be written first
Ca forms +2 ion and C forms -4 ion
Ca+2 C-4 switching charges gives Ca2C
(# metal) +2 +(#nonmetal) -4 = 0 solve
(2) +2 +(1) -4 = gives Ca2C
Practice 4: Barium and Phosphate (PO4-3)
Barium is metal so it MUST be written first
Ba forms +2 ion and PO4 is a -3 ion
Al+2 PO4-3 switching charges gives Al3(PO4)2
(# metal) +2 +(#nonmetal) -3 = 0 solve
(3) +2 +(2) -3 = gives Al3(PO4)2
MUST USE parenthesis to show having 2 phosphate molecules.

9. Ionic Naming – Type 1 metals
Type 1 metals are metals that form only 1 oxidation state.
They are found in groups 1, 2, & 13 in addition to Zn+2, Cd+2, and Ag+1
Determine the Cation and the Anion
If the cation is from a representative element write its name
The anion is a:
Polyatomic ion write it’s special name
Single nonmetal element write its root name followed by “ide”
write both parts of name side by side

10. Ionic Naming – Type 1 Example 1: Ca3N2 Example 1: Ca3(PO4)2
Calcium is the cation, nitrogen is anion
Calcium stays calcium
Nitrogen is NOT a polyatomic so it becomes Nitride
Ca3N2 is called calcium nitride
Example 1: Ca3(PO4)2
Calcium is the cation, phosphate is anion
Phosphate is a polyatomic so it’s name is phosphate
Ca3(PO4)2 is called calcium phosphate

11. Ionic Naming – Type 1 Practice KCl AlCl3 Ca2C InN Rb3PO3 Al(OH)3
In2(SO3)3
(NH4)3Br
Practice
Potassium chloride
Aluminum chloride
Calcium carbide
Indium nitride
Rubidium phosphite
Aluminum hydroxide
Indium sulfite
** Ammonium bromide

12. Ionic Naming – Type 2 metals
Most transition metals have the ability to borrow electrons from other orbitals and can form ions with different charges.
Metals in group 14 also have multiple oxidation states. +2 or +4
Example: Iron can from a +3 or +4 cation, copper can from a +2 or +1 ion
Not ALL transition metal do this but MOST do so when we name the compound we have to state the charge of the metal ion
EXCEPTIONS: three transition metals that you MUST memorize the following: Zn+2, Cd+2, Ag+1 as they do NOT need roman numerals

13. Ionic Naming – Type 2 Metals
Determine the Cation and the Anion
If the cation is from a transition element write its name followed by a roman numeral to show the charge of the metal ion.
The anion is a:
Polyatomic ion write it’s special name
Single nonmetal element write its root name followed by “ide”
write both parts of name side by side

14. Ionic Naming – Type 2 Common Roman numerals you MUST KNOW I 6. VI **
II VII
III VIII
IV ** 9. IX
V X
** commonly confused by students

15. Ionic Naming – Type 2 Example 1: FeO Example 2: Fe2O3
Fe is cation and O is anion
since Oxygen has a -2 charge Fe MUST have a +2 so it is Iron (II)
O is NOT a polyatomic so it becomes Oxide
FeO is Iron (II) Oxide
Example 2: Fe2O3
since Oxygen has a -2 charge Fe MUST have a +3 so it is Iron (III)
FeO is Iron (III) Oxide

16. Ionic Naming – Type 2 Example 3: FePO4 Example 4: Ag2O
Fe is cation and PO4 is anion
since PO4 has a -3 charge Fe MUST have a +3 so it is Iron (III)
PO4 is a polyatomic so it is phosphate
FeO is Iron (III) Phosphate
Example 4: Ag2O
Ag is cation and O is anion
Ag is an exception and only forms a +1 ion so is Silver
O is NOT a polyatomic so it becomes Oxide
Ag2O is Sliver Oxide
Remember Zn+2, Cd+2, Ag+1 do NOT need roman numerals

17. Ionic Names to formula
Use the name to determine the ions of the elements (or polyatomic) in compound
Write the ions for each element
Balance charges using either method(reduce if necessary)
Chemical formulas for COMPOUNDS do NOT have charges!!
The number of atoms MUST be shown as a subscript.
REMEMBER the size and the shape of the letters matter when writing chemical formulas: COS and CoS are two different things

18. Ionic Names to Formulas
Examples
Zinc Oxide
Zn+1 O-2
Zn2O
Cobalt (II) Oxide
Co+2 O-2
CoO
Manganese (IV) Sulfate
Mn+4 S-2
MnS2
Examples
Strontium Sulfide
Sr+2 S-2
SrS
Magnesium Cyanide
Mg CN-1
Mg(CN)2
Potassium Phosphide
K+1 P+3
K3P

19. Formation of Ionic Compounds
Metals lose their electrons to nonmetals
The opposite charges attract and form an ionic bond
Na Cl →Na Cl →Na Cl → NaCl
name is: sodium chloride
Mg + S →Mg + S →Mg S-2 → MgS
name is: Magnesium Sulfide

20. Properties of Ionic Compounds
Ionic compounds form by the TRANSFER of electrons
Most ionic compounds are crystalline solids at room temperature.
Ions in the crystals are arranged in repeating three-dimensional patterns.
The large attractive forces result in very stable structures
Ionic compounds generally have high melting points.
Ionic compounds can conduct an electric current when melted or dissolved in water
The ion movement allows electricity to flow between electrodes

22. Metallic Bonds and Metallic Properties
The valence electrons of metal atoms can be modeled as a sea of electrons.
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions.
the sea-of-electrons models explains many physical properties of metals
metals are good conductors of electric current because electrons can flow freely in them
metals are malleable (can be hammered or forced into shapes.)
metals are ductile (can be drawn into wires)

23. Alloys metal atoms are arranged in very compact and orderly patterns
alloys are mixtures composed of two or more elements, at least of one which is metal
alloys are important because their properties are superior to those of their components elements.
Bronze alloy is made of copper and iron
Steel alloys are made of iron and carbon with additional elements.