1. Review: 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

2. Review: 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.
What is a compound?

3. Chemistry Chapter 5 & 6 I. Introduction to bonding

4. Bonding: A. vocabulary
Chemical Bond
attractive force between atoms or ions that binds them together as a unit
bonds form in order to…
decrease potential energy (PE)
increase stability

5. B. Types of Bonds IONIC COVALENT
Bond Formation
e- are transferred from metal to nonmetal
e- are shared between two nonmetals
Type of Structure
crystal lattice
true molecules
Physical
State
solid
liquid or gas
Melting
Point
high
low
Solubility in
Water
yes
usually not
Electrical Conductivity
yes (solution or liquid) no
Other
Properties
odorous

6. B. Types of Bonds METALLIC e- are delocalized among metal atoms
Bond Formation
e- are delocalized among metal atoms
Type of Structure
“electron sea”
Physical
State
solid
Melting
Point
very high
Solubility in
Water no
yes (any form)
Electrical Conductivity
Other
Properties
malleable, ductile, lustrous

7. C. Bond Polarity
Most bonds are a blend of ionic and covalent characteristics.
Difference in electronegativity determines bond type.

8. C. Bond Polarity Electronegativity
Attraction an atom has for a shared pair of electrons.
higher e-neg atom  -
lower e-neg atom +

9. C. Bond Polarity Electronegativity Trend (p. 151)
Increases up and to the right.

10. C. Bond Polarity Nonpolar Covalent Bond e- are shared equally
symmetrical e- density
usually identical atoms

11. + - C. Bond Polarity Polar Covalent Bond e- are shared unequally
asymmetrical e- density
results in partial charges (dipole) + -

12. C. Bond Polarity
Nonpolar
Polar
Ionic
View Bonding Animations.

13. C. Bond Polarity 3.0-3.0=0.0 Nonpolar 3.0-2.1=0.9 Polar 3.0-0.9=2.1
Examples:
Cl2
HCl
NaCl
=0.0
Nonpolar
=0.9
Polar
=2.1
Ionic

14. II. Ionic Bonding and Naming
Chapter 7 and 9

15. SC1 Students will analyze the nature of matter and its classifications.
SC1.b. Identify substances based on chemical and physical properties.
SC1.c. Predict formulas for stable ionic compounds (binary and tertiary) based on balance of charges.
SC1.d. Use IUPAC nomenclature for both chemical names and formulas:
SC1.d.1 Ionic compounds (Binary and tertiary)
SC1.d.3 Acidic compounds (Binary and tertiary)
SC3.e. Compare and contrast types of chemical bonds (i.e. ionic, covalent).
SC3.b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties.

16. Ionic Bonding and Naming A. Ionic Nomenclature
Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

17. Ionic Bonding and Naming A. Vocabulary
1 atom
2 or more atoms
Monatomic
Ion
Polyatomic
Ion
Na+
NO3-

18. Ionic Bonding and Naming A. Vocabulary
COMPOUND
more than 2
elements
2 elements
Binary
Compound
Ternary
Compound
NaCl
NaNO3

19. Ionic Bonding and Naming 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

20. Ionic Bonding and Naming B. 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

21. Ionic Bonding and Naming B. Lewis Structures
Ionic – show transfer of e-

22. Ionic Bonding and Naming D. 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
Overall charge must equal zero.
If charges cancel, just write symbols.
If not, use subscripts to balance charges.
Use parentheses to show more than one polyatomic ion.
Stock System - Roman numerals indicate the ion’s charge.

23. Ionic Bonding and Naming D. 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

24. Ionic Bonding and Naming D. 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.

25. Ionic Bonding and Naming E. Ionic Nomenclature
Ionic Names
Write the names of both ions, cation first.
Change ending of monatomic ions to -ide.
Polyatomic ions have special names.
Stock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

26. Ionic Bonding and Naming E. Ionic Nomenclature
Consider the following:
Does it contain a polyatomic ion?
-ide, 2 elements  no
-ate, -ite, 3+ elements  yes
Does it contain a Roman numeral?
Check the table for metals not in Groups 1 or 2.
No prefixes!

27. Ionic Bonding and Naming E. Ionic Nomenclature
Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

28. Ionic Bonding and Naming E. Ionic Nomenclature
potassium chloride
magnesium nitrate
copper(II) chloride
K+ Cl-
 KCl
Mg2+ NO3-
 Mg(NO3)2
Cu2+ Cl-
 CuCl2

29. Ionic Bonding and Naming E. Ionic Nomenclature
NaBr
Na2CO3
FeCl3
sodium bromide
sodium carbonate
iron(III) chloride

30. 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:
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

31. 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

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

33. 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

34. 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

35. 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

36. 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

37. 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

38. C. Ionic Nomenclature Ionic Formulas
Write each ion, cation first. Don’t show charges in the final formula.
Overall charge must equal zero.
If charges cancel, just write symbols.
If not, use subscripts to balance charges.
Use parentheses to show more than one polyatomic ion.
Stock System - Roman numerals indicate the ion’s charge.

39. 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

40. 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

41. 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

42. 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

44. 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)

45. 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.