Name_______________________
Objectives:
 Define and describe the properties of ionic, covalent, and metallic bonds.
 Identify the number of valence electrons for a main group element and relate this to the charge
formed for an ion.
 Describe how ionic and covalent bonds form through Lewis dot structures.
 Follow rules to name and identify ionic and covalent compounds correctly.
I. Introduction:
A. What is a bond?
B. How do bonds form?
C. Terms:
a. Energy Levels:
b. Valence electrons:
D. ATOM PICTURES
1. Hydrogen
3. Lithium
2. Helium
4. Beryllium
**Why are valence electrons important?
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Name_______________________
II. Lewis Structures:
A. What is a Lewis structure?
B. Basic notation:
C. How to find the number of valence electrons for main group elements:
Column #
1
Valence Electrons
D. Examples:
Element
# of valence
electrons
Hydrogen
2
Transition
Metals
(vary – will be
given)
Lewis Dot
Structure
13
Element
14
15
# of valence
electrons
16
17
Lewis Dot
Structure
Aluminum
Helium
Chlorine
Sodium
Oxygen
Carbon
Krypton
Why do elements form compounds?
Octet Rule:
**All elements want a _______________________ and be like a _______________________.
2
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III. Ionic Bonds:
A. Terms:
a. Ion:
b. Cation:
c. Anion:
d. Lewis structure to ion:
Element
Lewis structure
Gain/Lose?
How many?
Charge
Lithium
Sodium
Magnesium
Calcium
Oxygen
Sulfur
Fluorine
Chlorine
B. Properties of ionic bonds:
3
Metal/Nonmetal?
Cation/Anion?
Name_______________________
C. Forming Ionic Bonds:
1) GOAL:
2) Metals ______________ electrons to become like ____________________.
3) Nonmetals ______________ electrons to become like ____________________.
4) Each element wants a ______________________________________________.
5) Lewis structure examples:
Metal Lewis
Elements
Structure
Nonmetal
Lewis Structure
Ionic Bond
Lithium and
Bromine
Calcium and
Oxygen
Sodium and
Oxygen
6) Charge examples:
Elements
Metal Charge
Nonmetal
Charge
Lithium and
Bromine
Calcium and
Oxygen
Sodium and
Oxygen
4
Ionic Bond
Name_______________________
D. Naming Ionic Compounds:
a. RULES FOR NAME (words) TO FORMULA (symbols)
1.
2.
3.
b. EXAMPLES
1. Sodium chloride
2. Iron (III) oxide
3. Potassium oxide
4. Tin (IV) selenide
5. Aluminum sulfide
c. RULES FOR FORMULA (symbols) TO NAME (words)
1.
a.
2.
a.
d. EXAMPLES
1. NaF
2. MgO
3. CaCl2
4. CuBr2
5. Al2O3
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Name_______________________
E. Naming with Polyatomic Ions
a. Polyatomic Ion:
b. Follow rules for naming ionic compounds; be aware that compounds with polyatomic ions will
have more than 2 elements.
c. Examples:
Name to Formula:
1. Sodium hydroxide
2. Calcium phosphate
3. sodium carbonate
4. Aluminum nitrate
5. Calcium hydroxide
Formula to Name:
1. KMnO4
2. NaCH3COO
3. Al2(SO4)3
4. Ca(CN)2
5. NaOH
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Name_______________________
IV. Covalent Bonds:
A. Terms:
a. Polar:
b. Nonpolar:
c. Review: Remember – like dissolves like
B. Properties of covalent bonds:
C. Forming Covalent Bonds:
1) GOAL:
2) Exceptions to Octet Rule:
H: only wants 2eS&P: can have more than 8eB: only wants 6e
3) Using Lewis dot structures for drawing covalent compounds
total valence
Molecule
Lewis Structure
electrons
H2O
(water)
CF4
(carbon tetrafluoride)
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Name_______________________
D. Naming Covalent Compounds
Number
Prefix
1
Mono-
2
Di-
3
Tri-
4
Tetra-
5
Penta-
6
Hexa-
7
Hepta-
8
Octa-
9
Nona-
10
Deca-
Greek Prefixes (Starters)
Other uses for these prefixes
a. RULES FOR NAME TO FORMULA
1.
2.
3.
4.
b. EXAMPLES
1. Nitrogen tribromide
2. Dinitrogen trisulfide
3. Carbon monoxide
4. Tetraphosphorus decoxide
5. Carbon tetrahydride
6. Diboron hexahydride
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Name_______________________
c. RULES FOR FORMULA TO NAME
1.
a.
b.
2.
a.
b.
d. EXAMPLES
1. CO2
2. H2O
3. P2O5
4. CCl4
5. CF4
REVIEW:
Describe each type of bond shown in the picture below:
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Name_______________________
V. Metallic:
A. Properties:
VI. Examples
a. Classify the following compounds as having Ionic (I), Covalent (C), or Metallic (M) bond.
1) CuCl2
________
2) CO2
________
3) Ag
________
4) NaCl
________
5) O2
________
6) Fe2O3
________
7) H2O
________
8) Na
________
9) CaF2
________
10) H2
________
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