Outline of Topics
1. REVIEW
Ions, Ionic Compounds
2. Naming Ionic Compounds
3. Properties of Ionic Compounds
4. Naming Covalent Compounds
5. VSEPR
REVIEW of IONS
OBJECTIVE: When atoms give
away electrons
IONS
ION
What is it?
An atom that
LOST/GAINED
electron(s)
IONS
Goal is to get to the NEAREST
Noble Gas
RULES
1. If you go LEFT, you become
POSITIVE.
2. If you go RIGHT, you become
NEGATIVE
IONS
Ions that LOSE
electrons have a
POSTIVE charge
called
cations
pronounced “cat – ions”
IONS
All metals become
CATIONS
IONS
USE HALF SHEET FOR TRANSITION METALS
IONS
Ions that GAINS
electrons have
a NEGATIVE
charge
called
anions
pronounced “an – ions”
IONS
Some ions are made from two or more atoms
Ex: CNNH4+
CO32Because these ions are made from two or
more atoms, they are called
polyatomic ions
IONS
-ite has less oxygen
than –ate
Memorize? Kind of
IONS
Summary & Review
1. What is an ion?
2. What are the two types of ions?
3. Which ions gains electrons: cations or anions?
4. Predict the charge of each atom if it were to
become an ion:
Ca, Cl, Cu, F, Fe, Li, Na, N, O
Ionic Compounds
OBJECTIVE: Joining Cations +
Anions to make compounds
Ionic Compounds
Na+ + Cl- 
NaCl
cation
anion
ionic compound
forumula
NaCl joined by
IONIC BOND
IONIC BOND = giving away/gaining
electrons
Ionic Compounds
Li+ + Cl-  LiCl
+
K + Cl- 
KCl
Ca2+ + Cl-  CaCl2
Li+ + O2-  Li2O
2+
2Ca + O  CaO
Charges must cancel and = 0
Ionic Compounds
+
Cu + CH3COO  CuCH3COO
+
NH4 + Cr2O7  NH4Cr2O7
2+
Mg
+ OH 
Mg(OH)2
Parenthesis for
POLYATOMIC
Ionic Compounds
Write formula for ionic compounds
Al3+ + O2- 
1.
2+
2. Fe + Cl 
3. Na+ + HCO3- 
4. Na+ + NO2- 
5. Ca2+ + PO43- 
6. H+ + SO42- 
7. Mg2+ + OH- 
8. NH4+ + PO43- 
Ionic Compounds
Write formula for ionic compounds
Al3+ + O2- 
1.
2+
2. Fe + Cl 
3. Na+ + HCO3- 
4. Na+ + NO2- 
5. Ca2+ + PO43- 
6. H+ + SO42- 
7. Mg2+ + OH- 
3+
8. Fe + Cl 
+
9. NH4 + PO43- 
1. Naming Ionic Compounds
Write from 1 to 5 in Roman Numerals
I
II
1. Naming Ionic Compounds
OBJECTIVE: Learn how to name
compounds like NaHCO3
1. Naming Ionic Compounds
First Name
+ Last Name =
Full Name
only
TRANSITION METALS
have roman numerals
Cations with Roman Numerals in BOLD
1. Naming Ionic Compounds
1. Start with
CATION, always
2. Name the anion using the suffix
“IDE”. If anion is polyatomic…
1. Naming Ionic Compounds
“uncross”
numbers to figure our
roman numeral for
cation
FeCl3 Cr2O3
Cu2O Mn3N2
Mn(NO2)3
Mn(NO3)3
Mn(NO3)2
If no numbers then
1. Figure out charge of
anion
FeO
MnO
CrO
CoN
CrPO4 ZnCrO7
CuSO4 CuNO3
1. Naming Ionic Compounds
1. Start with CATION, always
2. If cation is Transition Metal check
table for roman numerals
3. Name the anion using the suffix
“IDE”. If anion is polyatomic…
4. That’s it!
1. Naming Ionic Compounds
Writing formulas from names of ionic compounds
1. Write anion and charge.
-ATE
-ITE
half sheet
2. Write cation and charge.
3. Cross charges and write formula.
Naming Ionic Compounds
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
Sodium Chloride
Lithium Fluoride
Iron(II) Chloride
Sodium Nitrate
Magnesium Hydroxide
Sodium Acetate
Ammonium Chloride
Hydrogen Peroxide
Sodium Carbonate
Ammonium Phosphate
1. Naming Ionic Compounds
SUMMARY & REVIEW
Formula to Name
1. Start with cation
2. When to use roman numerals?
3. Then add…to anion
4. What about polyatomic ions?
Name to Formula
1. Start with anion – LAST NAME
2. What if anion ends in ATE or ITE?
3. Write symbol for cation – FIRST NAME
4. Roman numerals?
2. Properties of Ionic Compounds
What are some properties of salt?
2. Properties of Ionic Compounds
OBJECTIVE: Properties of salts
2. Properties of Ionic Compounds
Ionic compounds are
chemically joined by
IONIC BONDS
Ionic Bonds VERY STRONG!!
2. Properties of Ionic Compounds
Ionic compounds are generally called
SALTs
metal cation
+ non-metal anion
2. Properties of Ionic Compounds
Ionic Bonds
metal cation + non-metal anion
Ionic compounds are generally called
SALTs
2. Properties of Ionic Compounds
High boiling point = STRONG BONDS
2. Properties of Ionic Compounds
High boiling point = need lots of energy (heat) to break
ionic bond between cation and anion.
2. Properties of Ionic Compounds
Ionic Compounds
form crystals
2. Properties of Ionic Compounds
Ionic Compounds form crystals
Copper (II) sulfate
2. Properties of Ionic Compounds
Ionic Compounds
Brittle
(break, not bend)
2. Properties of Ionic Compounds
Ionic Compounds conducts electricity
Used to make
batteries
2. Properties of Ionic Compounds
conduct electricity
2. Properties of Ionic Compounds
2. Properties of Ionic Compounds
Mono Lake, CA
2. Properties of Ionic Compounds
Mono Lake, CA
2. Properties of Ionic Compounds
Mono Lake, CA
2. Properties of Ionic Compounds
Mono Lake, CA
2. Properties of Ionic Compounds
2. Properties of Ionic Compounds
Properties of Ionic Compounds
calcium carbonate
Properties of Ionic Compounds
calcium carbonate
2. Properties of Ionic Compounds
SUMMARY & REVIEW
1. Ionic compounds are generally called…
2. Ionic compounds have…
3. Ionic compounds forms
4. Ionic compounds are…
5. Ionic compounds can…
3. Naming Covalent Compounds
How many wheels on a bicycle?
How many wheels on a tricycle?
How many sides on a pentagon?
How many sides on a hexagon?
How many sides on an octagon?
3. Naming Covalent Compounds
OBJECTIVE: Learn how to name
compounds like H2O & CO2
3. Naming Covalent Compounds
Numbers MATTER!
CO
CO2
SO
SO2
3. Naming Covalent Compounds
FIRST ELEMENT
1. Name the element
2. If more than one, use prefix
NEVER used
3. “mono”
first name
SECOND ELEMENT
1. Name element
2. If more than one, use prefix
3. Add “IDE”
for
3. Naming Covalent Compounds
Name the compounds
1.CS2
2.NF3
3.SF6
4.CO
5.N2O3
3. Naming Covalent Compounds
Write the formula
1. Silicon tetrafluoride
2.Arsenic trichloride
3.Carbon dioxide
4.Boron tribromide
5.Dihydrogen monoxide
3. Naming Covalent Compounds
How to know if compound is
ionic or covalent?
IONIC: between metal and non-metal
COVALENT: between non-metals
3. Naming Covalent Compounds
IONIC: RED + BLUE
COVALENT: YELLOW/BLUE + BLUE
Covalent Compound Calculations
A. Name each compound/write formula
1. BF3
2. BrCl
3. IF4
4. SF6
5. carbon dioxide
6. boron tribromide
7. oxygen difluoride
8. xenon tetrafluoride
Properties of Covalent Bonds
2 types of covalent bonds
Polar
Electron shared UNEQUALLY
Non-Polar
Electrons shared EQUALLY
Properties of Covalent Bonds
Polar Covalent
have dipoles
Properties of Covalent Bonds
Bond Type Determines Properties of Things
Properties of Covalent Bonds
3. Namine Covalent Compounds
Summary & Review
1. How can you tell the difference
between ionic and covalent compounds
2. How is hydrogen different?
3. Namine Covalent Compounds
Summary & Review
1. How can you tell the difference
between ionic and covalent compounds
2. Name/write formula for the following
1. P4S5
2. SeF6
3. Si2Br6
4. SCl4
5. B2Si
6. antimony tribromide
7. hexaboron silicide
8. chlorine dioxide
9. hydrogen iodide
10. iodine pentafluoride
3. Namine Covalent Compounds
1. P4S5
2. SeF6
3. Si2Br6
4. SCl4
5. B2Si
6. antimony tribromide
7. hexaboron silicide
8. chlorine dioxide
9. hydrogen tri-iodide
10. iodine pentafluoride
4. Lewis Structures
OBJECTIVE:
How bonds are made
4. Lewis Structures
Most elements want
8 valence electrons
Octet Rule
4. Lewis Structures
dot = valence electron
4. Lewis Structures
blue line = bond
4. Lewis Structures
1. Write elements
2. Count total number of valence e
3. LEAST electronegative is in the
center (usually CARBON)
4. Draw bond
5. Then draw dots until you run out
6. Make double/triple bonds if
necessary
4. Lewis Dot Structures
Exceptions to the Octet Rule
1. Less than 8
2. More than 8
3. Polyatomic Ions
4. Lewis Dot Structures
Exceptions to the Octet Rule
1. Less than 8
Hydrogen
Beryllium and Boron
BeCl2
BCl3
4. Lewis Dot Structures
Exceptions to the Octet Rule
2. More than 8
Phosphorus ,Sulfur, Chlorine
Xenon
PCl5 SF6 XeF4
4. Lewis Dot Structures
Exceptions to the Octet Rule
3. Polyatomic Ions
Cations
Anions
SUBTRACT
electrons
add brackets
ADD
electrons
[ ]
4. Lewis Dot Structures
Resonance = 2 or more
possible Lewis Dot Structures
4. Lewis Dot Structures
Resonance = 2 or more
possible Lewis Dot
Structures
4. Lewis Structures
Summary & Review
1. Which elements have less
than 8?
2.Which elements have more
than 8?
4. Lewis Structures
Summary & Review
1. Which element goes in the middle of a
Lewis Structure?
2. Which is NEVER in the center?
3. Which elements do not need 8 dots?
4. Which elements can have more than 8?
5. What do you add to non polyatomic ions?
6. What is a resonance?
5. VSPER
1. Draw a triangle
2. Draw a square
3. Draw a pyramid
5. VSPER
OBJECTIVE:
Lewis Structures
in
3D
5. VSPER
How to determine shape?
VSEPR
Valence Shell Electron Pair
Repulsion
5. VSPER
How is VSEPR different from Lewis?
VSEPR
Lewis
Lewis in
3D
shows
bonds
5. VSPER
5 main shapes
Linear
5. VSPER
Triagonal Planar
5. VSPER
Tetrahedral
5. VSPER
Triagonal bipyramidal
5. VSPER
Octahedral
5. VSPER
More shapes derived from the
5 main ones
5. VSPER
5. VSPER
5. VSPER
5. VSPER
5. VSPER
5. VSPER
Bent
5. VSPER
Triagonal Pyramidal
5. VSPER
T-shape
5. VSPER
Seesaw
5. VSPER
Square Pyramidal
5. VSPER
Square Planar
5. VSPER
How to determine shape??
1. Draw Lewis Structure
2. Count how many THINGS around
the center atom?
3. How many LONE PAIRS?
4. Axial & Equatorial
5. VSPER
VSEPR
Main Idea:
Electrons around atoms
REPEL each other
5. VSPER
Determine shape by
1. Draw Lewis Structure
2. Add marshmallows around the center
3. Remove marshmallow that represent lone pairs
IMPORTANT
Things like:
charges, single, double, triple bonds
do
NOT matter
5. VSPER
Summary & Review
1. What is the main idea of VSEPR
2. How is VSEPR different from Lewis Structures
3. How do you determine the VSEPR shape?
Sample Problem
Charles Goodyear accidently created rubber
by heating atoms of carbon and sulfur
together. The resulting covalent compound
is named carbon disulfide. This covalent
compound is extremely useful because of its
elastic ability.
A. What is the formula for this compound?
B. Draw the Lewis Structure for this
compound.
C. What is the VSEPR shape?