Outline of Topics
1.
Naming Ionic Compounds
2.
Properties of Ionic Compounds
3.
Naming Covalent Compounds

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 NaHCO
3

1. Naming Ionic Compounds
First Name + Last Name = Full Name

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
FeCl
3
Cu
2
O Mn
3
Mn(NO
2
Mn(NO
3
Mn(NO
3
Cr
2
O
3
)
)
3
)
3
2
N
2
If no numbers then
1.
Figure out charge of anion
FeO CrO
MnO CoN
Cr PO
4
Cu SO
4
Zn CrO
7
Cu NO
3

1. Naming Ionic Compounds
1.
2.
3.
4.
“
Start with
If cation is Transition Metal check table for roman numerals
Name the anion using the suffix
IDE
CATION , always
”. If anion is polyatomic…
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
5.
6.
7.
8.
1.
2.
3.
4.
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?
3.
2.
1.
Name to Formula
Start with anion – LAST NAME
What if anion ends in ATE or ITE ?
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
1.
SUMMARY & REVIEW
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 H
2
O & CO
2

3. Naming Covalent Compounds
Numbers MATTER!
CO
CO
2
SO
SO
2

3. Naming Covalent Compounds
FIRST ELEMENT
1.
2.
Name the element
If more than one, use prefix
3.
“mono”
used first name
SECOND ELEMENT
1.
2.
Name element
If more than one, use prefix
3.
Add “
IDE
” for

3. Naming Covalent Compounds
Name the compounds
1.
2.
3.
4.
5.
2
2
3
6
3

3. Naming Covalent Compounds
Write the formula
1.
2.
Silicon tetra fluoride
Arsenic tri chloride
3.
4.
5.
Di hydrogen mon oxide

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

1.
2.
3.
4.
BF
3
BrCl
IF
SF
4
6
Covalent Compound Calculations
A.
Name each compound/write formula
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 shared

Properties of Covalent Bonds
Bond Type Determines Properties of Things

Properties of Covalent Bonds

3. Namine Covalent Compounds
1.
Summary & Review
How can you tell the difference between ionic and covalent compounds
1.
2.
3.
4.
5.
2.
P
4
S
SeF
5
Si
2
6
Br
6
SCl
4
B
2
Si
Name/write formula for the following
5. antimony tribromide
6. hexaboron silicide
7. chlorine dioxide
8. hydrogen iodide
9. iodine pentafluoride

4. Lewis Structures
OBJECTIVE:
How bonds are made

4. Lewis Structures
Most elements want
8 valence electrons

4. Lewis Structures

4. Lewis Structures

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 Structures
Elements that do not want 8 dots
H, Li, Na, K, etc.
Only wants
more exceptions later

4. Lewis Dot Structures
Exceptions to the Octet Rule
1. Less than 8
Group 1 &
Beryllium and Boron
BeCl
2
BCl
3

4. Lewis Dot Structures
Exceptions to the Octet Rule
2. More than 8
Phosphorus ,Sulfur and
PCl
5
Xenon
SF
6
XeF
4

4. Lewis Dot Structures
Exceptions to the Octet Rule
3. Polyatomic Ions
Cations Anions
SUBTRACT electrons add brackets
[ ]
ADD electrons

4. Lewis Dot Structures

4. Lewis Dot Structures

4. Lewis Structures
Summary & Review
1.
2.
Which element goes in the middle of a
Lewis Structure?
Which is NEVER in the center?
3.
Which elements do not need 8 dots?
4.
Which elements can have more than 8?
5.
6.
What do you add to polyatomic ions?
What is a resonance?

4. Lewis Dot Structures
Draw Lewis Structures and name the compounds
Print HO that classifies LS by # of Bonds
Create it as an assignment, the use it to have the students classify the VSEPR next

5. VSPER
3D

5. VSPER

5. VSPER
How is VSEPR different from Lewis?

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER
More shapes derived from the
5 main ones

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER

5. VSPER
T-shape

5. VSPER

5. VSPER
Square Pyramidal

5. VSPER

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

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
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.
B.
C.
What is the formula for this compound?
Draw the Lewis Structure for this compound.
What is the VSEPR shape?