Chapter 7, 8, and 9
Chemical Bond

Types of Bonds


o
o

Octet Rule

Atoms tend to lose or gain electrons to obtain the same electron configuration as a noble gas
Ions

Cations
o
o
o

Anions
o
o
o
Ionic Bonds (also known as

)
Electrons are _________________________________
o
o
o
The attractive forces (
)

Form between

A transfer of electrons
Properties of Ionic Compounds



Metallic Bonds

Electrons move through the substance with little restriction


o
Sea of electrons -
Properties of Metals



Chapter 9
Naming Ionic Compounds

Let’s recall

Charged particles (Ions)
o
Monatomic -
o
Polyatomic-
Monatomic Ions

A single atom that has acquired a charge by losing or gaining one or more electrons
o
o
o
o

Monatomic ions that are multivalent
o
o
o

Example:








o
A couple of exceptions (multivalent)

Silver

Zinc

Scandium

Cadmium
Naming Monatomic Ions
Chapter 8 Covalent Bonding
 Molecule –
 Electrons
 Electron pairs form a bond
 Both atoms achieve an octet in their outermost orbital
 Covalent bonds generally
 They are formed by
 Covalent compounds



 When two or more atoms bond covalently, they are called a_______________________
 Two types of covalent bonding:
o
Polar covalent –

o
Nonpolar covalent –

 Ionic or Covalent?
o
How can we determine which type of bond will form between atoms?
o
By the ________________________________of each atom


How to determine the bond type?
• Subtract
•
IONIC BOND
▫
(values differ depending on the reference, for example, 1.6 to 2.0)
•
COVALENT BOND
▫
▫
Two types of covalent:
•
•
Polarity
• Polar covalent bond
▫
▫
The more electronegative atom acquires a
▫
The less electronegative atom acquires a
+ -
▫
Example: H – Cl
or
H – Cl
•
Nonpolar covalent bond
▫
▫
Electronegativity difference =
▫
Example
H-H
Explanation of Polarity including examples:
•
Cl2
•
H2O
•
** Remember --Polar Covalent a bond formed by an unequal sharing of a pair of electrons
Bond Strength
Electronegativity Difference
Bond
C – Cl
H – Br
Cl – Cl
Ca – Cl
Diatomic Molecules
•
Diatomic Molecule –
•
Gases that exist as diatomic molecules:
▫
▫
▫
The big 7 on the periodic table
Molecular Formula
•
Bond Strength
Bond Type
How many covalent bonds can you have between atoms?
•
You can have up to three!!
Single Covalent Bonds
•
•
1 covalent bond =
** all halogens form______________________________________________
•
Unshared pair of electrons
o
Unshared pair –
o
Do not
o
Also known as a “____________________________” or a “___________________________”
•
•
Double and triple Bonds
•
Double Bonds
o
•
Triple Bonds
o
Chapter 9 – Naming Covalent Compounds
Covalent Compounds
•
Binary
o
The first element is named with ________________________________________
o
The second element is ________________________________________________
o
Prefixes ____________________________________________________________
Prefixes
•
Mono is
▫
•
Examples:

CO

CO2
If the prefix ends in a vowel and the element starts with a vowel drop the last vowel from the prefix
▫
Example:

N2O5
Writing Formulas
•
▫
Example:
▫
Boron Trifluoride =
Acids

Know your ions and acids are easy
•
Don’t know your ions and acids are difficult
•
You can recognize an acid as its formula will begin with an _____
•
Acids come in two types:
▫
▫
•
Rules of Naming Acids
1. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-. The stem of the
anion has the suffix –ic and followed by the name acid.
2. When the anion ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by
the word acid.
3. When the anion ends in –ate, the acid name is the stem of the anion with the suffix –ic, followed by the
word acid.
•
Examples: Always begin Hydro and end –ic acid
•
EXAMPLES
▫
HF=
▫
HCl =
▫
HBr=
▫
H2SO4 =
▫
H3PO4 =
▫
H2CO3 =
▫
HNO3 =
▫
HC2H3O2=
Bases
•
Produces a
•
Write formulas and names same as ionic compounds
•
NaOH –