CHAPTER 6
BONDS
Polyatomic ions
Name
Nitrate
Carbonate
Chromate
Acetate
Permanganate
Hydroxide
Sulfate
Chlorate
Phosphate
Ammonium
Symbol
NO3
CO3
CrO4
C2H3O2
MnO4
OH
SO4
ClO3
PO4
NH4
Flashcards-due Tomorrow-you can make them out
of cut paper if you don’t have index cards
Charge
-1
-2
-2
-1
-1
-1
-2
-1
-3
+1
Lewis DOT DIAGRAMS
A model of an
atom in which
each dot
represents a
valence eMax # of dots is 8
Li
He
Ne
C
X
DOT DIAGRAMS
Directions
Draw dot diagrams for the following elements.
1.
Hydrogen
2. Fluorine
On your paper
3. Tin
Name
1.
4. Sodium
5. Krypton
Dot Diagrams
CHEMICAL FORMULA
 Tells what elements a compound
contains & the ratio of those
elements.
 Ex: H2O
subscript- means “written below”
Tells how many atoms of that
element
superscript-means “written above”
Tells charge (oxidation #) of element
or compound
Ex: PO43- or PO4-3
Ex: List elements & give ratio
Your paper
Name
My paper
1. CuSO4
2. Li2S
11. Mg(OH)2
19. C2H5OH
Elements & ratios
1. CuSO4 =
2. Li2S =
11. Mg(OH)2 =
19. C2H5OH =
Answers
Ex: H2O = Hydrogen, Oxygen 2:1
Fe2O3 = Iron, Oxygen 2:3
Al(C2H3O2)3 = Aluminum, Carbon,
Hydrogen, Oxygen 1:6:9:6
HC2H3O2 = Hydrogen, Carbon,
Oxygen 1:2:3:2
Star questions
How many dots would Helium receive?
2
Define Chemical Formula
Tells what elements a compound contains & the
ratio of those elements.
Subscript means?
Written below
Superscript means?
Written above
CHEMICAL BONDS
Occur through interactions between the
valence electrons!!!
 Three major types of chemical
bonds:
1. Metallic
2. Ionic
3. Covalent
METALLIC BONDS
Metal + Metal = Metallic Bonds
“SEA of ELECTRONS”=valence e- are not
held tightly. They are freely moving or
swimming around the atom nucleus’ at all
times.
Forms a lattice
structure
METALLIC BONDS
Characteristics:
Malleable
Ductile
Ex: Aluminum foil: crumpling, wont
tear due to strong bonds!
More swimming electrons =
stronger bonds!
IONIC BONDS
 Formed when elements give
up or take e Formed between Metal &
NonMetal
IONIC BONDS
Protons no longer equal electrons!!
Particles formed by ionic bonds are
called ions (a charged atom)
Anion—An ion w/ a negative
charge (take e- , more negative)
Cation—An ion w/ a positive charge
(give up e-, more positive)
IONIC BONDS
EX:
Na + Cl = Na+Cl-
Na+ = Cation
Cl- = Anion
Write the purple words on your reference table!
Charge, AKA: Oxidation #
Group 1A
1 outer shell egives 1 e+1 charge
Group 2A
2 outer shell egives 2 e+2 charge
Group 3A
Group 4A
3 outer shell e-*special group
gives 3 ecan give, take
+3 charge
or share +/- 4
usually Carbon is -4
Group 5A
Group 6A
5 outer shell e- 6 outer shell etakes 3 etakes 2 e-3 charge
-2 charge
Group 7A
Group 8A
7 outer shell e- 8 outer shell etakes 1 e*already stable
-1 charge
0 charge
*Goal is to be stable by having 8
electrons (octet rule)
Covalent Bonds
•Formed when 2
atoms share
electrons
•You complete me!
•Only between
NONMETALS
Particles formed by covalent bonds
are called molecules (ex: O2 & H2O)
Polar molecules have a separated
+ area & a - area b/c the e- are not
shared equally! *most common covalent bond
Ex: HCl, NH2 & WATER (H20)
Nonpolar molecules have the
same charge (+ or -) because the
e- are shared equally!
Ex: Cl2, CO2, O2
Ionic Diagrams
1.Identify each
element as a
metal or
nonmetal
2.State if Ionic
or Covalent
3.Draw the
diagram for
the formation
of the
compound
Ionic Diagrams Need 4 things:
•Equation
•Dots
•Arrows
Your notes
paper
•Charges
1. Mg F2
Mg + F + F
MgF2
Covalent Diagrams
1.Identify each
element as a metal
or nonmetal
2.State if Ionic or
Covalent
3.Draw the diagram
for the formation of
the compound
4.If covalent, state if
Polar or nonpolar
Covalent Diagrams Need 2 things:
•Dots
Your notes
paper
•Circles
2. H F
H
F
Ionic and Covalent Diagrams
more examples
My paper
1. LiCl
2. Cl2
Your paper
1. LiF
2. Cl2
Name
I/C Diagrams
STAR questions
What type of bond would a metal and nonmetal
be?
Ionic
What is the name of the particles formed by a
covalent bond?
Molecules
What type of bond holds atoms of Au together?
metallic
Naming Binary Ionic Compounds
 Composed of 2 elements
1. Write the name of 1st element
2. Write the root of the 2nd element,
changing the ending to
–ide
One Nonmetal
and One Metal!
****(Name of cation, then anion)

*See chart on page 171
Examples:
MgO=Magnesium Oxide
NaCl=Sodium Chloride
Al2O3=
Writing Formulas Binary Ionic Compounds
1. Write symbol for 1st element
2. Write symbol for 2nd element
3. Find the oxidation # (charge) for
each element
4. drop n’ swap the oxidation #
(drop=w/out the + or - )
(swap=give the # to the other element)
5. Reduce if possible
Examples:
 Lead Oxide
1. Pb
2. O
3. Pb +/-4 and O -2
4. Pb2O4
5. PbO2
 Aluminum Sulfide = Al S
Al=+3, S=-2 ,
drop charges & swap #s
Al2S3
 Lithium Fluoride
 Calcium Oxide
Molecular Binary # of atoms Greek Prefix
1
MonoCovalent Compounds
The name &
formula of a
molecular
compound
describes the type
& # of atoms in a
molecule of the
compound
2
3
4
5
6
7
8
9
10
DiTriTetraPentaHexaHeptaOctaNonaDeca-
Naming molecular compounds ex:
1. N2O4
dinitrogen tetraoxide
2. CO2
carbon dioxide
Writing Molecular Formula ex:
1. Diphosporous tetraflouride
P2F4
2. Carbon dioxide
CO2
More Binary and Molecular
compounds examples
1. P2F4
2. Li2S
3. MgF2
4. Carbon Dioxide
5. Aluminum Oxide
6. Calcium Bromide
STAR questions
Another word for oxidation # is?
Charge
What is the difference between an
Anion and a Cation?
An Anion w/ a negative charge, a
Cation is an ion w/ a positive charge
How many elements are in Binary
compounds?
2
Naming Polyatomic Compounds
 Polyatomic ion-positive
or negative group of
atoms
1. Write name of first
element
2. Write name of the
polyatomic ion
Examples:
 CaCO3 = Calcium Carbonate
Mg(ClO3)2
Writing Formulas Polyatomic Compounds
1. Write symbol of first element
2. Write symbol of polyatomic ion
3. Find the oxidation #’s
4. drop n’ swap!
Use parenthesis around the
polyatomic ion if crossing more
than one!
5. Reduce if possible
Examples:
Lithium Sulfate
1.
2.
3.
4.
Li
SO4
Li +1, SO4 -2
Li2(SO4)
 Magnesium Nitrate
 Ammonium Bromide
STAR questions
 Another word for oxidation # is?
 Charge
 What does a subscript tell me?
 The #s of atoms of each element
 What does the superscript tell me?
 The charge for the elements or compound
 What type of elements are Molecular compounds?
 Covalent (nonmetals) binary (2 elements)