Bonding: The glue that holds
it all together
Ionic bonding
Metalic bonding
Covalent bonding
Intermolecular forces
Atom gain, lose or share
elections to follow the Octet
rule
• Metals give up electrons and
become “cations” (positive
charge)
• Nonmetals take in electrons and
become “anions” (negative
charge)
• Non metals may “share”
The Fatal attraction
Cations and anions
become “locked” in a
matrix of attraction
between positive and
negative particles
Ionic compounds
1. Crystalline solids that have high
melting points.
2. They are often soluble in water
3. They conduct electricity when in
solution, or when molten
•
Ionic
Compounds
Repeating links in
a crystal matrix.
• Cation are bound
to neighboring
anions
• Ions are “locked
in place”
The Formula unit is the smallest ratio that indicates
an electrically neutral unit of this matrix
Predicting the formula
1. Identify the
charge of the
cation
2. Identify the
charge of the
anion
3. Make a table
4. Add ions until the
positive charge
equals the
Calcium reacts with
Fluorine
1. How many
electrons will
calcium give up?
2.How many can
Fluorine take in?
3.Fill the table in
and make a neutral
formula unit !!
Ca+?
F-?
Name that compound !!
1. CaF2
2.The cation is
called Calcium
3.The anion is
called Fluoride
4.The compound is
Calcium Fluoride
Calcium fluoride
Ionic compounds
can have the same
formula, and have
different colors
and crystalline
shapes
Ionic Solids are Crystals
1. Aluminum
reacts with
oxygen
2.Make a table
3.Identify the
formula unit
4.Name that
compound !!
http://mineral.galleries.com
Sodium & Fluorine
What is my
formula?
What is my
name?
Ionic compounds often have
polyatomic ions
Polyatomic ions are
Mg+2
groups of atoms that
stay together, they
are treated like
“super atoms”
NO3NO3-
Mg(NO3)2
NH4+
NH4+
SO3-2
(NH4)2SO3
Calcium & carbonate
What is my
formula?
What is my
name?
Strontium and carbonate
Ammonium and chloride
Remember
:ide means
the anion
is a nonmetal
element!
What is my
formula?
What is my
name?
Calcium & sulfate
Copper reacts with Oxygen
Make a table
Identify the formula
unit
Name that compound
!!
You need more
information – What
do you need?
Ionic compounds with transition
metals
• Transition metals can
have more than one
charge.
• Make tables & work
backwards to determine
cation charge
• Indicate charge with a
roman numeral
• REMEMBER THE TABLE
MUST BE BALANCED !!!!!
Fe+?
O-2
Fe+?
O-2
O-2
iron(III) oxide
Some Ions we need to just Know
•
•
•
•
Silver is always +1
Zinc is always +2
Cadmium is always +2
Do not use a roman numeral with these
• Iron may be +2 or +3
Tin may be +2 or +4
Lead may be +2 or +4
Use a roman numeral with these if the charge is
+2  an unexpected charge
Lead(IV) & carbonate
Lead(II) and phosphate
Lets practice !!!!
Potassium + Phosphorus
Lithium + Selenium
Aluminum + Chlorine
Gallium + Sulfur
Magnesium + Iodine
Sodium + Carbonate
Sodium + Hydrogen Carbonate
Strontium + Phosphate
Ammonium + Chromate
Barium + Acetate
Lets practice !!!!
Potassium + Phosphorus K3P
Lithium + Selenium
Aluminum + Chlorine
Li2Se
AlCl3
Gallium + Sulfur
Ga2S3
Magnesium + Iodine
MgI2
Sodium + Carbonate
Na2CO3
Sodium + Bicarbonate
NaHCO3
Strontium + Phosphate
Sr3(PO4)2
Ammonium + Chromate
(NH4)2CrO4
Barium + Acetate
Ba(C2H3O2)2
Lets Review!!!
calcium chloride
cesium oxide
aluminum perchlorate
barium sulfide
sodium dichromate
aluminum phosphate
calcium carbonate
sodium carbonate
Lets Review!!!
calcium chloride
CaCl2
cesium oxide
Cs2O
aluminum perchlorate
Al (ClO4)3
barium sulfide
BaS
sodium dichromate
Na2Cr2O7
aluminum phosphate
Al PO4
calcium carbonate
CaCO3
sodium carbonate
Na2CO3
Lets Review!!!
potassium oxide
strontium nitride
strontium nitrate
strontium nitrite
aluminum hydroxide
magnesium sulfate
iron(III) oxide
silver oxide
Lets Review!!!
Potassium Oxide
K2O
Strontium Nitride
Sr3N2
Strontium Nitrate
Sr(NO3)2
Strontium Nitrite
Sr(NO2)2
Aluminum Hydroxide
Al(OH)3
Magnesium Sulfate
MgSO4
Iron(III) Oxide
Fe2O3
Silver Oxide
Ag2O
Lets practice!!
Na2S
Hg2S
Na2Cr2O7
Hg2Cr2O7
CuO
Lets Practice Answers
Na2S
sodium sulfide
Hg2S
mercury(I) sulfide
Na2Cr2O7
sodium dichromate
Hg2Cr2O7
mercury(I) dichromate
CuO
copper(II) oxide
Lets Practice
calcium carbonate
ammonium sulfate
copper(I) phosphate
chromium(IV) acetate
cadmium perchlorate
Lets Practice
calcium carbonate
CaCO3
ammonium sulfate
(NH4)2SO4
copper(I) phosphate
Cu3PO4
chromium(IV) acetate
Cr(C2H3O2)4
cadmium perchlorate
Cd(ClO4)2
Links to practice tests and games
• Interactive link 1
• Interactive link 2
• Interactive link 3
Bonding: Part Two
• Ionic bonding is one way that atoms
attain a stable electron condition – that
is satisfy the octet rule.
• In this section we will look at metallic
bonding, covalent bonding, and the
formation of acids and polymers
• All forms of bonding involve valence
electrons, and the tendency to satisfy
the “octet rule”
Metallic Bonding
The nuclei of
metal atoms are
held together by
their attraction to
free-floating
valence electrons
that are found
between adjacent
nuclei
Web Elements
Covalent Bonding: when atoms
share electrons
Atoms still obey the octet
rule
Nitrogen: another
diatomic
• You try it !!!!
Electrons are shared in a triple
bond
There are 7 diatomic
atoms
• Hydrogen, oxygen, fluorine, chlorine,
iodine, bromine, and nitrogen.
• Some satisfy the octet rule with a
single covalent bond, others use a
double or a triple bond. Why not try
them all
Geometric shapes of Molecules
• The Shape of the molecule depends on
how many bonds and how many unshared
pairs of electrons are present
• Work out the Lewis structures for the
following molecules:
• H2O
BF3
NH3
CH4
CO2
How about water?
Bent linear
BF3: Trigonal planar
Pyramidal and Tetrahedral
NH3
CH4
Build a molecule tutorial
Electrons try to be as far
apart as they can be:
Carbon dioxide is a linear molecule
Prefixes are used in the names of
molecular compounds
• mono- one
• di-two
• tri-three
• tetra-four
• penta-five
• hexa-six
• hepta-seven
• octa-eight
• nona-nine
• deca-ten
N2O5 : dinitrogen pentoxide
Naming compounds
1. The more metallic element is named
first. The full name of the
element is used
2. The second element is named as if it
were an anion.
3. The number of atoms of each
element is shown by a prefix, but
the prefix mono- is never used for
the first element.
4. If the second element is oxygen and
a prefix ends with either an o or an
a, these letters are dropped from
Lets try some!!!!
CO2
P2O5
NO
SiO2
Al2O3
SO2
SO3
NO2
CO2
Carbon dioxide
P2O5
Diphosphorous pentoxide
NO
Nitrogen monoxide
SiO2
Silicone dioxide
Al2O3
Aluminum oxide
SO2
Sulfur dioxide
SO3
Sulfur trioxide
NO2
Nitrogen dioxide
Boron trifluoride
Silver fluoride
Copper (II) fluoride
Magnesium chloride
Manganese (I)
chloride
Nitrogen dichloride
Ammonium
carbonate
Dinitrogen
heptoxide
Gold (II) oxide
Try it !!!
Boron trifluoride
Silver fluoride
Copper (II) fluoride
Magnesium chloride
Manganese (I) chloride
Nitrogen dichloride
Ammonium carbonate
Dinitrogen heptoxide
Gold (II) oxide
Heptoxide monofloride
BF3
AgF
CuF2
MgCl2
MnCl
NCl2
(NH4)2CO3
N2O7
AuO
O7F
Acids – special molecular
compounds
1. When hydrogen is the first element,
the compound has special
characteristics, and is named as an
acid
2. Acids are electrolytes (like ionic
compounds)
3. Acids are reactive, and dissasociate
to form ions when placed in water
4. HCl H+ + Cl-
Acids get their own names
Identify and name the anion
Use the following rules ones you know the
name of the anion:
1. ide  hydro ________ ic acid (HCl)
2. ite  ____________ous acid (HClO2)
3. ate _____________ic acid
(HClO3)
(hydrochloric acid, chlorous acid, chloric
H 3N
Try Naming some acids !!!
HNO2
HNO3
H 2S
H2SO4
H2SO3
H2CO3
H3PO4
H 3N
Try Naming some acids !!!
Hydronitric acid
HNO2
Nitrous acid
HNO3
Nitric acid
H 2S
Hydrosulfuric acid
H2SO4
Sulfuric acid
H2SO3
Sulfurous acid
H2CO3
Carbonic acid
H3PO4
Phosphoric acid
Write some formulas
Hydrobromic acid
Hypochlorous acid
Perchloric acid
Permanganic acid
Chromatic acid
Hydrosulfuric acid
Hydrohydroxic acid
Acetic acid
Oxylic acid
Nitrous acid
Write some formulas
Hydrobromic acid
HBr
Hypochlorous acid
HClO
Perchloric acid
HClO4
Permanganic acid
Chromatic acid
HMnO4
Hydrosulfuric acid
H2CrO4
H2SO4
Hydrohydroxic acid
HOH
Acetic acid
HC2H3O2
Oxylic acid
H2C2O4
Nitrous acid
HNO2
Organic molecules
• These have there own rules, and their own prefixes that
indicate how many carbons:
• The alkanes have the formula CnH2n+2
• Methane (one carbon)
• Ethane (two carbons)
• Propane (three carbons)
• Butane (four carbons)
• Pentane (five carbons)
• Hexane (six carbons)
• Heptane (seven carbons)
• Octane (eight carbons)
Each carbon develops 4 bonds
methane
Ethane : C2H6
Propane: C3H8
Link to bondit
Benzene
Metallic Bonding
The nuclei of
metal atoms are
held together by
their attraction to
free-floating
valence electrons
that are found
between adjacent
nuclei
Web Elements