Types of Chemical Bonds
• Covalent Bonds
– Single
– Double
– Triple
-- Polar
-- Non-Polar
Once again…
AN OVERVIEW
of the 3 main types of bond:
while keeping in mind:
• Ionic Bonds
• Metallic Bonds
• Other “Bonds”
– Inter-Molecular Forces
Ionic Bonds
An ionic bond is the attraction between
a metal cation and a non-metal anion
Metallic Bonding
Atoms are unhappy if their outer
energy level is not full!!
Atoms only bond with other atoms in
order to fill their outer energy level.
Covalent Bonds
A covalent bond exists when two electrons
are shared by non-metallic atoms.
Ionic bonds
Metal + Non-metal
• Difference in electronegativity is high; so high
that non-metal atoms will strip away valence
electrons from the metal atoms, forming ions.
Takes place in a
“SEA” OF MOBILE VALENCE
ELECTRONS
These bonds are formed due to an attraction
between opposite charges (+,-);
there is no sharing of electrons.
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Ionic Bonds
Ionic Bonds
17+
11+
Sodium
Chlorine
17+
11+
Sodium Ion (+1)
Na now has 11p+ and
10e-. It now carries a
charge of +1.
Ionic Bonding: How it Works
Chloride Ion (-1)
Cl now has 17p+ and
18e-. It now carries a
charge of -1
Rules for Naming Ionic Compounds:
i) Metal + Non Metal
ii) Ions Form (via electron transfer)
•
•
iii) Opposites attract
Name the cation
Name the anion
2 Questions:
Why don’t we need any prefixes?
How do you name a cation or an anion?
Naming Cations
• Cation- if the charge is always the same
(i.e. Groups 1, 2 or 13) just write the name of
the metal.
Examples:
Sodium
Aluminum
Magnesium
• Transition metals can have more than one type
of charge, so we need Roman Numeral in
parentheses to indicate the charge.
Examples:
Copper (II)
Titanium (IV)
Iron (III)
+1
Some element always form
the same old ions…
+2
+3
-3 -2 -1
2
•
•
•
•
Na +1
Al +3
Fe +2
Pb +2
Name these
Write Formulas for these
•
•
•
•
Potassium ion
Magnesium ion
Chromium (IV) ion
Mercury (II) ion
Name these
•
•
•
•
Cl-1
N-3
Br-1
S-2
Write Formulas for these
•
•
•
•
Sulfide ion
Iodide ion
Phosphide ion
Sulfide ion
And practice with predicting formulae:
SrBr2
______
Strontium Bromide
TiO2
______
Titanium (IV) Oxide
CoS
______
Cobalt (II) Sulfide
Li3N
______
Lithium Nitride
AlCl3
______
Aluminum Chloride
Naming Anions
• Non-metals are predictable; each nonmetal element can only form one anion.
• Change the element ending to – ide
• Fluorine (F) becomes Fluoride (F1-)
• Oxygen (O) becomes Oxide (O2-)
Now for practice naming the compounds:
KI
Potassium Iodide
__________________________
TiCl
Titanium (I) Chloride
__________________________
MnBr2
Manganese (II) Bromide
__________________________
Al2O3
Aluminum Oxide
__________________________
Ions are charged atoms…
…or charged groups of atoms.
Polyatomic ion: A covalently
bonded group of atoms with a net
charge.
1- Anions:
Acetate
C2H3O2 -1
Hydroxide
Nitrate
NO3-1
Permanganate MnO4-1
Nitrite
NO2-1
Cyanide
OH-1
CN-1
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More polyatomic ions
2- Anions:
SO4-2
Sulfite
SO3-2
Carbonate CO3-2
Chromate CrO4-2
Dichromate Cr2O7-2
Sulfate
3- Anions:
Phosphate PO4-3
Phosphite PO3-3
Ammonium NH4+1
Magnesium Hydroxide
__________________________
Sodium Acetate
NaC2H3O2 __________________________
CuSO4
KOH
1+ Cations:
Now for practice naming these compounds:
Mg(OH)2
Ionic Compounds containing
polyatomic ions have ionic and
covalent bonds:
Copper (II) Sulfate
__________________________
Calcium Phosphate
Ca3(PO4)2 __________________________
K+
Ionic bond
(:O H)-
And practice with predicting these formulae:
CaCO3
______
Calcium Carbonate
NaOH
______
Sodium Hydroxide
KMnO4
______
Potassium Permanganate
Pb(NO3)2
______
Lead (II) Nitrate
MgSO3
______
Magnesium Sulfite
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