Chemical Bonding
1 Compounds
definition Compound
A substance made of two or more elements chemically combined
definition Valence shell
The outermost shell or energy level
definition Octet Rule
{ Atoms tent to gain, lose or share electrons reach a con
guration with 8 electrons in the
valence shell (Noble gas con
guration)
Exceptions: Transition metals, elements near helium (Bond to get 2 electrons in outer
shell) }
2 Ionic Bonding
definition Ionic Bonding
Electrostatic force of attraction between two oppositely charged ions
definition Ion
Atom or group of atoms that have gained or lost electron(s)
definition Cation
Positive Ion
Na+ Ca2+ Al3+
definition Anion
Negitive Ion
F O2 N3
Ionic bonds form when ∆En > 1.7
example
Na Na+ + e
Cl + e Cl
Na+ + Cl NaCl
Complex Ions
Name Formula Charge
Hydroxide OH -1
Nitrate NO3 -1
1
, Name Formula Charge
Hydrogencarbonate HCO3 -1
Permanganate MnO4 -1
Carbonate CO32 -2
Chromate CrO42 -2
Dichromate Cr2O72 -2
Sulfate SO42 -2
Sul
te SO32 -2
Thiosulfate S2O32 -2
Phosphate PO43 -3
Ammonium NH4+ +1
definition Transition Metal
Forms at least one ion with a partially
lled D-sublevel
Have a variable valency
Formulas using Transition metals
Roman numeral is the group which that atom behaves like
IE the number of electrons in its outer shell
1 4 → 1+ 4+
example Iron(II) Chloride → Fe2+ + 2 Cl FeCl2
Iron(III) Chloride → Fe3+ + 3 Cl FeCl3
3 Covalent Bonding
definition Molecule
A group of atoms joined together. It is the smallest particle of an element or com-
pound that can exist independently
definition Valency
The number of monovalent elements which an atom of that element combines with
Covalent bonds form when ∆En < 1.7
3.1 Types of bonds
Single bonds bonds
definition Sigma (σ ) Bond
Formed from the head on overlap of two orbitals
Two atomic orbitals form a molecular orbital
Double Bonds
2
1 Compounds
definition Compound
A substance made of two or more elements chemically combined
definition Valence shell
The outermost shell or energy level
definition Octet Rule
{ Atoms tent to gain, lose or share electrons reach a con
guration with 8 electrons in the
valence shell (Noble gas con
guration)
Exceptions: Transition metals, elements near helium (Bond to get 2 electrons in outer
shell) }
2 Ionic Bonding
definition Ionic Bonding
Electrostatic force of attraction between two oppositely charged ions
definition Ion
Atom or group of atoms that have gained or lost electron(s)
definition Cation
Positive Ion
Na+ Ca2+ Al3+
definition Anion
Negitive Ion
F O2 N3
Ionic bonds form when ∆En > 1.7
example
Na Na+ + e
Cl + e Cl
Na+ + Cl NaCl
Complex Ions
Name Formula Charge
Hydroxide OH -1
Nitrate NO3 -1
1
, Name Formula Charge
Hydrogencarbonate HCO3 -1
Permanganate MnO4 -1
Carbonate CO32 -2
Chromate CrO42 -2
Dichromate Cr2O72 -2
Sulfate SO42 -2
Sul
te SO32 -2
Thiosulfate S2O32 -2
Phosphate PO43 -3
Ammonium NH4+ +1
definition Transition Metal
Forms at least one ion with a partially
lled D-sublevel
Have a variable valency
Formulas using Transition metals
Roman numeral is the group which that atom behaves like
IE the number of electrons in its outer shell
1 4 → 1+ 4+
example Iron(II) Chloride → Fe2+ + 2 Cl FeCl2
Iron(III) Chloride → Fe3+ + 3 Cl FeCl3
3 Covalent Bonding
definition Molecule
A group of atoms joined together. It is the smallest particle of an element or com-
pound that can exist independently
definition Valency
The number of monovalent elements which an atom of that element combines with
Covalent bonds form when ∆En < 1.7
3.1 Types of bonds
Single bonds bonds
definition Sigma (σ ) Bond
Formed from the head on overlap of two orbitals
Two atomic orbitals form a molecular orbital
Double Bonds
2
