Ionic Bonding and Octet Rule in Chemistry
Ionic Bonding
Ionic Bonding
Ga Standards
Ga Standards
Students know
atoms combine to
form molecules by sharing electrons to
form covalent or metallic bonds or
by
exchanging electrons to form ionic
bonds.
Students know
salt crystals, such
as NaCl, are repeating patterns of
positive and negative ions held
together by electrostatic attraction.
Bonds
Bonds
Forces that hold groups of atoms
Forces that hold groups of atoms
together and make them function
together and make them function
as a unit.
as a unit.
Ionic bonds – transfer of
Ionic bonds – transfer of
electrons
electrons
Covalent bonds – sharing of
Covalent bonds – sharing of
electrons
electrons
The
The
Octet
Octet
Rule – Ionic Compounds
Rule – Ionic Compounds
Ionic compounds form so that each atom, by
gaining or losing
electrons, has an octet of
electrons in its highest occupied energy level.
Metals lose electrons to form positively-charged
cations
Nonmetals gains electrons to form negatively-
charged anions
Ionic Bonding:
Ionic Bonding:
The Formation of Sodium Chloride
The Formation of Sodium Chloride
Sodium has 1 valence electron
Cl:
1s
2
2s
2
2p
6
3s
2
3p
5
Na:
1s
2
2s
2
2p
6
3s
1
Chlorine has 7 valence electrons
An electron transferred gives
each an octet
Ionic Bonding:
Ionic Bonding:
The Formation of Sodium Chloride
The Formation of Sodium Chloride
Cl
-
1s
2
2s
2
2p
6
3s
2
3p
6
Na
+
1s
2
2s
2
2p
6
This transfer forms
ions, each
with an
octet
:
Ionic Bonding:
Ionic Bonding:
The Formation of Sodium Chloride
The Formation of Sodium Chloride
Cl
-
Na
+
The resulting ions come together
due to electrostatic attraction
(opposites attract)
:
The net charge on the compound
must equal zero
Examples of Ionic compounds
Examples of Ionic compounds
Mg
2+
Cl
-
2
Na
+
2
O
2-
Magnesium chloride:
Magnesium
loses two electrons and each
chlorine gains one electron
Sodium oxide:
Each sodium loses one
electron and the oxygen gains two
electrons
Al
3+
2
S
2-
3
Aluminum sulfide:
Each aluminum
loses two electrons (six total) and
each sulfur gains two electrons (six
total)
Sodium Chloride Crystal Lattice
Sodium Chloride Crystal Lattice
Ionic compounds form
Ionic compounds form
solid
solid
crystals
crystals
at ordinary
at ordinary
temperatures.
temperatures.
Ionic compounds organize
Ionic compounds organize
in a characteristic
in a characteristic
crystal lattice of
crystal lattice of
alternating positive and
alternating positive and
negative ions.
negative ions.
All salts
are ionic compounds
and form
crystals
.
Properties of Ionic Compounds
Properties of Ionic Compounds
Understanding the concept of ionic bonding and octet rule in chemistry is essential for grasping how atoms combine to form molecules through sharing or exchanging electrons. This process involves the formation of positive and negative ions held together by electrostatic attraction, leading to the creation of various ionic compounds. Metal monatomic cations play a crucial role in this bonding process. Explore the forces that hold atoms together to form functional units, whether through ionic or covalent bonds, and delve into examples of different ionic compounds such as magnesium chloride, sodium oxide, and aluminum sulfide.
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Presentation Transcript
Ga Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction.
Bonds Forces that hold groups of atoms together and make them function as a unit. Ionic bonds transfer of electrons Covalent bonds sharing of electrons
The Octet Rule Ionic Compounds Ionic compounds form so that each atom, by gaining or losing electrons, has an octet of electrons in its highest occupied energy level. Metals lose electrons to form positively-charged cations Nonmetals gains electrons to form negatively- charged anions
Ionic Bonding: The Formation of Sodium Chloride Sodium has 1 valence electron Chlorine has 7 valence electrons An electron transferred gives each an octet Na: 1s22s22p63s1 Cl: 1s22s22p63s23p5
Ionic Bonding: The Formation of Sodium Chloride This transfer forms ions, each with an octet: Na+ 1s22s22p6 Cl- 1s22s22p63s23p6
Ionic Bonding: The Formation of Sodium Chloride The resulting ions come together due to electrostatic attraction (opposites attract): Na+ Cl- The net charge on the compound must equal zero
Examples of Ionic compounds Mg2+Cl-2 Magnesium chloride: Magnesium loses two electrons and each chlorine gains one electron Na+2O2- Sodium oxide: Each sodium loses one electron and the oxygen gains two electrons Al3+2S2-3 Aluminum sulfide: Each aluminum loses two electrons (six total) and each sulfur gains two electrons (six total)
Metal Monatomic Cations Li+ Na+ K+ Mg2+ Ca2+ Ba2+ Al3+ Ion name Lithium Sodium Potassium Magnesium Calcium Barium Aluminum Lithium Sodium Potassium Magnesium Calcium Barium Aluminum
Nonmetal Monatomic Anions F- Cl- Br- I- O2- S2- N3- P3- Ion Name Fluorine Chlorine Bromine Iodine Oxygen Sulfur Nitrogen Phosphorus Fluoride Chloride Bromide Iodide Oxide Sulfide Nitride Phosphide
Sodium Chloride Crystal Lattice Ionic compounds form solid crystals at ordinary temperatures. Ionic compounds organize in a characteristic crystal lattice of alternating positive and negative ions. All salts are ionic compounds and form crystals.
Properties of Ionic Compounds Structure: Melting point: Boiling Point: Electrical Conductivity: Solubility in water: Crystalline solids Generally high Generally high Excellent conductors, molten and aqueous Generally soluble
