3. Introduction to bonding
• An attraction between atoms that allows the
formation of chemical substances that contain
two or more atoms.
• Atoms form chemical bonds to become stable.
4. Ionic bonding
• Ionic bonds are formed between cation
and ion. Ionic bonds is a type of chemical
bond formed through an electrostatic
attraction between two oppositely
charged ions.
• Greater charge = Greater electrostatic
attraction; stronger bond = Higher
melting point
5. Ionic Bonding Continued
• The size of the ions also affect the
melting point! Ionic solids don’t
conduct electricity!
6. Covalent Bonds
• When atoms bond covalently they count a
share in the pair of electrons in the covalent
bond as two electrons in their counter shell.
• A single covalent bond is when two electrons
are shared between atoms. A double band is
when four electrons are shared and a triple is
when six electrons are shared.
7. Covalent Bonds Continued
• A sigma bond is the end to the end overlap of
the bonding orbitals, usually hybrid orbitals.
The sigma bond is a single bond. A pi bond is
the side to side overlap of hybridized p-
orbitals. Together they form a double bond.
• As bond length decreases, bond dissociation
energy increases.
8. Metallic Bonds
• A metallic bond is formed when atoms of
metal group together to for a crystal.
• Alloys- a homogeneous mixture or solid
solution of two or more metals, the atoms of
one repulsing or occupying interstitial
positions between atoms of others.
