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Introduction: What is Covalent Bonding?
Covalent bonds are a type of chemical bond formed when two atoms share pair(s) of valence electrons. Each atom contributes at least one electron to the shared pair.
Covalent bonding decreases the potential energy of atoms' electron configurations by sharing electrons.
The bonding electrons attract the nuclei of parent atoms together via electrostatic forces.
Types: Single (1 e⁻ pair), Double (2 e⁻ pairs), Triple (3 e⁻ pairs).
This type of bonding typically occurs between nonmetal atoms of similar electronegativities.
The Purpose of Covalent Bonding
By sharing electrons, atoms of a molecule or lattice can acquire more stable electron configurations.
Example: A water molecule (H₂O) forms when two hydrogen atoms each share their single electron with an oxygen atom, which shares one of its own electrons with each hydrogen atom. This covalent bond stabilizes the electron configurations of all three atoms by filling their outer electron shells.
Properties of Covalent Compounds
Covalent compounds typically exist as:
Molecular Compounds: Composed of molecules, which are atoms that are covalently bonded together and act as discrete units of a compound.
Melting Point: Low
Conductivity: Not conductive.
Solubility: Depends on the polarity of the solid and the solvent.
Physical Properties: Generally softer than other types of solids.
Covalent Networks: Composed of a pattern of atoms that are covalently bonded together, creating a crystal lattice. The pattern can go on indefinitely, so we use formula units to define them in a unitary manner.
Melting Point: High
Conductivity: Not conductive.
An exception is graphite, which is conductive due to the presence of delocalized electrons.
Solubility: Insoluble in most solvents.
Physical Properties: Hard and brittle.
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