* Sharing Electrons: Nonmetals have a high electronegativity, meaning they have a strong attraction for electrons. When nonmetals bond, they share electrons rather than transferring them (like in ionic bonds). This sharing creates a stable, balanced arrangement of electrons, forming a covalent bond.
* Strong Attraction: The shared electrons create a strong attraction between the nuclei of the bonded atoms, holding them together.
* Types of Covalent Bonds: Covalent bonds can be further categorized as:
* Single Bonds: One pair of electrons is shared between the atoms.
* Double Bonds: Two pairs of electrons are shared between the atoms.
* Triple Bonds: Three pairs of electrons are shared between the atoms.
Examples:
* Water (H₂O): Two hydrogen atoms share electrons with an oxygen atom, forming two covalent bonds.
* Carbon Dioxide (CO₂): A carbon atom shares two pairs of electrons with each oxygen atom, forming two double covalent bonds.
* Nitrogen (N₂): Two nitrogen atoms share three pairs of electrons, forming a triple covalent bond.
Key Point: While covalent bonds are the most common type of bond between nonmetal atoms, there are some exceptions. For example, diatomic molecules like bromine (Br₂) and iodine (I₂) form relatively weak covalent bonds.
