Final answer:
A covalent bond involves the sharing of valence electrons between two atoms. This type of bond is fundamental for molecular stability and is found when atoms with similar electronegativity form a compound. Examples of covalent bonds include H-Cl, O=O, and N=N, where atoms share one, two, or three pairs of electrons, respectively.
Step-by-step explanation:
Understanding Covalent Bonds
The type of bonding that involves the sharing of valence electrons between two atoms is called a covalent bond. This kind of chemical bond is essential for the formation of molecules, where electrons occupy the space between nuclei and are considered to be shared by the atoms. Covalent bonds are characterized by the sharing of one or more pairs of valence electrons, and they are integral to the structural framework of many compounds.
The strength of a covalent bond can vary and is typically weaker than metallic and ionic bonds, yet much stronger than intermolecular forces. These bonds are crucial in the creation of stable compounds where the shared electrons allow atoms to complete their valence shells, leading to the stability of the molecule. A classic example of a covalent bond is seen in the hydrogen chloride (H-Cl) molecule, where hydrogen and chlorine share a pair of electrons, with chlorine also having three nonbonding or lone pairs of electrons. Moreover, atoms can share two pairs of electrons to form a double bond or three pairs to form a triple bond.
Covalent bonds can form between atoms of nonmetals and arise when there is a moderate to zero electronegativity difference between the atoms (<1.9). The shared valence electrons provide an attractive force that holds the atoms together, creating a stable configuration such as in a molecule of hydrogen gas (H-H), where each hydrogen atom shares its single electron.