Atoms in a molecule are held together by chemical bonds, which can be covalent, ionic, or metallic. Covalent bonds form when atoms share electrons, while ionic bonds form when atoms transfer electrons. Metallic bonds form in metal atoms due to the sharing of electrons in a "sea" of electrons. In this article, we will study in detail about "What Holds Atoms Together in a Molecule?"
1. Chemical Bonds That Hold Atoms Together in a Molecule
1.1 Covalent Bond A covalent bond is a type of chemical bond that occurs when two atoms share electrons. This bond forms when the atoms have similar electronegativity values and the shared electrons are attracted to the nuclei of both atoms. Covalent bonds are typically found in molecules made up of non-metal atoms. The strength of a covalent bond depends on the number of electrons shared and the distance between the atoms. Covalent bonds are characterized as either single, double, or triple bonds, depending on the number of electrons shared.
1.2 Ionic Bond An ionic bond is a type of chemical bond that occurs when one atom gives up one or more electrons to another atom. This results in the formation of ions, which are atoms or molecules that have a positive or negative charge. Ionic bonds typically form between a metal atom and a non-metal atom. The metal atom loses one or more electrons to form a positive ion (or cation), while the non-metal atom gains electrons to form a negative ion (or anion). The electrostatic attraction between the cation and anion holds the ionic compound together. Ionic bonds are typically stronger than covalent bonds and weaker than metallic bonds. They are typically found in compounds between a metal and a non-metal.
1.3 Metallic Bond A metallic bond is a type of chemical bond that occurs in metallic elements and alloys. It is characterized by the delocalized, or "sea" of electrons that surrounds metal ions. The metallic bond is formed by the attraction between the positively charged metal ions and the delocalized or mobile electrons that surround them. These electrons are free to move throughout the metal lattice, which gives metallic materials their unique properties, such as high electrical conductivity and thermal conductivity. The strength of a metallic bond depends on the number of delocalized electrons and the number of metal ions in the lattice. It is typically weaker than covalent and ionic bonds.
