Answer:
Ionic, Covalent, Metallic, Hydrogen
Step-by-step explanation:
Ionic Bonds:
Formation: Ionic bonds are formed when one atom transfers electrons to another atom, resulting in the formation of oppositely charged ions. Typically, one atom loses electrons (cation, positively charged) while the other gains electrons (anion, negatively charged).
Example: Sodium (Na) forms an ionic bond with chlorine (Cl) to create sodium chloride (NaCl, table salt).
Covalent Bonds:
Formation: Covalent bonds are formed when two atoms share electrons to achieve a full outer electron shell. In a covalent bond, electrons are shared between atoms, creating molecules.
Example: In a water molecule (H₂O), hydrogen atoms share electrons with an oxygen atom.
Metallic Bonds:
Formation: Metallic bonds occur between atoms in metals and are characterized by the sharing of a "sea" of electrons that move freely throughout the metal lattice, allowing for excellent electrical conductivity and malleability.
Example: In a piece of pure elemental copper, the copper atoms are held together by metallic bonds.
Hydrogen Bonds:
Formation: Hydrogen bonds are not true chemical bonds but are strong electrostatic attractions between a hydrogen atom that is covalently bonded to a highly electronegative atom (e.g., oxygen, nitrogen, or fluorine) and another electronegative atom in a different molecule.
Example: In water (H₂O), hydrogen bonds form between the partially positive hydrogen atom of one water molecule and the partially negative oxygen atom of another, giving water its unique properties like high surface tension and high heat capacity.