Ionic, Covalent and Metallic Bonding

Ionic bonding is the electrostatic attraction between oppositely charged ions, typically formed when one atom donates an electron to another, resulting in the formation of cations and anions.

Covalent bonding is the sharing of electron pairs between atoms, allowing them to achieve a full outer shell of electrons.

Metallic bonding is the attraction between metal ions and delocalized electrons, allowing metals to conduct electricity and heat.

Ionic compounds typically consist of a metal and a non-metal, and they often have high melting and boiling points.

Covalent compounds usually consist of non-metals and may have lower melting and boiling points compared to ionic compounds.

Magnesium oxide (MgO) is an example of an ionic compound.

Sulfur dioxide (SO2) is an example of a covalent compound.

Electron sharing allows atoms to achieve a stable electron configuration, similar to that of noble gases.

Electronegativity is a measure of an atom's ability to attract electrons; it helps determine whether a bond will be ionic or covalent.

A polar covalent bond is a type of covalent bond where electrons are shared unequally between atoms, resulting in partial charges.