Chemistry - Chemical Bonding (Ionic, Covalent, and Metallic)

Ionic Bonding: The electrostatic attraction between oppositely charged ions formed by the complete transfer of electrons from a metal to a non-metal, such as in $NaCl$.

Covalent Bonding: The electrostatic attraction between a shared pair of electrons and the positively charged nuclei of the atoms involved, typically occurring between non-metals like in $H_{2}O$.

Metallic Bonding: The electrostatic attraction between a lattice of positive metal ions ($cations$) and a 'sea' of delocalized valence electrons.

The Octet Rule: Atoms tend to lose, gain, or share electrons to achieve a stable electron configuration with $8$ electrons in their valence shell, similar to Noble Gases ($Group 18$).

Electronegativity Difference ($\Delta\chi$): Used to predict bond type. If $\Delta\chi > 1.8$, the bond is generally ionic; if $0.5 < \Delta\chi < 1.8$, it is polar covalent; if $\Delta\chi < 0.5$, it is non-polar covalent.

Giant Covalent Structures: Substances like Diamond ($C$), Graphite ($C$), and Silicon Dioxide ($SiO_{2}$) which have high melting points due to a network of strong covalent bonds.

Properties of Ionic Compounds: High melting/boiling points due to strong lattice enthalpy, and the ability to conduct electricity only in molten or aqueous states ($aq$) where ions are mobile.