Study Notes on Chemical Bonding

Definition: This type of bonding involves the transfer of electrons, typically from a metal to a non-metal.

Good Conductors of Electricity: Electrovalent compounds, when dissolved in water or molten, conduct electricity due to the presence of charged ions.
Crystal Structure: They form crystalline solids with organized structures.
High Melting and Boiling Points: Electrovalent compounds generally showcase elevated melting and boiling points due to the strong ionic bonds between charged ions.
Insoluble in Organic Solvents: These compounds typically do not dissolve in organic solvents, but can dissolve in polar solvents like water.

Definition: This bond is characterized by the sharing of electrons between atoms, usually occurring between non-metals.

Poor Conductors of Electricity: Covalent compounds do not conduct electricity well because they do not have free ions or charged particles.
Lower Melting and Boiling Points: Generally, covalent compounds have lower melting and boiling points compared to ionic compounds due to weaker intermolecular forces (Van der Waals forces) compared to ionic bonds.
Less Ionic Character: Covalent bonds often have lower ionic character than ionic bonds due to the nature of electron sharing.

Definition: Also known as a dative bond, this occurs when one atom shares a pair of electrons that originated from a single atom when forming a bond with another atom.

This bond involves one atom providing both of the electrons for the shared pair, allowing the bond to form without both atoms having to supply electrons.

An example of a coordinate covalent bond is the formation of ammonium ion (NH₄⁺), where a nitrogen atom shares a lone pair of electrons with a hydrogen ion (H⁺) to form a stable compound.