Molecular compounds are formed when two or more non-metal atoms share electrons to create covalent bonds. This sharing of electrons allows the atoms to achieve a stable electron configuration, similar to noble gases.
Here's a breakdown of key characteristics:
* Made of nonmetals: Examples include carbon (C), oxygen (O), nitrogen (N), chlorine (Cl), etc.
* Covalent bonding: Atoms share electrons, not transfer them like in ionic compounds.
* Discrete molecules: These compounds exist as distinct, individual units, often with a specific geometric shape.
* Lower melting and boiling points: Generally have weaker intermolecular forces compared to ionic compounds.
* Usually non-conductive: Do not conduct electricity in their solid or liquid states.
* Often exist as gases or liquids at room temperature: Due to weaker intermolecular forces.
Examples of molecular compounds:
* Water (H2O): Two hydrogen atoms share electrons with one oxygen atom.
* Carbon dioxide (CO2): One carbon atom shares electrons with two oxygen atoms.
* Methane (CH4): One carbon atom shares electrons with four hydrogen atoms.
* Sugar (C12H22O11): A complex molecule with multiple covalent bonds.
In contrast to ionic compounds:
* Ionic compounds form from the electrostatic attraction between oppositely charged ions, usually involving a metal and a non-metal.
* They have high melting and boiling points, are often crystalline solids, and can conduct electricity when dissolved in water.
Understanding the difference between ionic and molecular compounds is crucial in chemistry, allowing you to predict their properties and reactions.
