What are the differences between ionic and covalent compounds?

Ionic compounds are formed from a metal and a non-metal, while covalent compounds are formed between two non-metals.

Ionic compounds are formed when a metal and a non-metal react with each other. In this reaction, the metal loses electrons to become a positively charged ion, while the non-metal gains these electrons to become a negatively charged ion. This transfer of electrons results in the formation of an ionic bond, which is the force of attraction between the oppositely charged ions. This bond is very strong, which is why ionic compounds have high melting and boiling points. They also conduct electricity when dissolved in water or melted, as the ions are free to move and carry charge. Examples of ionic compounds include sodium chloride (NaCl) and magnesium oxide (MgO).

On the other hand, covalent compounds are formed when two non-metals combine. Instead of transferring electrons as in ionic bonding, the atoms in a covalent bond share electrons. This sharing allows each atom to achieve a stable electron configuration. Covalent bonds can be single, double, or triple, depending on the number of electron pairs being shared. Covalent compounds generally have lower melting and boiling points compared to ionic compounds, as the forces between molecules (intermolecular forces) are weaker than ionic bonds. They also do not conduct electricity, as there are no charged particles free to move. Examples of covalent compounds include water (H2O) and carbon dioxide (CO2).

In summary, the key differences between ionic and covalent compounds lie in the types of elements involved, the nature of the bonding, and their physical properties such as melting and boiling points and electrical conductivity.