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Ionic compounds are formed when a metal bonds with a non-metal. This type of bonding involves the transfer of electrons. Generally, the metal donates electrons to the non-metal. In the process, the metal becomes a positively charged ion called a cation, while the non-metal becomes a negatively charged ion called an anion. These opposite charges attract, holding the ions together in an ionic bond.
These compounds usually have high melting and boiling points because the ionic bonds are very strong. They often form crystalline structures and can conduct electricity when dissolved in water.
In the exercise, compounds like \(\mathrm{CaF}_{2}\) and \(\mathrm{AlF}_{3}\) are examples of ionic compounds. Calcium, aluminum, and the non-metal fluorine, form strong ionic bonds due to the transfer of electrons.

Molecular compounds, also known as covalent compounds, are formed when two or more non-metal atoms share electrons. This sharing results in a covalent bond. Unlike ionic bonds, there isn't a transfer of electrons. Instead, the atoms attain stable electron configurations by sharing electrons.
Molecular compounds tend to have lower melting and boiling points compared to ionic compounds. They might not conduct electricity, as they don't form ions in solutions.
Consider the compound \(\mathrm{ClF}_{3}\) from the exercise. Chlorine and fluorine are both non-metals, and they share electrons, making \(\mathrm{ClF}_{3}\) a molecular compound. The naming reflects how many atoms of each are present, for example, Chlorine Trifluoride, indicating one chlorine and three fluorine atoms.

The naming conventions for ionic and molecular compounds are different due to their distinct bond types.

• Ionic Compounds: Usually named by stating the cation first and then the anion. If the metal can have different charges (transition metals), the specific charge is indicated by a Roman numeral in parentheses. For example, \(\mathrm{VF}_{3}\) is called Vanadium(III) Fluoride.
• Molecular Compounds: These use prefixes to denote the numbers of atoms. Mono- is often omitted for the first element. Examples include mono-, di-, tri-, tetra-, etc. For example, \(\mathrm{ClF}_{3}\) is named Chlorine Trifluoride, reflecting the presence of three fluorine atoms.

These systematic naming patterns help universally identify compounds by their chemical composition.