Final answer:
Covalent compounds have lower melting and boiling points, poor electrical conductivity, and their water solubility varies based on the intermolecular forces present.
Step-by-step explanation:
Covalent compounds, also known as molecular compounds, are characterized by atoms sharing pairs of valence electrons, resulting in the formation of covalent bonds. These covalent bonds lead to several distinctive properties:
- Low melting and boiling points: Compared to ionic compounds, covalent compounds have much lower melting and boiling points, often existing as gases or liquids at room temperature.
- Poor electrical conductivity: Covalent compounds do not conduct electricity well in any state due to their electrically neutral molecules.
- Variability in water solubility: The water solubility of covalent compounds is highly dependent on the type of intermolecular forces involved. Substances with hydrogen bonding or dipole-dipole forces are generally more soluble, while those with London dispersion forces tend to be less soluble.
These properties contrast sharply with ionic compounds, which typically have high melting and boiling points, can conduct electricity when dissolved in water, and are often water-soluble.
Covalent compounds, also known as molecular compounds, have several distinctive properties. Unlike ionic compounds and metals, covalent compounds have lower boiling and melting points, are often in the form of gases or low-boiling liquids, and are typically softer. They are generally poor conductors of electricity, whether in the solid or liquid state, and they may not dissolve easily in water.