Covalently bonded molecules have strong intramolecular bonds but weak intermolecular forces, resulting in low melting and boiling points. Since no charged particles are formed, these compounds are generally poor conductors of electricity.
Why do covalently bonded molecules like ammonia and methane have low melting and boiling points, and why are they generally poor conductors of electricity?
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Covalently bonded molecules like ammonia and methane have low melting and boiling points due to weak intermolecular forces. In these compounds, molecules are held together by comparatively weaker van der Waals forces or hydrogen bonding, requiring less energy for state changes. Furthermore, covalent compounds are generally poor conductors of electricity because they lack free ions. In covalent bonds, electrons are shared rather than transferred, resulting in the absence of charged particles that can carry an electric current. The combination of weak intermolecular forces and the absence of free ions contributes to the low melting and boiling points and poor conductivity in covalently bonded molecules.