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Why do covalently bonded compounds have low boiling point?
Have strong covalent bond within molecules but weak intermolecular force
Have weak covalent bond within molecules but weak intermolecular force
Have strong covalent bond within molecules and also strong intermolecular force
Have strong intermolecular force within molecules but weak covalent bond
Have strong covalent bond within molecules but weak intermolecular force
Covalent compounds generally have low melting and boiling points because the forces of attraction between individual molecules (intermolecular forces) are very weak, even though the covalent bonds holding the atoms together within each molecule are extremely strong.
Covalent compounds generally have low melting and boiling points because the forces of attraction between individual molecules (intermolecular forces) are very weak, even though the covalent bonds holding the atoms together within each molecule are extremely strong.
Think of covalent molecules like tightly bound footballs: the leather panels are stitched together with incredibly strong thread (intramolecular covalent bonds), but the footballs themselves just sit next to each other on a shelf with barely any force holding one ball to the next (weak intermolecular forces). It takes very little effort to push the balls apart from one another.
Intra is strong inside, Inter is weak in between!
FinterтАЛтЙкFintraтАЛ тАФ Comparison of intermolecular vs intramolecular force strength
In covalent molecular compounds (such as methane, water, or carbon dioxide), atoms share electrons to form discrete molecules with strong intramolecular covalent bonds. However, the forces holding these discrete molecules to each other in the solid or liquid state are weak intermolecular forces (such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds). When a covalent compound melts or boils, it is these weak intermolecular forces that must be overcomeтАФnot the strong covalent bonds. Consequently, very little thermal energy is required to separate the molecules, resulting in low melting and boiling points.
Covalent compounds consist of neutral molecules rather than charged ions.
The bonds holding atoms together within the molecule (intramolecular) are strong covalent bonds.
The forces holding different molecules together in the bulk substance (intermolecular forces) are weak van der Waals forces or dipole-dipole interactions.
Melting or boiling requires breaking intermolecular attractions, not intramolecular bonds.
Explains why many covalent compounds are gases or liquids at room temperature (e.g., CO2тАЛ, H2тАЛO, CH4тАЛ).
Does not apply to giant covalent structures like diamond, graphite, or silicon dioxide, which have high melting points due to extensive covalent networks.
Fractional distillation of crude oil relies on low boiling points of hydrocarbon molecules.
Refrigerants and propellants utilize low boiling points of small covalent molecules.
Option A is correct: Covalent compounds have strong covalent bonds within molecules but weak intermolecular forces between them.
Giant covalent lattices (like diamond) are important exceptions to this rule.
A is correct тАФ Covalent compounds have strong covalent bonds within molecules but weak intermolecular forces.
Always distinguish between intramolecular forces (bonds inside a molecule) and intermolecular forces (forces between separate molecules) when answering questions on physical properties like
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