Why do covalent compounds generally not conduct electricity? ((A)) They have high melting points and therefor…

Question

Why do covalent compounds generally not conduct electricity?
((A)) They have high melting points and therefore resist electron flow.
((B)) They exist as molecules with no free ions or electrons to carry charge.
((C)) They dissolve in water to form neutral solutions.
((D)) Their molecules are too large to allow electron movement.

Accepted Answer

## Model Answer **(B)** Electrons are shared between atoms so no charged particles (ions) are formed. Covalent compounds exist as molecules; since electrons are shared, no free ions or electrons are produced to carry electric charge, making them poor conductors. *Source: Carbon and its Compounds, Section 4.1* ## Explanation The textbook states: *"Since the electrons are shared between atoms and no charged particles are formed, such covalent compounds are generally poor conductors of electricity."* Examiners expect you to link **electron sharing → no ions formed → no charge carriers → poor conduction**. Option B matches this exactly. Options A and C are incorrect (covalent compounds have *low* melting points); Option D is not a reason given in the text.

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