Asked by: Jofre Huzangai
asked in category: General Last Updated: 8th June, 2020

Can covalent compounds conduct electricity?

Although solid ionic compounds do not conduct electricity because there are no free mobile ions or electrons, ionic compounds dissolved in water make an electrically conductive solution. In contrast, covalent compounds do not exhibit any electrical conductivity, either in pure form or when dissolved in water.

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Herein, why do covalent bonds not conduct electricity?

Covalent compounds do not conduct electricity because they are formed between non metal atoms by sharing of electrons. Covalent compounds have no free electrons and no ions and hence they do not conduct electricity.

Subsequently, question is, can giant covalent bonds conduct electricity? Most substances with giant covalent structures have no charged particles that are free to move. This means that most cannot conduct electricity. Graphite, a form of carbon which can conduct electricity, is an exception. State three properties that are typical of substances with giant covalent structures.

Hereof, why can some covalent compounds conduct electricity?

Covalent compounds form when atoms that have similar electronegativity values form covalent chemical bonds. Because there are no free electrons or ions in the water (electrolytes) dissolved covalent compounds can't conduct electricity. Similarly, covalent compounds aren't conductive in pure form either.

Can metallic compounds conduct electricity?

They are hard and brittle, they are not malleable or ductile (i.e. cannot be shaped without cracking/breaking), and they do not conduct electricity. Metallic bonding describes a lattice of positively charged ions, surrounded by a mobile 'sea' of valence electrons.

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