EVERYDAY SCIENCE

Detailed explanation-1: -Covalent compounds are generally poor conductors of electricity: During the formation of a covalent bond, when the electrons get shared within the bonds, hence, there are no electrons or ions available to conduct electricity.

Detailed explanation-2: -Covalent compounds do not conduct electricity; this is because covalent compounds do not have charged particles capable of transporting electrons. Lewis theory also accounts for bond length; the stronger the bond and the more electrons shared, the shorter the bond length is.

Detailed explanation-3: -Covalent molecular structures do not conduct electricity because the molecules are neutral and there are no charged particles (no ions or electrons) to move and carry charge.

Detailed explanation-4: -b. Covalent compounds do not conduct electricity even when molten because the resultant mobile particles are neutral molecules. Their movement cannot be used to carry an electric charge. Metals conduct electricity in the solid state because the valence electrons of the atoms generate a mobile “sea” of electrons.

Detailed explanation-5: -Covalent compounds (solid, liquid, solution) do not conduct electricity. Metal elements and carbon (graphite) are conductors of electricity but non-metal elements are insulators of electricity. Ionic bonds are the electrostatic attraction between positive and negative ions.