Covalent compounds are generally poor conductors of electricity. Why?

Academic Chemistry NCERT Class 10

Covalent compounds are formed by sharing electrons so they do not produce ions in solution or on melting. Hence, they are poor conductors of electricity.

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Updated on: 10-Oct-2022

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Covalent compounds generally don't conduct electricity. Give Reason.
Explain why:(a) Covalent compounds have generally low melting points.(b) Ionic compounds have generally high melting points.
Which of the following statements are correct for carbon compounds?(i) Most carbon compounds are good conductors of electricity (ii) Most carbon compounds are poor conductors of electricity.(iii) Force of attraction between molecules of carbon compounds is not very strong. (iv) Force of attraction between molecules carbon compounds is very strong.
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Generally, non-metals are not conductors of electricity, which of the following is a good conductor of electricity?FullerenesGraphiteDiamondSulphur
Giver Reason: Why Carbon can neither form C4+ cations nor C4- anions, but forms covalent compounds and are bad conductors of electricity and have low melting and boiling points?
Two examples of metals which are poor conductors of heat are _______, _____________.
(a) Explain why, ionic compounds conduct electricity in solution whereas covalent compounds do not conduct electricity.(b) Which of the following will conduct electricity and which not?MgCl2, CCl4, NaCl, CS2, Na2S
……… are the good conductors of heat and electricity.
(a) State the reason why carbon can neither form C4+ cations nor C4– anions, but forms covalent bonds. Also state reasons to explain why covalent compounds (i) are bad conductors of electricity.(ii) have low melting and boiling points.(b) Write the structural formula of benzene, C6H6.
Give two examples each: The metals that are good conductors and poor conductors of heat, respectively.
Covalent compounds have low melting and boiling point. Why?
(a) Giving one example each, state what are (i) ionic compounds, and (ii) covalent compounds.(b) Compare the properties of ionic compounds and covalent compounds.
What are ionic compounds? Why do ionic compounds not conduct electricity in the solid-state?

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