Why are ionic compounds good conductors of electricity?

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Blake Zieme asked a question: Why are ionic compounds good conductors of electricity?
Asked By: Blake Zieme
Date created: Mon, Mar 29, 2021 8:13 AM
Date updated: Thu, Jun 23, 2022 5:50 AM

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Top best answers to the question «Why are ionic compounds good conductors of electricity»

  • only when ionic compounds are broken into ions (by melting them at v. high temperatures or dissolving them into a solvent) they conduct electricity by displacement of ions. -unlike metals, they do not have free electrons to conduct electricity. -unlike ionic compounds, they can not be broken up into two charged particles. Rate! Rate!

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Generally, ionic compounds are better conductors of heat (and electricity) when in molten form or when dissolved in the water. Metals are also good conductors of heat due to the availability of electrons that can vibrate and also move around.

Explanation: Ionic compounds conduct electricity when molten (liquid) or in aqueous solution (dissolved in water), because their ions are free to move from place to place. Ionic compounds are conductors of electricity when molten or in solution, and insulators when solid.

Why are ionic compounds good conductors of electricity? a. The strong electrostatic attraction between ions allows electricity to flow freely b. Aqueous solutions of ionic compounds cause ions to dissociate and are free to conduct electricity.

Why are ionic compounds good conductors? Ionic compounds conduct electricity when molten (liquid) or in aqueous solution (dissolved in water), because their ions are free to move from place to place. Ionic compounds are conductors of electricity when molten or in solution, and insulators when solid.

Why are ionic compounds good conductors of electricity - 13427238 maskone1968 maskone1968 15.04.2021 Science Junior High School answered Why are ionic compounds good conductors of electricity 2 See answers donnabelle37 donnabelle37 ...

Why are most ionic compounds good conductors of electricity? - 9061351 aanyakkumar3152 aanyakkumar3152 28.03.2019 Chemistry Secondary School answered Why are most ionic compounds good conductors of electricity? 2 See answers Advertisement

Yes ;Ionic compounds are good conductors of electricity because ionic compounds dissociate into ions in molten or aqueous solution and these ions are responsible for the conduction … Something went wrong.

In summary, ionic compounds don't conduct electricity very well because the charge carriers can't move through the crystal. They can conduct heat because the kinetic energy itself is the "heat carrier" - it can be transferred without moving ions too far from their mean positions.

Why are ionic compounds good conductors of electricity? - 12383052 aizamagarao aizamagarao 19.03.2021 Science Senior High School answered Why are ionic compounds good conductors of electricity? 1 See answer Advertisement ...

Ionic compounds conduct electricity when dissolved in water because the movement of their negatively-charged and positively-charged particles forms an electrical current, explains About.com.

Why are ionic compounds good conductors of electricity? a. The strong electrostatic attraction between ions allows electricity to flow freely. b. Aqueous solutions of ionic compounds cause ions to dissociate and are free to conduct electricity.

5. Why are ionic compounds good conductors of electricity? a. The strong electrostatic attraction between ions allows electricity to freely flow b. Aqueous solutions of ionic compounds causesto ions dissociate and are free to conduct electricity. C. Strong electrostatic attraction between crystal lattice of ionic compounds is

Ionic compounds do not conduct electricity. only when ionic compounds are broken into ions (by melting them at v. high temperatures or dissolving them into a solvent) they conduct electricity by displacement of ions. covalent compounds do not conduct electricity because: -unlike metals, they do not have free electrons to conduct electricity.

Ionic compounds, like NaCl or MgSO4, form crystal lattices in a solid state. Thus, there are no moving bits. The +ves and the -ves are bound firmly to each other. There are no delocalised electrons, as in metals or some covalent structures, so they can't migrate either.

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