QQuestionChemistry
QuestionChemistry
Why do ionic compounds conduct electricity when dissolved in water, but most covalent compounds do not?
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this problem step by step, explaining the key concepts behind ionic and covalent compound electrical conductivity:
Step 2:: Understanding Ionic Compounds
\mathrm{NaCl} \rightarrow \mathrm{Na}^{+} + \mathrm{Cl}^{-}
Ionic compounds are composed of positively and negatively charged ions held together by electrostatic attraction. When dissolved in water, these ions can separate and move freely.
Step 3:: Dissociation in Water
\mathrm{H}_{2}\mathrm{O} \text{ helps } \mathrm{NaCl} \rightarrow \mathrm{Na}^{+} + \mathrm{Cl}^{-}
When an ionic compound dissolves in water, the water molecules (which are polar) break apart the ionic bonds, separating the ions.
Step 4:: Charge Carriers
The separated ions act as charge carriers. Positively charged ions (cations) move toward the negative electrode, while negatively charged ions (anions) move toward the positive electrode.
Step 5:: Covalent Compounds
\mathrm{H}_{2}\mathrm{O} \text{ remains as } \mathrm{H}_{2}\mathrm{O \text{ molecules}}
In contrast, covalent compounds share electrons and do not form ions. When dissolved, they typically remain as intact molecules.
Step 6:: Electrical Conductivity Mechanism
- Ionic compounds: Free-moving ions can conduct electricity - Covalent compounds: No free-moving charged particles to conduct electricity
Final Answer
Ionic compounds conduct electricity when dissolved in water because the dissolved ions can move freely and act as charge carriers, while most covalent compounds do not conduct electricity because they do not form mobile ions when dissolved.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students