Chemistry

Question Analysis
This question involves comparing ionic and covalent compounds and explaining how bonding type affects conductivity when dissolved in water.

Key Concept Explanation
Ionic compounds dissociate into free-moving ions when dissolved in water. These ions can carry electric charge, allowing the solution to conduct electricity.
Covalent molecular compounds usually dissolve as neutral molecules and do not produce charge carriers.

Step-by-step Solution
1. Classify the bond type of each substance:
KNO₃ (potassium nitrate): An ionic compound composed of K⁺ and NO₃⁻ ions.
C₆H₁₂O₆ (glucose): Covalent molecular compound (all bonds are covalent, forming neutral molecules).
2. Analyze the dissolution behavior in water:
KNO₃: When dissolved in water, it dissociates into ions (K⁺ and NO₃⁻). The free-moving ions allow the solution to conduct electricity.
C₆H₁₂O₆: When dissolved, it remains as neutral molecules. No ions are present to carry electric charge.
3. Conclusion:
KNO₃ is more likely to conduct elect...