Which of the following types of molecules conduct electricity when dissolved in water?

• A. Nonpolar molecules such as O2
• B. Ionic compounds such as NaCl
• C. Covalent compounds such as C6H12O6 (glucose)
• D. Organic acids such as CH3COOH (acetic acid) in pure form

Answer: (B)

Verified step by step guidance

1. Understand that electrical conductivity in aqueous solutions depends on the presence of charged particles (ions) that can move freely to carry electric current.
2. Recognize that nonpolar molecules like O\_2 do not ionize or produce ions in water, so they do not conduct electricity.
3. Know that ionic compounds such as NaCl dissociate into their constituent ions (Na\^+ and Cl\^- ) when dissolved in water, allowing the solution to conduct electricity.
4. Realize that covalent compounds like C\_6H\_{12}O\_6 (glucose) dissolve as whole molecules without producing ions, so they do not conduct electricity.
5. Note that organic acids like CH\_3COOH (acetic acid) in pure form are not ionized and thus do not conduct electricity; however, when dissolved in water, they partially ionize and can conduct electricity to some extent.