11. Among the following molecules, which one contains the fewest covalent bonds?
Answer: C
Chlorine molecule (Cl2) contains the fewest covalent bonds.
The chlorine molecule (Cl2) consists of a single covalent bond that connects the two chlorine atoms. This bond is formed by the sharing of one pair of electrons, making it the molecule with the fewest covalent bonds among the options provided.
A) Water molecule (H2O)
The water molecule (H2O) contains two covalent bonds. Each hydrogen atom forms a single covalent bond with the oxygen atom, resulting in a total of two bonds. Therefore, it has more covalent bonds than the chlorine molecule.
B) Methane molecule (CH4)
The methane molecule (CH4) consists of four covalent bonds. Each hydrogen atom is bonded to the carbon atom through a single covalent bond, leading to a total of four bonds. This makes it have significantly more bonds than Cl2.
C) Chlorine molecule (Cl2)
The chlorine molecule (Cl2) is comprised of only one covalent bond, which is formed between the two chlorine atoms. This makes it the molecule with the fewest covalent bonds compared to the other options listed.
D) Ammonia molecule (NH3)
The ammonia molecule (NH3) contains three covalent bonds. Each of the three hydrogen atoms is bonded to the nitrogen atom through single covalent bonds, resulting in three total bonds. Thus, ammonia has more covalent bonds than the chlorine molecule.
Conclusion
The chlorine molecule (Cl2) is the only option with a single covalent bond, making it the molecule with the fewest covalent bonds. In contrast, all other options—water, methane, and ammonia—contain multiple covalent bonds, confirming that C is the correct answer.