Which of the following best explains why noble gases do not normally form chemical bonds?

• A. They have the highest atomic radii in their respective periods, preventing bonding.
• B. They have the lowest ionization energies, making them highly reactive.
• C. They have a complete valence electron shell, resulting in very low electron affinity.
• D. They possess unpaired electrons that repel other atoms.

Answer: (C)

Verified step by step guidance

1. Understand the electronic configuration of noble gases: Noble gases have a full valence shell, meaning their outermost electron shell is completely filled with electrons.
2. Recall the concept of chemical bonding: Atoms tend to form bonds to achieve a more stable electron configuration, usually by filling or emptying their valence shell.
3. Analyze why a complete valence shell affects bonding: Since noble gases already have a stable, full valence shell, they have little tendency to gain, lose, or share electrons with other atoms.
4. Consider ionization energy and electron affinity: Noble gases have high ionization energies (not low) and very low electron affinities, meaning they do not easily lose or gain electrons, which reduces their reactivity.
5. Conclude that the best explanation is that noble gases do not normally form chemical bonds because they have a complete valence electron shell, resulting in very low electron affinity and high stability.