Why don't noble gases normally form chemical bonds?

• A. They have the highest electronegativity in their respective periods.
• B. They readily lose electrons to achieve a stable configuration.
• C. They have a complete valence electron shell, resulting in very low electron affinity.
• D. Their atomic radii are too small to allow bonding with other elements.

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 noble gases do not form bonds: Since noble gases already have a complete valence shell, they are already in a stable, low-energy state and have little tendency to gain, lose, or share electrons.
4. Consider electron affinity and electronegativity: Noble gases have very low electron affinity because they do not easily attract additional electrons, and their electronegativity does not drive bonding as it does in other elements.
5. Conclude that the stability from a full valence shell explains why noble gases normally do not form chemical bonds.