Valence and bonding of noble gases Neon (Ne) has a complete outer shell with eight valence electrons. How many covalent bonds does Ne readily form under standard conditions?

Introduction / Context:
Noble gases such as neon, argon, and helium are often described as inert because their valence shells are filled, making them exceptionally stable and unreactive. Understanding why a filled octet discourages covalent bond formation clarifies periodic trends, Lewis structures, and reactivity patterns in general chemistry.

Given Data / Assumptions:

• Neon's electron configuration is 1s^2 2s^2 2p^6 (full octet in the n = 2 shell).
• Standard conditions imply no extreme pressures, temperatures, or plasma states.
• We consider ordinary covalent bonding behavior.

Concept / Approach:
Atoms form covalent bonds to attain a lower energy state, often by achieving a filled valence shell. Neon already has a filled octet, so there is no energetic drive to share electrons. Consequently, Ne resists forming stable covalent compounds and remains monatomic. Rare exceptions of noble-gas compounds exist primarily for heavier noble gases (e.g., xenon) under special conditions; neon compounds are essentially unknown and unstable.

Step-by-Step Solution:

Verification / Alternative check:
Experimental chemistry catalogs show no stable neutral neon covalent compounds. Contrast with xenon fluorides (formed under extreme conditions) to see how heavier noble gases can be coerced into bonding, whereas neon remains inert.

Why Other Options Are Wrong:

• One, two, four, eight: all imply electron sharing to reach stability, which neon already possesses.

Common Pitfalls:
Overgeneralizing noble-gas chemistry from xenon to neon; heavier noble gases have accessible d orbitals and lower ionization energies, enabling limited compound formation unlike neon.

Final Answer:
None