Which of the following elements typically do not naturally form chemical bonds under standard conditions?

• A. Neon (Ne)
• B. Oxygen (O)
• C. Chlorine (Cl)
• D. Nitrogen (N)

Answer: (A)

Verified step by step guidance

1. Understand the concept of chemical bonding: Atoms form chemical bonds to achieve a more stable electron configuration, often by filling their outermost electron shell.
2. Identify the electron configuration of each element: Neon (Ne) has a full outer shell (a complete octet), while Oxygen (O), Chlorine (Cl), and Nitrogen (N) have incomplete outer shells and tend to form bonds to achieve stability.
3. Recognize that noble gases like Neon are chemically inert under standard conditions because their valence shells are already full, making them unlikely to form bonds naturally.
4. Compare the reactivity of the elements: Oxygen, Chlorine, and Nitrogen are all reactive nonmetals that commonly form covalent bonds to complete their octets.
5. Conclude that Neon (Ne) typically does not form chemical bonds under standard conditions due to its stable electron configuration.