Which of the following best explains whether a stable compound can be formed between a sodium (Na) atom and a chlorine (Cl) atom?

• A. Yes, because sodium and chlorine share electrons equally to form a covalent bond.
• B. Yes, because sodium can transfer an electron to chlorine, forming a stable ionic bond.
• C. No, because both atoms have full valence shells and cannot bond.
• D. No, because sodium and chlorine are both metals and do not react.

Answer: (B)

Verified step by step guidance

1. Identify the types of elements involved: Sodium (Na) is a metal and chlorine (Cl) is a nonmetal.
2. Recall that metals tend to lose electrons to achieve a full valence shell, while nonmetals tend to gain electrons.
3. Understand that sodium has one electron in its outer shell and chlorine has seven electrons in its outer shell.
4. Recognize that sodium can transfer its one valence electron to chlorine, allowing sodium to achieve a full shell (like neon) and chlorine to complete its octet.
5. Conclude that this electron transfer results in the formation of oppositely charged ions (Na⁺ and Cl⁻), which attract each other to form a stable ionic bond.