Which statement best explains why bromine (Br) is more likely than neon (Ne) to form a covalent bond?

• A. Bromine is a noble gas and does not readily form bonds, unlike neon.
• B. Both bromine and neon have incomplete valence shells, so they are equally likely to form covalent bonds.
• C. Bromine has seven valence electrons and needs one more to achieve a stable octet, while neon already has a complete octet.
• D. Neon is more reactive than bromine because it has a higher atomic number.

Answer: (C)

Verified step by step guidance

1. Identify the electron configurations of bromine (Br) and neon (Ne) to understand their valence electron arrangements.
2. Recall that neon is a noble gas with a complete octet (8 valence electrons), making it chemically stable and unlikely to form bonds.
3. Recognize that bromine has seven valence electrons, which means it needs one more electron to complete its octet and achieve stability.
4. Understand that atoms tend to form covalent bonds by sharing electrons to complete their valence shells and reach a stable octet configuration.
5. Conclude that bromine is more likely to form covalent bonds because it seeks to gain one electron to complete its octet, whereas neon already has a full valence shell and is chemically inert.