In Lewis dot structures, when are multiple bonds (double or triple bonds) required between atoms?

• A. When all atoms in the molecule are metals
• B. When there are not enough electrons to satisfy the octet rule for all atoms using only single bonds
• C. When the molecule contains only hydrogen and helium
• D. When atoms have more than eight valence electrons

Answer: (B)

Verified step by step guidance

1. Understand that Lewis dot structures represent valence electrons around atoms to show bonding and lone pairs.
2. Recall the octet rule, which states that atoms (especially nonmetals) tend to form bonds to have eight electrons in their valence shell.
3. Recognize that single bonds involve sharing one pair of electrons between two atoms, but sometimes this is not enough to satisfy the octet rule for all atoms in the molecule.
4. When there are not enough electrons to complete the octet for all atoms using only single bonds, multiple bonds (double or triple bonds) are introduced to share more electron pairs between atoms.
5. Note that multiple bonds increase the number of shared electrons, helping atoms achieve a full octet and a more stable electronic configuration.