In Lewis dot structures, when is it appropriate to form double or triple bonds between atoms?

• A. When single bonds do not satisfy the octet rule for all atoms involved.
• B. If the atoms have the same electronegativity.
• C. Only when the molecule contains hydrogen atoms.
• D. Whenever two nonmetals are present in a molecule.

Answer: (A)

Verified step by step guidance

1. Understand that Lewis dot structures are used to represent the valence electrons of atoms in a molecule and how they share electrons to form bonds.
2. Recall the octet rule, which states that atoms tend to form bonds until they are surrounded by eight electrons (except for hydrogen, which follows the duet rule).
3. Recognize that single bonds involve sharing one pair of electrons, but sometimes this is not enough to satisfy the octet rule for all atoms in the molecule.
4. When single bonds do not provide enough shared electrons to complete the octet for all atoms, double or triple bonds are formed by sharing two or three pairs of electrons respectively.
5. Note that the formation of multiple bonds depends on the need to satisfy the octet rule rather than the electronegativity of atoms, presence of hydrogen, or simply the presence of two nonmetals.