Final answer:
The accurate statement about the octet rule is that fluorine, nitrogen, and oxygen can form varying numbers of bonds to satisfy the octet rule. Contrary to forming four covalent bonds, these elements adjust their bonding based on their needs to attain eight valence electrons, consistent with the electron configuration of a noble gas.
Step-by-step explanation:
The Octet Rule
The octet rule states that atoms tend to form compounds in ways that give them eight valence electrons, and thus the electron configuration of a noble gas. Exceptions to this rule include hydrogen, which seeks to complete two valence electrons based on the nearest noble gas helium, known as the duet rule. Other exceptions are boron and aluminum which can have less than eight valence electrons and elements in period 3 and beyond that can exceed the octet due to the presence of d and f orbitals.
The correct answer to the question is: d. Fluorine, nitrogen, and oxygen can form more or less than four bonds and still satisfy the octet rule. This is because the number of covalent bonds nonmetals form is based on the number of valence electrons required to reach an octet, not necessarily four bonds. For instance, nitrogen typically forms three covalent bonds, as seen in N₂, and oxygen typically forms two, as in O₂.
Exceptions to the Octet Rule
While halogens like fluorine typically form a single bond as in F₂, and thus are not common exceptions to the octet rule, other heavier group 13 elements such as boron can have less than an octet, and elements of period 3 and beyond can exceed the octet. This is due to their ability to utilize available d or f orbitals to accommodate additional valence electrons.