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Riya Sood 4C wrote:Do C, N, O, and F always follow the octet guideline even if their formal charge is not 0?
Because they're located in period 2, where n=2, those atoms do not have access to an empty d-block where they can form bonds transcending the octet rule; therefore, they will pretty much always follow the octet rule in covalent bonding. Formal charge and octet rule aren't dependent on each other; the way you form an octet for C, N, O, or F will determine whether the formal charge is zero or not.
Yes, they have to follow the octet rule because they cannot have an expanded octet since they are in the second period and do not have the shell n=3. Therefore, they do not possess a d orbital which can hold up to 10 electrons and therefore allow the atom to expand its octet. Atoms in the first and second period only have up to 2p which can hold up to 6 electrons and thus they can only have a max of 8 electrons in their valence shell which is n=2 since the second shell only has the orbitals s and p.
Yes, I believe they have to follow the octet rule as they can only have valence electrons as many as eight. Formal charges definitely don't have to be 0, even though the formal charges that are close to 0 makes the molecule more stable.
C, N, O, and F must follow the octet rule at all times. Atoms can begin having expanded octets at period 3 or greater. Typical atoms with expanded octets include sulfur, phosphorus, and silicon (all of which are in period 3).
As Carbon, Nitrogen, Oxygen, and Fluorine are all located in period 2 of the periodic table, their valence electrons are found in n=2. Thus, they do not have the extra 3d subshell that would allow them to have an expanded octet an must follow the octet guideline. Furthermore, although we try to minimize it in Lewis Structures, you do not always have to have a formal charge of 0.
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