Question

which of the following is the correct orbital diagram for fluorine?

Explanation:

Fluorine has an atomic number of 9. Its electron configuration is \(1s^{2}2s^{2}2p^{5}\). According to Hund's rule, electrons will occupy degenerate orbitals (in the \(2p\) sub - shell here) singly before pairing up. The \(1s\) and \(2s\) orbitals are fully filled (each can hold 2 electrons with opposite spins). In the \(2p\) sub - shell (which has 3 orbitals), 4 electrons are paired (2 pairs) and 1 electron is unpaired.

Answer:

A.