Hund's rule states that within a subshell, electrons
Correct answer: B. occupy separate orbitals singly with parallel spins before any pairing occurs
- A. pair up in the lowest orbital first
- B. occupy separate orbitals singly with parallel spins before any pairing occurs
- C. always have opposite spins
- D. fill the highest energy orbital first
Explanation
Spreading out into empty orbitals minimises electron electron repulsion, so nitrogen's three 2p electrons occupy the three separate p orbitals rather than crowding two into one. This is why so many transition metal ions are paramagnetic. Pairing only begins once every orbital in the subshell holds one electron.
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About Electronic Configuration
Electronic configuration describes how electrons occupy shells, subshells and orbitals around an atom. Questions use the Aufbau principle, Pauli exclusion principle and Hund's rule to write configurations, identify valence electrons, form ions and explain periodic trends, including common exceptions such as chromium and copper.
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