Which of the following best describes the magnetic properties of F_2, and why?

• A. F_2 is diamagnetic because all electrons are paired in its molecular orbitals.
• B. F_2 is paramagnetic because it has unpaired electrons in its molecular orbitals.
• C. F_2 is diamagnetic because it contains unpaired electrons.
• D. F_2 is paramagnetic because it has a net magnetic moment.

Answer: (A)

Verified step by step guidance

1. Recall that the magnetic properties of a molecule depend on the presence or absence of unpaired electrons in its molecular orbitals.
2. Understand that diamagnetic substances have all electrons paired, resulting in no net magnetic moment, while paramagnetic substances have one or more unpaired electrons, causing a net magnetic moment.
3. Determine the electron configuration of the F_2 molecule by filling its molecular orbitals according to the molecular orbital theory, starting from the lowest energy orbitals and moving to higher ones.
4. Count the number of unpaired electrons in the molecular orbitals of F_2 after filling all electrons; if all electrons are paired, the molecule is diamagnetic.
5. Conclude that since F_2 has all electrons paired in its molecular orbitals, it is diamagnetic, which explains its magnetic behavior.