In which of the following molecules does the molecular orbital configuration sho

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Question: In which of the following molecules does the molecular orbital configuration show unpaired electrons?

Options:

Correct Answer: O2

Solution:

O2 has two unpaired electrons in its π* orbitals, making it paramagnetic.

In which of the following molecules does the molecular orbital configuration show unpaired electrons?

In which of the following molecules does the molecular orbital configuration show unpaired electrons?

Step 1: Understand what unpaired electrons are. Unpaired electrons are electrons that are alone in an orbital and not paired with another electron.
Step 2: Know that molecular orbitals are formed when atomic orbitals combine. Electrons fill these orbitals according to specific rules.
Step 3: Identify the molecule in question, which is O2 (oxygen gas).
Step 4: Write the electron configuration for O2. Oxygen has 8 electrons, so O2 has a total of 16 electrons.
Step 5: Fill the molecular orbitals for O2 according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
Step 6: After filling the orbitals, check the π* (pi star) orbitals. In O2, there are 2 electrons in the π* orbitals.
Step 7: Determine if these electrons are paired or unpaired. In O2, the two electrons in the π* orbitals are unpaired.
Step 8: Conclude that O2 has unpaired electrons, which makes it paramagnetic (it is attracted to a magnetic field).

Molecular Orbital Theory – This theory explains the behavior of electrons in molecules, including the formation of bonding and antibonding orbitals.
Paramagnetism vs. Diamagnetism – Paramagnetic substances have unpaired electrons and are attracted to magnetic fields, while diamagnetic substances have all paired electrons and are repelled.