Among H2, He2^+, Li2, Be2, B2, C2, N2, O2 and F2, the number of diamagnetic species is (Atomic

step 1 Among these compounds, the number of diametic species is. So we have to check how many diametic

Among H2, He2^+, Li2, Be2, B2, C2, N2, O2 and F2, the...

Among $\mathrm{H}_{2}, \mathrm{He}_{2}^{+}, \mathrm{Li}_{2}, \mathrm{Be}_{2}, \mathrm{~B}_{2}, \mathrm{C}_{2}, \mathrm{~N}_{2}, \mathrm{O}_{2}$ and $\mathrm{F}_{2}$, the number of diamagnetic species is (Atomic numbers: $\mathrm{H}=1, \mathrm{He}=2, \mathrm{Li}=3, \mathrm{Be}=4, \mathrm{~B}=5, \mathrm{C}=6, \mathrm{~N}=7, \mathrm{O}=8$, $\mathrm{F}=9$ )

Among $\mathrm{H}_{2}, \mathrm{He}_{2}^{+}, \mathrm{Li}_{2}, \mathrm{Be}_{2}, \mathrm{~B}_{2}, \mathrm{C}_{2}, \mathrm{~N}_{2}, \mathrm{O}_{2}$ and $\mathrm{F}_{2}$, the number of
diamagnetic species is (Atomic numbers: $\mathrm{H}=1, \mathrm{He}=2, \mathrm{Li}=3, \mathrm{Be}=4, \mathrm{~B}=5, \mathrm{C}=6, \mathrm{~N}=7, \mathrm{O}=8$,
$\mathrm{F}=9$ )

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Key Concepts

Diamagnetism

Diamagnetism is a property of a substance whose electrons are all paired, resulting in a net zero magnetic moment. Diamagnetic species are weakly repelled by magnetic fields and do not have any unpaired electrons, which is key to identifying them in molecular orbital diagrams.

Paramagnetism

Paramagnetism occurs when a molecule has one or more unpaired electrons. The presence of these unpaired electrons imparts a net magnetic moment to the species, causing it to be attracted to magnetic fields. Understanding which molecular orbital configurations lead to unpaired electrons is essential for predicting paramagnetic behavior.

Molecular Orbital Theory

Molecular Orbital Theory is a framework for describing the electronic structure of molecules by constructing molecular orbitals that are delocalized over the entire molecule. These orbitals, formed from the linear combination of atomic orbitals, can be bonding, antibonding, or nonbonding and determine the stability, bond order, and magnetism of the molecule.

Electron Configuration

Electron configuration in molecules involves the orderly filling of molecular orbitals with electrons according to principles like the Aufbau principle, Pauli exclusion principle, and Hund’s rule. This configuration is crucial in determining whether electrons are unpaired or paired in a molecule.

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