According to molecular orbital theory, paramagnetism of {O₂} molecule is due to presence of

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4.Chemical Bonding and Molecular Structure

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According to molecular orbital theory, the paramagnetism of ${O_2}$ molecule is due to presence of

Unpaired electrons in the bonding $\sigma $ molecular orbital

Unpaired electrons in the antibonding $\sigma $ molecular orbital

Unpaired electron in the bonding $\pi $ molecular orbital

Unpaired electrons in the antibonding $\pi $ molecular orbital

Solution

The reason that it is paramagnetic is because the oxygen molecule has two unpaired electrons. Electrons not only go around the atom in their orbitals, they also spin, which creates a magnetic field. The reason that it is paramagnetic is because the oxygen molecule has two unpaired electrons. The last two electrons go into separate, degenerate $\pi$ orbitals, according to Hund's Rule. Thus, oxygen has two unpaired electrons and is paramagnetic

Standard 11

Chemistry

Among the following, the molecule expected to be stabilized by anion formation is

normal

(JEE MAIN-2019)

Give electron configuration, Magnetic property, bond order and energy diagram for carbon $\left( {{{\rm{C}}_2}} \right)$.

normal

Which of the following statement is correct for peroxide ion

$A.$ has completely filled antibonding molecular orbitals
$B.$ is diamagnetic
$C.$ has bond order one
$D.$ is isoelectronic with Neon

hard

Select incorrect statement

hard

Maximum unpaired electrons are present in