Magnetic nature of C2 molecule will be A) paramagnetic (1.7BM) B) diamagnetic C) paramagnetic(2.8BM) D) paramagnetic(3.8BM)?

Question

Answer

The C2 molecule is diamagnetic because all electrons are paired there are no unpaired electrons.Hence opt B is correct

Answer

The C2 molecule is diamagnetic because all electrons are paired...

Answer

If the electronic configuration of a molecule has only one paired or spin paired electrons then that molecule is said to be diamagnetic molecule Here C2 has all paired in electronic configuration so it is diamagnetic

Answer

Introduction:
The magnetic nature of the C2 molecule can be determined by analyzing its electronic configuration and molecular orbital theory.

Diamagnetic and Paramagnetic:
Diamagnetic substances have all of their electrons paired up in their orbitals, resulting in a net magnetic moment of zero. Paramagnetic substances have at least one unpaired electron in their orbitals, resulting in a net magnetic moment.

Electronic Configuration of C2 Molecule:
The C2 molecule has a total of 12 valence electrons, with each carbon atom having six valence electrons. The electronic configuration of the C2 molecule is (σ1s)2 (σ1s*)2 (σ2s)2 (σ2s*)2 (π2px)2 (π2py)2.

Molecular Orbital Theory:
The C2 molecule has a total of six molecular orbitals, three bonding and three antibonding. The molecular orbitals are σ1s, σ2s, π2px, π2py, σ1s*, and σ2s*. The bonding molecular orbitals are filled first, followed by the antibonding molecular orbitals.

Analysis of Magnetic Nature:
The C2 molecule has a total of two unpaired electrons in its π2px and π2py molecular orbitals. Therefore, the C2 molecule is paramagnetic. The magnetic moment of the C2 molecule is 1.7BM.

Conclusion:
In conclusion, the C2 molecule is paramagnetic due to the presence of two unpaired electrons in its π2px and π2py molecular orbitals. The magnetic moment of the C2 molecule is 1.7BM.

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