Chemistry, asked by maitysayan333, 9 months ago

NO is paramagnetic and NO+ is diamagnetic..justify using MO configuration

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Answered by drpanditds
1

Answer:

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Answered by aryansuts01
0

Answer:

Concept:

A molecular orbital diagram, often known as a MO diagram, is a qualitative descriptive tool used to explain chemical bonding in molecules using the linear combination of atomic orbitals (LCAO) approach and general molecular orbital theory. These theories are based on the fundamental idea that as atoms join together to form molecules, a specific number of atomic orbitals combine to create the same number of molecular orbitals, even though the orbitals' electrons may be distributed differently. When discussing even comparatively simple polyatomic compounds, like methane, this method gets more complicated. It works very well for simple diatomic molecules like dihydrogen, dioxygen, and carbon monoxide.

Given:

NO is paramagnetic and NO+ is diamagnetic. justify using MO configuration

Find:

Find the answer for the given question

Answer:

The odd electron in nitric oxide causes it to be paramagnetic (unpaired electron). When this electron is lost, the diamagnetic NO+ is created.

There are no unpaired electrons in the MO configuration of the isoelectronic species CN-, CO, and NO+ because they each have 14 electrons. They are hence diamagnetic.

All of the electrons in the NO molecule cannot be paired because their number is odd. Its single unpaired electron makes it paramagnetic.

When exposed to a magnetic field, diamagnetic materials are partially repulsed and lose their magnetic properties when the external field is removed. When exposed to a magnetic field, paramagnetic materials are only weakly drawn to it; once the external field is removed, the materials lose their magnetic qualities.

By looking at a substance's electron configuration, one can identify whether or not it has magnetic qualities. A substance is paramagnetic if any of its electrons are unpaired; it is diamagnetic if all of its electrons are paired.

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