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In Which of the following ionisation processes the bond energy increases and the magnetic behavior changes from paramagnetic to diamagnetic?

  • Option 1)

    N_{2}\rightarrow N_{2}^{+}

  • Option 2)

    O_{2}\rightarrow O_{2}^{+}

  • Option 3)

    C_{2}\rightarrow C_{2}^{+}

  • Option 4)

    NO\rightarrow NO^{+}

 

Answers (1)

best_answer

As we learnt in 

Magnetic behavior of molecule -

If  all the molecular orbitals in a molecule are doubly occupied, the substance is diamagnetic

- wherein

However if one or more molecular orbital are singly occupied it is paramagnetic e.g. O2

 

 

Bond strength -

The energy required to break one mole of bonds of particular type in gaseous state is called bond energy or bond strength.

- wherein

The same amount of energy is released in the formation of one mol of particular bond.

 

 Bond energy \propto  Bond order

Electronic config of NO =   \sigma_{1s^{2}} \: \sigma ^{*}_{1s^{2}}\:\sigma_{2s^{2}} \:\sigma ^{*}_{2s^{2}}\:\pi^{2}_{2py^{2}}\: \pi^{2}_{2pz^{2}} \:\sigma^{2}_{px^{2}}\:\pi ^{\theta}_{2py^{1}}

\therefore B.O = \therefore \frac{1}{2}\left ( 10-5 \right )=2.5

 Electronic config of NO^{+} = \sigma_{1s^{2}} \:\sigma ^{*}_{1s^{2}}\:\sigma^2_{s^{2}}\:\sigma ^{*}_{2s^{2}}\:\pi^{2}_{py^{2}}\:\pi_{2pz}^{2} \:\sigma^{2}_{2px} \:\pi ^{\theta }_{2py^{2}}\:\pi^{\theta }_{2px}

\therefore B.O = \frac{1}{2}\left ( 10-4 \right )=3

Since there are no unpaired electrons in NOas there are in NO, NO+ is diamagnetic while NO is paramagnetic due to 1 unpaired electron.


Option 1)

N_{2}\rightarrow N_{2}^{+}

Incorrect

Option 2)

O_{2}\rightarrow O_{2}^{+}

Incorrect

Option 3)

C_{2}\rightarrow C_{2}^{+}

Incorrect

Option 4)

NO\rightarrow NO^{+}

Correct

Posted by

prateek

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