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Please,please help me In Which of the following ionisation processes the bond energy increasesand the magnetic behavior changes from paramagnetic to diamagnetic?

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 (2)
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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

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

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