Among the following species N2 N2 N2 N22 O2 O2 O2 O22 the

Question

Among the following species N_2, N_2^+, N_2^-, N_2^2-, O_2, O_2^+, O_2^-, O_2^2- the number of species showing diamagnesim is _______________.

DivineJEE · Accepted Answer

Those species which have unpaired electrons are called paramagnetic species.

And those species which have no unpaired electrons are called diamagnetic species.

(1)

N_2

has 14 electrons.

Moleculer orbital configuration of

N_2

=

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,{\sigma _{2p_z^2}}

Here no unpaired electron present, so it is diamagnetic.

(2) Moleculer orbital configuration of

N_2^{ + }

(13 electrons)

=

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,{\sigma _{2p_z^1}}

Here in

N_2^{ + }

, 1 unpaired electron present, so it is paramagnetic.

(3)

\mathrm{N}_{2}^{2-}

has 16 electrons.

Moleculer orbital configuration of

\mathrm{N}_{2}^{2-}

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z^2}}\,\,{\pi _{2p_x^2}}\,= \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * = \,\,\pi _{2p_y^1}^ *

Here 2 unpaired electron present, so it is paramagnetic.

(4)

\mathrm{N}_{2}^{-}

has 15 electrons.

Moleculer orbital configuration of

\mathrm{N}_{2}^{-}

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z^2}}\,\,{\pi _{2p_x^2}}\,= \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * = \,\,\pi _{2p_y^0}^ *

Here 1 unpaired electron present, so it is paramagnetic.

(a)

O_2^{2−}

has 18 electrons.

Moleculer orbital configuration of

O_2^{2−}

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\sigma _{2p_z^2}}\,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,\pi _{2p_x^2}^ * \, = \,\pi _{2p_y^2}^ *

Here is no unpaired electron so it is diamagnetic.

(b)

O_2^{−}

has 17 electrons.

Moleculer orbital configuration of

O_2^{2−}

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\sigma _{2p_z^2}}\,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,\pi _{2p_x^2}^ * \, = \,\pi _{2p_y^1}^ *

Here 1 unpaired electron present, so it is paramagnetic.

(c)

O_2

has 16 electrons.

Moleculer orbital configuration of

O_2

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z^2}}\,\,{\pi _{2p_x^2}}\,= \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * = \,\,\pi _{2p_y^1}^ *

Here 2 unpaired electron present, so it is paramagnetic.

(d)

O_2^{+}

has 15 electrons.

Moleculer orbital configuration of

O_2^{+}

is

{\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z^2}}\,\,{\pi _{2p_x^2}}\,= \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * = \,\,\pi _{2p_y^0}^ *

Here 1 unpaired electron present, so it is paramagnetic.

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