1

AIPMT 2015 Cancelled Paper

Which of the following species contains equal number of $\sigma$- and $\pi$-bonds ?
A
(CN)2
B
CH2(CN)2
C
HCO3$-$
D
XeO4

Explanation

Number of $\sigma$ bonds = 4

Number of $\pi$ bonds = 4
2

AIPMT 2015 Cancelled Paper

Maximum bond angle at nitrogen is present in which of the following ?
A
NO2+
B
NO3$-$
C
NO2
D
NO2$-$

Explanation

Species $NO_3^-$ $NO_2$ $NO_2^-$ $NO_2^+$
Hybridisation sp2 sp2 sp2 sp(linear)
Bond Angle 120o 134o 115o 180o
3

AIPMT 2015 Cancelled Paper

Which of the following pairs of ions are isoelectronic and isostructural ?
A
SO32$-$,  NO3$-$
B
ClO3$-$,  SO32$-$
C
CO32$-$, SO32$-$
D
ClO3$-$, CO32$-$,

Explanation

Species Hybridisation Shape No. of e-
$SO_3^{2-}$ sp3 Pyramidal 42
$ClO_3^{-}$ sp3 Pyramidal 42
$CO_3^{2-}$ sp2 Triangular planar 32
$NO_3^{-}$ sp2 Triangular planar 32
4

AIPMT 2015 Cancelled Paper

The correct bond order in the following species is
A
O2+ < O2$-$ < O22+
B
O2$-$ < O2+ < O22+
C
O22+ < O2+ < O2$-$
D
O22+ < O2$-$ < O2+

Explanation

$\,$ Bond order $= {1 \over 2}$ [Nb $-$ Na]

Nb = No of electrons in bonding molecular orbital

Na $=$ No of electrons in anti bonding molecular orbital

In O atom 8 electrons present, so in O2, 8 $\times$ 2 = 16 electrons present.

Then in $O_2^ +$ no of electrons = 15

in $O_2^ -$ no of electrons = 17

in $O_2^{2 + }$ no of electrons = 14

$\therefore\,\,\,\,$ Molecular orbital configuration of O2 (16 electrons) is

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

$\therefore\,\,\,\,$Na = 6

Nb = 10

$\therefore\,\,\,\,$ BO = ${1 \over 2}\left[ {10 - 6} \right] = 2$

Molecular orbital configuration of O$_2^ +$ (15 electrons) is

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

$\therefore\,\,\,\,$ Nb = 10

Na = 5

$\therefore\,\,\,\,$ BO = ${1 \over 2}\left[ {10 - 5} \right]$ = 2.5

Molecular orbital configuration of $O_2^ -$ (17 electrons) is

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

$\therefore\,\,\,\,$ Nb = 10

Na = 7

$\therefore\,\,\,\,$ BO = ${1 \over 2}\left[ {10 - 7} \right]$ = 1.5

Molecular orbital configuration of O $_2^{2 + }$ (14 electrons) is

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

$\therefore\,\,\,\,$ Nb = 10

Na = 4

$\therefore\,\,\,\,$ BO = ${1 \over 2}$ [ 10 $-$ 4] = 3

$O_2^-$ $O_2$ $O_2^+$ $O_2^{2+}$
B.O. : 1.5 2.0 2.5 3.0