Please be patient as the PDF generation may take upto a minute.

Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule $B_2$ is
(1) 1 and diamagnetic
(2) 0 and diamagnetic
(3) 1 and paramagnetic
(4) 0 and paramagnetic

Out of the two compounds shown below, the vapour pressure of B at a particular temperature is expected to be

1. higher than that of A
2. lower than that of A
3. same as that of A
4. can be higher or lower depending upon the size of the
vessel
 

Which of the following pairs of species would you expect to have largest difference in spin only magnetic moment ?
(1) $O_2, O_2^{+}$
(2) $O_2, O_2^{2-}$
(3) $O_2^{+}, O_2^{2-}$
(4) $O_2^{-}, O_2^{+}$

The correct order of the bond angles is :-
1. ${\mathrm{NH}}_3>{\mathrm{H}}_2\mathrm{O}>{\mathrm{PH}}_3>{\mathrm{H}}_2\mathrm{S}$
2. ${\mathrm{NH}}_3>{\mathrm{PH}}_3>{\mathrm{H}}_2\mathrm{O}>{\mathrm{H}}_2\mathrm{S}$
3. ${\mathrm{NH}}_3>{\mathrm{H}}_2\mathrm{S}>{\mathrm{PH}}_3>{\mathrm{H}}_2\mathrm{O}$
4. ${\mathrm{PH}}_3>{\mathrm{H}}_2\mathrm{S}>{\mathrm{NH}}_3>{\mathrm{H}}_2\mathrm{O}$

The volatility of HF is low as compare to other Hydra
acid of Halogen because of :-
1. its low polarizability
2. the weak dispersion interaction between the molecules
3. its small molecular mass
4. its strong hydrogen bonding

The experimental value of the dipole moment of HCl is
1.03 D. The length of the H – Cl bond is 1.275 Å. The
percentage of ionic character in HCl is :-
1. 43 
2. 21
3. 17 
4. 7

In which of the following compound all the bond angles are equal :-
(1) $S{F}_4$                              (2) $CC{l}_4$
(3) $CHC{l}_3$                         (4) $Xe{F}_6$

The structure of diborane (B₂H₆) contains :-
1. four (2c – 2e^–) bonds and two (2c – 3e^–) bonds
2. two (2c – 2e^–) bonds and two (3c – 2e^–) bonds
3. four (2c – 2e^–) bonds and four (3c – 2e^–) bonds
4. none

In which of the following is not correctly match between given species and type of overlapping ?
(1) $Xe{O}_3$: Three $(d\mathrm{\pi }-\mathrm{p\pi })$ bonds
(2) $H_{2}S{O}_4$: Two $(d\mathrm{\pi }-\mathrm{p\pi })$ bonds
(3) $S{O}_3$: Three $(d\mathrm{\pi }-\mathrm{p\pi })$ bonds
(4) $HCl{O}_4:$ Three $(d\mathrm{\pi }-\mathrm{p\pi })$ bonds

B₃N₃H₆ + solution of hydrochloric acid $\to$ ?
Select correct about above reaction :
1. no reaction
2. B₃N₃H₆ show substitution reaction & produce B₃N₃Cl₆
3. B₃N₃H₆ show addition reaction and produce B₃N₃H₉Cl₃
in which Cl is bonded to boron
4. B₃N₃H₆ show addition reaction and produce B₃N₃H₉Cl₃
in which Cl is bonded to nitrogen
 

Which of the following compounds have the same no. of
lone pairs with their central atom :-
(I) XeF₅^–
(II) BrF₃
(III) XeF₂
(IV) Triple methylene
1. (IV) and (V) 
2. (I) and (III)
3. (I) and (II) 
4. (II), (IV) and (V

Consider the following compounds and select the incorrect statement from the following:
$N{H}_3, P{H}_3, H_{2}S, S{O}_2,$$S{O}_3, B{F}_3, PC{l}_3,I{F}_7, P_4, H_2$
(1) 3 molecules out of given compounds involve $S{p}^2$ hybridisation.
(2) Three molecules are hyprevalent compounds.
(3) Six molecules out of above compounds are non-planar in structure
(4) Two molecules out of given compounds involves $\left(d\mathrm{\pi }-\mathrm{p\pi }\right)$ bonding as well as also involves $\left(p\mathrm{\pi }-\mathrm{p\pi }\right)$ bonding.

The molecular orbital configuration of CN⁺ is :-
1. $\mathrm{KK} \mathrm{\sigma }\left(2{\mathrm{s}}^2\right),{\mathrm{\sigma }}^{*}\left(2{\mathrm{s}}^2\right),\mathrm{\pi }{(2\mathrm{p}}^{}$_x)2,π(2p_y)2
2. $\mathrm{KK} \mathrm{\sigma }\left(2{\mathrm{s}}^2\right),{\mathrm{\sigma }}^{*}\left(2{\mathrm{s}}^2\right),\mathrm{\pi }{\left(2{\mathrm{p}}_z\right)}^2,\mathrm{\pi }{\left(2{\mathrm{p}}_x\right)}^1,\mathrm{\pi }{\left(2{\mathrm{p}}_{\mathrm{y}}\right)}^1$
3. $\mathrm{KK} \mathrm{\sigma }\left(2{\mathrm{s}}^2\right),{\mathrm{\sigma }}^{*}\left(2{\mathrm{s}}^2\right),\mathrm{\pi }{\left(2{\mathrm{p}}_z\right)}^2,\mathrm{\pi }{\left(2{\mathrm{p}}_x\right)}^2,\mathrm{\pi }{\left(2{\mathrm{p}}_{\mathrm{y}}\right)}^1$
4. $\mathrm{KK} \mathrm{\sigma }\left(2{\mathrm{s}}^2\right),{\mathrm{\sigma }}^{*}\left(2{\mathrm{s}}^2\right),\mathrm{\sigma }{\left(2{\mathrm{p}}_z\right)}^2,\mathrm{\pi }{\left(2{\mathrm{p}}_x\right)}^2,\mathrm{\pi }{\left(2{\mathrm{p}}_{\mathrm{y}}\right)}^2$

Write order of dipole moment of following compounds :-

1. (iii) > (ii) > (i) > (iv) > (v) > (vi)
2. (iii) > (i) > (ii) = (vi) > (iv) > (v)
3. (ii) > (i) = (iii) = (iv) > (v) = (vi)
4. (iii) > (i) > (iv) > (v) > (ii) > (vi)

The colour of halogens progressively deepens from fluorine to iodine because :-
1. halogens of higher atomic number absorb light of longer wavelength since the difference in energy between the ground state and excited state decreases as the atomic number increases.
2. fluorescence and phosphorescence become more intense as the atomic numbers of halogen increases
3. the standard electrode potential increases from I₂
to F₂
4. halogens of higher atomic number absorb light of
shorter wavelength since the difference in energy between the ground state and excited state increases as
the atomic number increases.

The bond order in NO is 2.5 while that in NO⁺
is 3. Which of the following statements is true for these two
species?
1. Bond length in NO⁺ is equal to that in NO
2.  Bond length in NO is greater than in NO⁺
3. Bond length in NO⁺ is greater than in NO
4. Bond length is unpredictable

In which of the following ionizion processes, the bond
order has increased and the magnetic behaviour has
changed
1. $\mathrm{NO}\to {\mathrm{NO}}^{+}$
2. ${\mathrm{O}}_2\to {\mathrm{O}}_2^{+}$
3. ${\mathrm{N}}_2\to {\mathrm{N}}_2^{+}$
4. ${\mathrm{C}}_2\to {\mathrm{C}}_2^{+}$

Using MO theory predict which of the following species
has the shortest bond length?
1. ${\mathrm{O}}_2^{-}$
2. ${\mathrm{O}}_2^{2-}$
3. ${\mathrm{O}}_2^{2+}$
4. ${\mathrm{O}}_2^{+}$

The molecule having smallest bond angle is
1. PCl₃
2. NCl₃
3. AsCl₃
4. SbCl₃

According to molecular orbital theory which of the
following statement about the magnetic character and bond
order is correct regarding ${\mathrm{O}}_2^{+}$
1. Paramagnetic and Bond order < O₂
2. Paramagnetic and Bond order >O₂
3. Diamagnetic and Bond order < O₂
4. Diamagnetic and Bond order > O₂

Which of the following B.P. order is not correct
(1) $Si{F}_4<SiC{l}_4$                    (2) $C{H}_4<Si{H}_4<Ge{H}_4$
(3) $C{H}_4<C{D}_4$                       (4) $He>H_2$

The fluoride which is most soluble in water :-
(1) $Ca{F}_2$                    (2) $Ba{F}_2$
(3) $Sr{F}_2$                     (4) $Be{F}_2$

Which of the following compounds give metal and oxygen gas at high temp :-
(1) $NaN{O}_3$                       (2) $A{g}_{2}C{O}_3$
(3) $K_{2}C{O}_3$                        (4) $L{i}_{2}C{O}_3$

How many BP (Bonding 'e' pair) are present in white phosphorus :-
(1) 6            (2) 4              (3) 12               (4) 8

Structure of carbon suboxide $\left(C_3{O}_2\right)$ is ;-
(1) Linear                            (2) Bent
(3) Trigonal planer              (4) Distorted tetrahedral

In $O_2^{-}, O_2 and O_2^{-2}$ species total No.  of antibonding electrons are respectively :-
(1) 7, 6, 8                           (2) 1, 0, 2
(3) 6, 6, 6                           (4) 8, 6, 8

Which of the following carbide of s-block element gives methane on reaction with water :-
(1) $B{e}_{2}C$                           (2) $A{l}_4{C}_3$
(3) $Ca{C}_2$                           (4) Both (1) and (2)

Which shows highest Dipole moment :-
(1) HF                       (2) HCl
(3) HBr                      (4) HI

In $CI{F}_3$ lone pair of electrons present at :-
(1) Equatorial position
(2) Axial position
(3) Both (1) and (2)
(4) None of these

The number of $p\mathrm{\pi }-\mathrm{p\pi }$ bonds present in $Xe{O}_3$ and $Xe{O}_{4-}$ molecules are respectively
(1) 3, 4                (2) 4, 2              (3) 2, 3              (4) 3, 2