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In which of the following pairs the two species are not isostructural ?
(1) $AI{F}_6^{3-} and S{F}_6$                                 
(2) $C{O}_3^{2-} and N{O}_3^{-}$
(3) $PC{l}_4^{+} and SiC{l}_4$                               
(4) $P{F}_5 and Br{F}_5$

Identify the least stable ion amongst the following:
(1) $L{i}^{-}$                                       
(2) $B{e}^{-}$
(3) $B^{-}$                                       
(4) $C^{-}$

The decreasing values of bond angles from $N{H}_3$(106°) to $Sb{H}_3$(91°) down group-15 of the periodic table is due to 
(1) decreasing lp – bp repulsion                 
(2) increasing electronegativity 
(3) increasing bp – bp repulsion                 
(4) increasing p-orbital character in $s{p}^3$

Which of the following conversions demonstrates an increase in bond order and a change in magnetic behaviour?
1. $NO\to N{O}^{+}$                                 
2. $O_2\to O_2+$
3. $N_2\to N_2^{+}$                                   
4. $C_2\to C_2^{+}$

Which of the following hydrogen bonds is the strongest
(1) F–H.....F                             
(2) O–H.....O
(3) O–H.....F                             
(4) O–H.....N

Which of the following species exhibits the diamagnetic behaviour
(1) $O_2^{+}$                                   
(2) $O_2$
(3) NO                                   
(4) $O_2^{2-}$

The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, 
$K^{+}, C{a}^{+2}, M{g}^{+2}, B{e}^{+2}$
(1) $B{e}^{+2}<K^{+}<C{a}^{+2}<M{g}^{+2}$                     
(2) $K^{+}<C{a}^{+2}<M{g}^{+2}<B{e}^{+2}$
(3) $C{a}^{+2}<M{g}^{+2}<B{e}^{+2}<K^{+}$                     
(4) $M{g}^{+2}<B{e}^{+2}<K^{+}<C{a}^{+2}$
 

Using MO theory predict which of the following species has the shortest bond length?
(1) $O_2^{-}$                                   
(2) $O_2^{2-}$
(3) $O_2^{2+}$                                 
(4) $O_2^{+}$
 

The hybridisation of orbitals of N atom in $N{O}_3^{-}$, $N{O}_2^{+}$ and $N{H}_4^{+}$ are respectively:-
(1) $sp, s{p}^3, s{p}^2$                                 
(2) $s{p}^2, s{p}^3, sp$
(3) $sp, s{p}^2, s{p}^3$                                 
(4) $s{p}^2, sp, s{p}^3$
 

The structure of $I{F}_7$ is :-
(1) octahedral                                   
(2) pentagonal bipyramid
(3) square pyramid                           
(4) trigonal bipyramid

Among the following the maximum covalent character is shown by the compound :-
(1) $AlC{l}_3$                                   
(2) $MgC{l}_2$
(3) $FeC{l}_2$                                   
(4) $SnC{l}_2$

Which of the following has maximum number of lone pairs associated with Xe ?
(1) $Xe{O}_3$                             
(2) $Xe{F}_4$
(3) $Xe{F}_6$                             
(4) $Xe{F}_2$

The number of types of bonds between two carbon atoms in calcium carbide is :-
(1) One sigma, two pi                       
(2) One sigma, one pi
(3) Two sigma, one pi                       
(4) Two sigma, two pi

Ortho-Nitrophenol is less soluble in water than p– and m– Nitrophenols because :-
(1) Melting point of o–Nitrophenol is lower than those of m– and p– isomers
(2) o–Nitrophenol is more volatile in steam than those of m– and p– isomers
(3) o–Nitrophenol shows Intramolecular H–bonding
(4) o–Nitrophenol shows Intermolecular H–bonding

Iron exhibits +2 and +3 oxidation states. Which of the following statements about iron is incorrect ?
(1) Ferrous compounds are more easily hydrolysed than the corresponding ferric compounds.
(2) Ferrous oxide is more basic in nature than the ferric oxide.
(3) Ferrous compounds are relatively more ionic than the corresponding ferric compounds.
(4) Ferrous compounds are less volatile than the corresponding ferric compounds

The molecule having the smallest bond angle is-

Moving from right to left in a periodic table, the atomic size is:
1. increased                                               
2. decreased
3. remains constant                                     
4. none of these

The increasing order of electronegativity in the following elements:
(1) C, N, Si, P                                 
(2) N, Si, C, P
(3) Si, P, C, N                                 
(4) P, Si, N, C

Which statement accurately describes an element with an atomic weight of 39 and the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹?
1. High value of Ionisation Energy                               
2. Transition element
3. Isotone with \(_{18}^{38}\text{Ar}\) 
4. None of the above

The number of paired electrons in oxygen atom is:
(1) 6                                               
(2) 16
(3) 8                                               
(4) 32

The decreasing size of $K^{+}, C{a}^{2+}, C{l}^{-} \& S^{2-}$  follows the order:
(1) $K^{+}>C{a}^{+2}>S^{-2}>C{l}^{-}$                   
(2) $K^{+}>C{a}^{+2}>C{l}^{-}>S^{-2}$
(3) $C{a}^{+2}>K^{+}>C{l}^{-}>S^{-2}$                   
(4) $S^{-2}>C{l}^{-}>K^{+}>C{a}^{+2}$

Which of the following has the maximum number of unpaired electrons
(1) $M{g}^{2+}$                                     
(2) $T{i}^{3+}$
(3) $V^{3+}$                                       
(4) $F{e}^{2+}$

The incorrect statement among the following is:
1. the first ionisation potential of Al is less than the first ionisation potential of Mg
2. the second ionisation potential of Mg is greater than the second ionisation potential of Na
3. the first ionisation potential of Na is less than the first ionisation potential of Mg
4. the third ionisation potential of Mg is greater than the third ionisation potential of Al

The electrons, identified by n & l ;
(i) n = 4 , l = 1               
(ii) n = 4 , l = 0                 
(iii) n = 3 , l = 2
(iv) n = 3 , l = 1 can be placed in order of increasing energy, from the lowest to highest as :
(1) (iv) < (ii) < (iii) < (i)                         
(2) (iii) < (ii) < (iv) < (i)
(3) (i) < (iii) < (ii) < (iv)                         
(4) (iii) < (i) < (iv) < (ii)

Assertion : F atom has a less negative electron gain enthalpy than Cl atom.
Reason : Additional electron is repelled more efficiently by 3p electron in Cl atom than by 2p electron in F atom.

The correct order of radii is:
(1) N < Be < B                               
(2) $F^{-}<O^{2-}<N^{3-}$
(3) Na < Li < K                               
(4) $F{e}^{3+}<F{e}^{2+}<F{e}^{4+}$

The set representing correct order of $I{P}_1$ is
(1) K > Na > Li                           
(2) Be > Mg > Ca
(3) B > C > N                           
(4) Fe > Si > C