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Which one of the following is not paramagnetic ?
1. NO
2. ${\mathrm{N}}_2^{+}$
3. CO
4. ${\mathrm{O}}_2^{-}$

The angular shape of ozone molecule (O₃) consists of 
1. 1 sigma and 2 pi-bonds
2. 2 sigma and 2 pi-bonds
3. 1 sigma and 1 pi-bonds
4. 2 sigma and 1 pi-bonds

In which of the following molecules are all the bonds not equal?
1. ClF₃
2. BF₃
3.  PF₃
4. NF₃

According to molecular orbital theory, arrange the nitrogen species in each list in ascending order of bond order:
1. ${\mathrm{N}}_2^{-} < {\mathrm{N}}_2 < {\mathrm{N}}_2^{2-}$
2. ${\mathrm{N}}_2^{2-} < {\mathrm{N}}_2^{-} < {\mathrm{N}}_2$
3. ${\mathrm{N}}_2 < {\mathrm{N}}_2^{2-} <\hspace{0.17em}{\mathrm{N}}_2^{-}$
4. ${\mathrm{N}}_2^{-} < {\mathrm{N}}_2^{2-} < {\mathrm{N}}_2$

Which one of the following is planar ?
1. XeF₄
2. XeO₄
3. XeO₃
4. XeO₃F₂

The dielectric constant of H₂O is 80. The electrostatic force of attraction between Na⁺ and Cl^- will be
1. reduced to $\frac{1}{40}$ in water than in air
2. reduced to $\frac{1}{80}$ in water than in air
3. will be increased to 80 in water than in air
4. will remain unchanged

Which of the following is isoelectronic? 
1. ${\mathrm{CO}}_2, {\mathrm{NO}}_2$
2. ${\mathrm{NO}}_2^{-}, {\mathrm{CO}}_2$
3. ${\mathrm{CN}}^{-}, \mathrm{CO}$
4. ${\mathrm{SO}}_2, {\mathrm{CO}}_2$

In an octahedral structure, the pair of d orbitals involved in d²sp³-hybridisation is
1. $d_{x^2-y^2}, d_{z^2}$
2. $d_{xy}, d_{x^2\mathit{-}{y}^{\mathit{2}}}$
3. $d_{{\mathrm{z}}^2}, d_{xz}$
4. $d_{xy}, d_{yz}$

Equilateral shape has
1. sp hybridisation
2. sp² hybridisation
3. sp³ hybridisation
4. dsp² hybridisation

Overlap of which of the following atomic orbitals would be maximum to form the strongest covalent bond.
1. 1s-2s (σ)
2. 1s-2p (σ)
3. 2p-2p (π)
4. 2p-2p (σ)

Among LiCl, BeCl₂, BCl₃ and CCl₄,
the covalent bond character varies as:
1. LiCl < BeCl₂ > BCl₃ > CCl₄
2. LiCl > BeCl₂ < BCl₃ < CCl₄
3. LiCl < BeCl₂ < BCl₃ < CCl₄
4. LiCl > BeCl₂ > BCl₃ > CCl₄

Which of the following statement is not correct from the view point of molecular orbital theory ?
1. Be₂ is not a stable molecule
2. He₂ is not a stable but He_2⁺ is expected to exist.
3. Bond strength of N₂ is maximum amongst the homonuclear diatomic molecules belonging to the second period.
4. The order of energies of molecular orbitals in N₂ molecule is
 s2s < s*2s < s2p_z < (p2p_x=p2p_y) < (p*2p_x=p*2p_y) < s*2p_z  

Compound that does not exhibit hydrogen bonding is-

1.	CH3CH2OH	2.
3.		4.

PCl₅ is highly unstable and in a solid-state, it exists as into  [PCl₄]⁺ and [PCl₆]^- ions.
The geometry of [PCl₆]^- is   
1. Octahedral
2. Tetrahedral
3. Square pyramidal
4. Square planar

Which of the following species has maximum number of lone-pair of electrons on the central atom ?
1. XeF₂
2. H₃O⁺
3. XeF₄
4. XeF₆

Which is the least polarizable gas among the following?

The correct order of  bond angle order is 
(1) ${\mathrm{NH}}_2^{-}>{\mathrm{NH}}_3 >{\mathrm{NH}}_4^{+}$
(2) ${\mathrm{NH}}_4^{+}>{\mathrm{NH}}_3 >{\mathrm{NH}}_2^{-}$
(3) ${\mathrm{NH}}_3^{}>{\mathrm{NH}}_{{}_2}^{-} >{\mathrm{NH}}_4^{+}$
(4) ${\mathrm{NH}}_3^{}>{\mathrm{NH}}_4^{+} >{\mathrm{NH}}_2^{-}$

The number of sigma bonds in P₄O₁₀ is 
1. 6
2. 16
3. 20
4. 7

Among the following iso-structural compounds, the one that has the highest lattice energy is: 
1. LiCl
2. MgO
3. NaCl
4. LiF

A sbonded molecule MX₃ is T-shaped. The number of non-bonding pairs of electrons is :
1. 0
2. 2
3. 1
4. Can be predicted only if atomic number of M is known,
 
 

In a chemical change from ${\mathrm{PCl}}_3 \stackrel{ }{\to }{\mathrm{PCl}}_5$, the hybrid state of P changes from:
1. sp² to sp³
2. sp³ to sp²
3. sp³ to sp³d
4. sp³ to dsp²

Which molecules/ions are most paramagnetic?
1. B₂
2. C₂
3. ${\mathrm{O}}_2^{+}$
4. ${\mathrm{O}}_2^{-}$

In which case observed dipole moment is greater than theoretical dipole moment?
1.
2.
3.
4.

Which has highest bond angle ?
(1) NH₃
(2) H₂O
(3) H₂S
(4) PH₃

Select the correct order of solubility (in water) from the following:
1. SrSO₄ < CaSO₄ < MgSO₄ < BeSO₄
2. NaF < KF < RbF < CsF
3. Ba(OH)₂ > Sr(OH)₂ > Ca(OH)₂ > Mg(OH)₂
4 All of the above

The hydride of group 16 having highest boiling point is:
1. H₂O because of H-bonding
2. H₂Te because of higher molecular weight
3. H₂S because of H-bonding
4. H₂Se because of lower molecular weight

Which of the following is correct :-
(1) Extent of hydration is PCl₅ > SiCl₄ and BCl₃ < CCl₄
(2) K⁺ ion will be more Hydrated than Li⁺
(3) In BCl₃ there are no vacant d-orbitals but still it can undergo expansion
(4) None

The correct order in which the O-O bond length increases in the following is
1. H₂O₂ < O₂ < O₃
2. O₃ < H₂O < O₂
3. O₂ < O₃< H₂O₂
4. O₂ < H₂O₂ < O₃

Carbon suboxide (C₃O₂) has
1. Linear structure
2. Bent structure
3. Trigonal structure
4. Disorted tetrahedral structure

The pair of electrons in the given carbanion, CH₃C≡C^-, is present in which of the following orbitals?

Which of the following species contains equal number of $\mathrm{\sigma }$ and $\mathrm{\pi }$ bonds?
1. ${\mathrm{HCO}}_3^{-}$                                   
2. XeO₄
3. (CN)₂                                     
4. CH₂(CN)₂

The correct bond order in the following species is
1. ${\mathrm{O}}_2^{2+}>{\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{-}$
2. ${\mathrm{O}}_2^{2+}<{\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{+}$
3. ${\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{2+}$
4. ${\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{2+}$

XeF₂ is isostructural with : 
1. TeF₂
2. ICI₂^-
3. SbCl₃
4. BCl₃

Which one of he following pairs is isostructural (i.e., having the same shape and
hybridization)?
1. [BCl₃ and BrCl₃]
2. [NH₃ and ${\mathrm{NO}}_3^{-}$]
3. [NF₃ and BF₃]
4. [${\mathrm{BF}}_4^{-}$ and ${\mathrm{NH}}_4^{+}$]

Bond order of 1.5 is shown by
1. ${\mathrm{O}}_2^{+}$     
2. ${\mathrm{O}}_2^{-}$       
3. ${\mathrm{O}}_2^{2-}$     
4. O₂

What is the dominant intermolecular force on bond that must be overcome in converting
liquid CH₃OH to a gas?
1. Hydrogen bonding
2. Dipole-dipole interaction
3. Covalent bonds
4. London dispersion force

The correct order of electronegativity of hybrid orbitals of carbon is:
(1) sp>sp²<sp³             
(2) sp>sp²>sp³
(3) sp<sp²>sp³             
(4) sp<sp²<sp³

$H_{2}O$ has a net dipole moment while Be$F_2$ has zero dipole moment because :
(1) F is more electronegativity than oxygen 
(2) Be is more electronegativity than oxygen 
(3) $H_{2}O$ molecule is linear and Be$F_2$ is bent 
(4) $Be{F}_2$ molecule is linear and $H_{2}O$ is bent

Which of the following compound have the same no. of lone pair with their central atom?
(i)${\mathrm{XeF}}_5^{- }$             
(ii) ${\mathrm{BrF}}_3$                 
(iii) ${\mathrm{XeF}}_2$                     
(iv) ${\mathrm{H}}_3{\mathrm{S}}^{+}$               
(v) Triple Methylene     
options are as follows :        
(1) (iv) and (v)                                     
(2) (i) and (iii) 
(3) (i) and (ii)                                     
(4) (ii) (iv), (v)

In which of the following species central atom is NOT surrounded by exactly 8 valence electrons?
(a) $B{F_4}^{-}$
(b) $NC{l}_3$
(c) PC${l_4}^{+}$
(d) $S{F}_4$

The least polar bond is present in which of the following?

Which set contains only covalently bonded molecules?
(1) $BC{l}_{3 }, SiC{l}_4 ,PC{l}_3$
(2) $N{H}_{4}Br , N_2{H}_4,HBr$
(3) $I_{2 ,}{H}_{2}S , NAI$
(4) $A{l}_2,O_{3 }, A{S}_4$

$N{F}_3$ is:
(1) non-polar compound 
(2) electrovalent compound 
(3) having low value of dipole moment than $N{H}_3$
(4) having more dipole moment than $N{H}_3$

Which of the following statement is true for $I{O}_2{F_2}^{-}$according to VSEPR theory?
(A) The lone pair and two I-O double bonds occupy the equatorial positions of trigonal
bipyramid.
(B) It has $s{p}^3$ hybridization and is T-shaped.
(C)  Its structure is analogous to $S{F}_4$.
(D) (A) and (C) both

Most covalent compound among the following is :