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In which of the following molecules, all atoms are coplanar?
1.
2.
3.
4.

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. ${\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{2+}$

A molecule having the maximum dipole moment among the following is -
1. CO₂
2. CH₄
3. NH₃
4. NF₃

Which among the following species has a triangular planar shape?

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

The correct order of increasing bond length of 
C-H, C-O, C-C and C=C is
1. C-C<C=C<C-O<C-H
2. C-O<C-H<C-C<C=C
3. C-H<C-O<C-C<C=C
4. C-H<C=C<C-O<C-C

In which of the following pairs of molecules/ions, the central atoms have \(\mathrm{sp}^2\) hybridisation?

The correct order of increasing bond angles in the following triatomic species is
(1) NO₂^- < NO₂⁺ < NO₂
(2) NO₂^- < NO₂   < NO₂⁺
(3) NO₂⁺ < NO₂   <NO₂^-
(4) NO₂⁺ < NO₂^- < NO₂

The correct geometry and hybridization for XeF₄ are : 
1.  Octahedral, sp³d²
2.  Trigonal bipyramidal, sp³d³
3.  Planar triangle, sp³d³
4.  Square planar, sp³d²

Which one of the following pairs is isostructural?
1. $\left[{\mathrm{BCl}}_3 \mathrm{and} {\mathrm{BrCl}}_3\right]$
2. $\left[{\mathrm{NH}}_3 \mathrm{and} {\mathrm{NO}}_3^{-}\right]$
3. $\left[{\mathrm{NF}}_3 \mathrm{and} {\mathrm{BF}}_3\right]$
4. $\left[{\mathrm{BF}}_4^{-} \mathrm{and} {\mathrm{NH}}_4^{+}\right]$

The correct order of increasing bond angles in the following species is
1.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2 < {\mathrm{ClO}}_2^{-}$
2.  ${\mathrm{ClO}}_2 < {\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-}$
3.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-} < {\mathrm{ClO}}_2$
4.  ClO₂^- < Cl₂O < ClO₂

The correct order of \(\mathrm{C-O}\) bond length among \(\mathrm{CO},\mathrm{CO}_3^{2-},\) and \(\mathrm{CO_2}\) is :
1. \(\mathrm{CO}_2<\mathrm{CO}_3^{2-}<\mathrm{CO} \)
2. \(\mathrm{CO}<\mathrm{CO}_3^{2-}<\mathrm{CO}_2 \)
3. \(\mathrm{CO}_3^{2-}<\mathrm{CO}_2<\mathrm{CO} \)
4. \(\mathrm{CO}<\mathrm{CO}_2<\mathrm{CO}_3^{2-}\)

${\mathrm{N}}_2$ and ${\mathrm{O}}_2$ are converted to monocations ${\mathrm{N}}_2^{+}$ and ${\mathrm{O}}_2^{+}$ respectively, which is wrong statements:
1. In ${\mathrm{N}}_2^{+}$, the $\mathrm{N}-\mathrm{N}$ bond weakens
2. In ${\mathrm{O}}_2^{+}$, the $\mathrm{O}-\mathrm{O}$ bond order increases
3. In ${\mathrm{O}}_2^{+}$, the paramagnetism decreases
4. ${\mathrm{N}}_2^{+}$ becomes diamagnetic

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

The shape of ${\mathrm{XeF}}_3^{+}$ is :
1. Trigonal planar
2. Pyramidal
3. Bent T-shape
4. See-saw

In bisulphate ion, HSO₄^-, the formal charge on S atom is
1. +6
2. +4
3. +1
4. +2

The shape of covalent molecule AX₃ is
1. Triangular
2. T-shape
3. Pyramidal
4. Any of the above three depending upon the number of lone pairs present in A

The geometrical arrangement and shape of $I_3^{-}$ are respectively
1. Trigonal bipyramidal geometry, linear shape
2. Hexagonal structure, linear shape
3. Triangular planar geometry, triangular shape
4. Tetrahedral geometry, pyramidal shape

Which has non-zero dipole moment?
1. PCl₅
2. PCl₃F₂
3. PCl₃Br₂
4. PCl₃(CH₃)₂

Which molecules/ions are most paramagnetic?
1. B₂
2. C₂
3. $O_2^{+}$
4. $O_2^{-}$

The correct statement is
1. When O₂ is converted into $O_2^{+}$ then bond distance increases
2. When N₂ is converted into $N_2^{+}$ then bond distance increases
3. When CO is converted into CO⁺ then bond distance increases
4. All of these

Benzene ring contains
1. 12 $\sigma$ and 3$\pi$
2. 6 $\sigma$ and 3$\pi$
3. 9 $\sigma$ and 3$\pi$
4. 8 $\sigma$ and 2$\pi$

In ${\mathrm{PO}}_4^{3-}$ ion, the formal charge on each oxygen atom and P-O bond order respectively are :
1.  -0.75, 0.6
2.  -0.75, 1.0
3.  -0.75, 1.25
4.  -3.1, 1.25

In which of the following molecules are all the bonds not equal?
1. $Cl{F}_3$
2. $B{F}_3$
3. $Al{F}_3$
4. $N{F}_3$

Consider the following structures :

 
1. ${\mathrm{\theta }}_1>{\mathrm{\theta }}_2>{\mathrm{\theta }}_3>{\mathrm{\theta }}_4$
2 ${\mathrm{\theta }}_1>{\mathrm{\theta }}_3>{\mathrm{\theta }}_4>{\mathrm{\theta }}_2$
3. ${\mathrm{\theta }}_3>{\mathrm{\theta }}_1>{\mathrm{\theta }}_2>{\mathrm{\theta }}_4$
4. ${\mathrm{\theta }}_1>{\mathrm{\theta }}_3>{\mathrm{\theta }}_2>{\mathrm{\theta }}_4$