Chemical Bonding · JEE Main previous year questions

In $\stackrel{1}{\mathrm{C}}{\mathrm{H}}_2=\stackrel{2}{\mathrm{C}}=\stackrel{3}{\mathrm{C}}\mathrm{H}-\stackrel{4}{\mathrm{C}}{\mathrm{H}}_3$ molecule, the hybridization of carbon 1, 2, 3 and 4 respectively, are :

1. A.$\mathrm{s}{\mathrm{p}}^2,\mathrm{sp},\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^3$
2. B.$\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^3$
3. C.$\mathrm{s}{\mathrm{p}}^3,\mathrm{sp},\mathrm{s}{\mathrm{p}}^3,\mathrm{s}{\mathrm{p}}^3$
4. D.$\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^3,\mathrm{s}{\mathrm{p}}^2,\mathrm{s}{\mathrm{p}}^3$

Which among the following species has unequal bond lengths?

1. A.$\mathrm{Xe}{\mathrm{F}}_4$
2. B.$\mathrm{B}{\mathrm{F}}_4^{-}$
3. C.$\mathrm{Si}{\mathrm{F}}_4$
4. D.$\mathrm{S}{\mathrm{F}}_4$

If $\mathrm{A}{\mathrm{B}}_4$ molecule is a polar molecule, a possible geometry of $\mathrm{A}{\mathrm{B}}_4$ is

1. A.Tetrahedral
2. B.see-saw
3. C.Square pyramidal
4. D.Square planar

The molecular geometry of $\mathrm{S}{\mathrm{F}}_6$ is octahedral. What is the geometry of $\mathrm{S}{\mathrm{F}}_4$ (including lone pair(s) of electrons, if any)?

1. A.Tetrahedral
2. B.Trigonal bipyramidal
3. C.Square planar
4. D.Pyramidal

If enthalpy of atomisation for ${\mathrm{Br}}_2(l)$ is x kJ/mol and bond enthalpy for ${\mathrm{Br}}_2$ is y kJ/mol, the relation between them :

1. A.does not exist
2. B.is $x<y$
3. C.is $x>y$
4. D.is $x=y$

Chlorine reacts with hot and concentrated NaOH and produces compounds (X) and (Y). Compound (X) gives white precipitate with silver nitrate solution. The average bond order between Cl and O atoms in (Y) is.

The bond order and the magnetic characteristics of $\mathrm{C}{\mathrm{N}}^{-}$ are :

1. A.3, paramagnetic
2. B.$2\frac{1}{2}$, paramagnetic
3. C.3, diamagnetic
4. D.$2\frac{1}{2}$, diamagnetic

The number of $\mathrm{s}{\mathrm{p}}^2$ hybridised carbons present in "Aspartame" is

The C–C bond length is maximum in :

1. A.${\text{C}}_{60}$
2. B.diamond
3. C.graphite
4. D.${\text{C}}_{70}$

The isoelectronic set of ions is :

1. A.${\mathrm{F}}^{-}$, $\mathrm{L}{\mathrm{i}}^{+}$, $\mathrm{N}{\mathrm{a}}^{+}$ and $\mathrm{M}{\mathrm{g}}^{2+}$
2. B.$\mathrm{L}{\mathrm{i}}^{+}$, $\mathrm{N}{\mathrm{a}}^{+}$, ${\mathrm{O}}^{2-}$ and ${\mathrm{F}}^{-}$
3. C.${\mathrm{N}}^{3-}$, ${\mathrm{O}}^{2-}$, ${\mathrm{F}}^{-}$ and $\mathrm{N}{\mathrm{a}}^{+}$
4. D.${\mathrm{N}}^{3-}$, $\mathrm{L}{\mathrm{i}}^{+}$, $\mathrm{M}{\mathrm{g}}^{2+}$ and ${\mathrm{O}}^{2-}$

Among the following species, the diamagnetic molecule is

1. A.$\mathrm{CO}$
2. B.${\mathrm{B}}_2$
3. C.${\mathrm{O}}_2$
4. D.$\mathrm{NO}$

The ion that has $s{p}^3{d}^2$ hybridization for the central atom, is :

1. A.$[\mathrm{IC}{\mathrm{l}}_2{]}^{-}$
2. B.$[\mathrm{IC}{\mathrm{l}}_4{]}^{-}$
3. C.$[\mathrm{I}{\mathrm{F}}_6{]}^{-}$
4. D.$[\mathrm{Br}{\mathrm{F}}_2{]}^{-}$

Among the following molecules / ions, ${\mathrm{C}}_2^{2-},{\mathrm{N}}_2^{2-},{\mathrm{O}}_2^{2-},{\mathrm{O}}_2$ which one is diamagnetic and has the shortest bond length?

1. A.${\mathrm{O}}_2$
2. B.${\mathrm{C}}_2^{2-}$
3. C.${\mathrm{N}}_2^{2-}$
4. D.${\mathrm{O}}_2^{2-}$

In Wilkinson's catalyst, the hybridization of central metal ion and its shape are respectively :

1. A.${\text{sp}}^3\text{d}$, trigonal bipyramidal
2. B.${\text{sp}}^3$, tetrahedral
3. C.${\text{dsp}}^2$, square planar
4. D.${\text{d}}^2{\text{sp}}^3$, octahedral

Which of the following conversions involves change in both shape and hybridisation ?

1. A.${\text{NH}}_3\to {\text{NH}}_4^{+}$
2. B.${\text{CH}}_4\to {\text{C}}_2{\text{H}}_6$
3. C.${\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}$
4. D.${\text{BF}}_3\to {\text{BF}}_4^{-}$

Identify the pair in which the geometry of the species is T-shape and square - pyramidal, respectively :

1. A.${\text{ClF}}_3$ and $I{O}_4^{-}$
2. B.${\text{ICl}}_2^{-}$ and ${\text{ICl}}_5$
3. C.${\text{XeOF}}_2$ and ${\text{XeOF}}_4$
4. D.${\text{IO}}_3^{-}$ and ${\text{IO}}_2{\text{F}}_2^{-}$

The decreasing order of bond angles in ${\text{BF}}_3,{\text{NH}}_3,{\text{PF}}_3$ and ${\text{I}}_3^{-}$ is :

1. A.${\text{I}}_3^{-}>{\text{NH}}_3>{\text{PF}}_3>{\text{BF}}_3$
2. B.${\text{I}}_3^{-}>{\text{BF}}_3>{\text{NH}}_3>{\text{PF}}_3$
3. C.${\text{BF}}_3>{\text{I}}_3^{-}>{\text{PF}}_3>{\text{NH}}_3$
4. D.${\text{BF}}_3>{\text{NH}}_3>{\text{PF}}_3>{\text{I}}_3^{-}$

$\text{H}-\text{N}\stackrel{\text{(I)}}{---}\text{N}\stackrel{\text{(II)}}{---}\text{N}$ In hydrogen azide (above) the bond orders of bond (I) and (II) are :

1. A.(I) < 2, (II) > 2
2. B.(I) > 2, (II) < 2
3. C.(I) > 2, (II) > 2
4. D.(I) < 2, (II) < 2

Total number of lone pair of electrons in ${\text{I}}_3^{-}$ ion is

1. A.3
2. B.9
3. C.6
4. D.12

1. A.(I)
2. B.(II)
3. C.(III)
4. D.(IV)

Which of the following is paramagnetic ?

1. A.$\mathrm{N}{\mathrm{O}}^{+}$
2. B.$\mathrm{CO}$
3. C.$O_2^{2-}$
4. D.${\mathrm{B}}_2$

$\mathrm{s}{\mathrm{p}}^3{\mathrm{d}}^2$ hybridization is not displayed by :

1. A.$\mathrm{Br}{\mathrm{F}}_5$
2. B.$\mathrm{S}{\mathrm{F}}_6$
3. C.$[\mathrm{Cr}{\mathrm{F}}_6{]}^{3-}$
4. D.$\mathrm{P}{\mathrm{F}}_5$

The species in which the $N$ atom is in a state of $sp$ hybridization is :

1. A.$\mathrm{N}{\mathrm{O}}_2^{+}$
2. B.$\mathrm{N}{\mathrm{O}}_2^{-}$
3. C.$\mathrm{N}{\mathrm{O}}_3^{-}$
4. D.$\mathrm{N}{\mathrm{O}}_2$

Dipole moment is shown by

1. A.1,2-dichlorobenzene
2. B.trans-2,3-dichloro-2-butene
3. C.1,4-dichlorobenzene
4. D.trans-1,2-dinitroethene

The formation of molecular complex $\mathrm{B}{\mathrm{F}}_3-\mathrm{N}{\mathrm{H}}_3$ results in a change in hybridization of boron

1. A.from $s{p}^2$ to $ds{p}^2$
2. B.from $s{p}^2$ to $s{p}^3$
3. C.from $s{p}^3$ to $s{p}^2$
4. D.from $s{p}^3$ to $s{p}^{3}d$