Chemical Bonding · JEE Main previous year questions

Match the LIST-I with LIST-II $$\begin{array}{ll}\text{LIST-I}& \text{LIST-II}\\ \text{(Molecules/ion)}& \text{(Hybridisation of central atom)}\\ \text{A.}\mathrm{P}{\mathrm{F}}_5& \text{I}\mathrm{ds}{\mathrm{p}}^2\\ \text{B}\mathrm{S}{\mathrm{F}}_6& \text{II}\mathrm{s}{\mathrm{p}}^3\mathrm{d}\\ \text{C}\mathrm{Ni}(\mathrm{CO}{)}_4& \text{III}\mathrm{s}{\mathrm{p}}^3{\mathrm{d}}^2\\ \text{D}[\mathrm{PtC}{\mathrm{l}}_4{]}^{2-}& \text{IV}\mathrm{s}{\mathrm{p}}^3\end{array}$$ Choose the correct answer from the options given below:

1. A.A-IV, B-I, C-II, D-III
2. B.A-III, B-I, C-IV, D-II
3. C.A-II, B-III, C-IV, D-I
4. D.A-I, B-II, C-III, D-IV

Among ${\mathrm{SO}}_2,{\mathrm{NF}}_3,{\mathrm{NH}}_3,{\mathrm{XeF}}_2,{\mathrm{ClF}}_3$ and ${\mathrm{SF}}_4$, the hybridization of the molecule with nonzero dipole moment and highest number of lone-pairs of electrons on the central atom is

1. A.${\mathrm{sp}}^3$
2. B.${\mathrm{dsp}}^2$
3. C.${\mathrm{sp}}^3{\mathrm{d}}^2$
4. D.${\mathrm{sp}}^3\mathrm{d}$

Which among the following molecules is (a) involved in $\mathrm{s}{\mathrm{p}}^3\mathrm{d}$ hybridization, (b) has different bond lengths and (c) has lone pair of electrons on the central atom?

1. A.$\mathrm{Xe}{\mathrm{F}}_4$
2. B.$\mathrm{Xe}{\mathrm{F}}_2$
3. C.$\mathrm{P}{\mathrm{F}}_5$
4. D.$\mathrm{S}{\mathrm{F}}_4$

In 3,3-dimethylhex-1-en-4-yne, there are ____ $\mathrm{s}{\mathrm{p}}^3$, ____ $\mathrm{s}{\mathrm{p}}^2$ and ____ $\mathrm{sp}$ hybridised carbon atoms respectively.

1. A.4, 2, 2
2. B.2, 4, 2
3. C.3, 3, 2
4. D.2, 2, 4

The type of hybridization and the magnetic property of $[\mathrm{MnC}{\mathrm{l}}_6{]}^{3-}$ are,

1. A.$s{p}^3{d}^2$, paramagnetic with four unpaired electrons.
2. B.$d^{2}s{p}^3$, paramagnetic with four unpaired electrons.
3. C.$s{p}^3{d}^2$, paramagnetic with two unpaired electrons.
4. D.$d^{2}s{p}^3$, paramagnetic with two unpaired electrons.

Total number of sigma (σ) _______ and pi(π) ______ bonds respectively present in hex-1-en-4-yne are:

1. A.14 and 3
2. B.11 and 3
3. C.13 and 3
4. D.3 and 13

Consider ' n ' is the number of lone pair of electrons present in the equatorial position of the most stable structure of $\mathrm{Cl}{\mathrm{F}}_3$. The ions from the following with ' n ' number of unpaired electrons are A. ${\mathrm{V}}^{3+}$ B. $\mathrm{T}{\mathrm{i}}^{3+}$ C. $\mathrm{C}{\mathrm{u}}^{2+}$ D. $\mathrm{N}{\mathrm{i}}^{2+}$ E. $\mathrm{T}{\mathrm{i}}^{2+}$ Choose the correct answer from the options given below:

1. A.B and D Only
2. B.A, D and E Only
3. C.B and C Only
4. D.A and C Only

1. A.Both Statement I and Statement II are correct
2. B.Statement I is incorrect but Statement II is correct
3. C.Both Statement I and Statement II are incorrect
4. D.Statement I is correct but Statement II is incorrect

The formation enthalpies, $\Delta {\mathrm{H}}_{\mathrm{f}}^{\ominus }$ for ${\mathrm{H}}_{(\mathrm{g})}$ and ${\mathrm{O}}_{(\mathrm{g})}$ are $220.0$ and $250.0\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$, respectively, at $298.15\mathrm{K}$ , and $\Delta {\mathrm{H}}_{\mathrm{f}}^{\ominus }$ for ${\mathrm{H}}_2{\mathrm{O}}_{(\mathrm{g})}$ is $-242.0\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$ at the same temperature. The average bond enthalpy of the $\mathrm{O}-\mathrm{H}$ bond in water at $298.15\mathrm{K}$ is ____ $\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$ (nearest integer).

Which of the following statement is true with respect to ${\mathrm{H}}_2\mathrm{O}$, $\mathrm{N}{\mathrm{H}}_3$ and $\mathrm{C}{\mathrm{H}}_4$ ? A. The central atoms of all the molecules are $\mathrm{s}{\mathrm{p}}^3$ hybridized. B. The $\mathrm{H}-\mathrm{O}-\mathrm{H}$, $\mathrm{H}-\mathrm{N}-\mathrm{H}$ and $\mathrm{H}-\mathrm{C}-\mathrm{H}$ angles in the above molecules are $104.5^{\circ }$ , $107.5^{\circ }$ and $109.5^{\circ }$ , respectively. C. The increasing order of dipole moment is $\mathrm{C}{\mathrm{H}}_4<\mathrm{N}{\mathrm{H}}_3<{\mathrm{H}}_2\mathrm{O}$. D. Both ${\mathrm{H}}_2\mathrm{O}$ and $\mathrm{N}{\mathrm{H}}_3$ are Lewis acids and $\mathrm{C}{\mathrm{H}}_4$ is a Lewis base. E. A solution of $\mathrm{N}{\mathrm{H}}_3$ in ${\mathrm{H}}_2\mathrm{O}$ is basic. In this solution $\mathrm{N}{\mathrm{H}}_3$ and ${\mathrm{H}}_2\mathrm{O}$ act as Lowry-Bronsted acid and base respectively. Choose the correct answer from the options given below:

1. A.A, D and E Only
2. B.C, D and E Only
3. C.A, B and C Only
4. D.A, B, C and E Only

1. A.3 and 5
2. B.3 and 6
3. C.4 and 5
4. D.4 and 6

Given below are two statements : Statement (I) : Experimentally determined oxygen-oxygen bond lengths in the ${\mathrm{O}}_3$ are found to be same and the bond length is greater than that of a $\mathrm{O}=\mathrm{O}$ (double bond) but less than that of a single $(\mathrm{O}-\mathrm{O})$ bond. Statement (II) : The strong lone pair-lone pair repulsion between oxygen atoms is solely responsible for the fact that the bond length in ozone is smaller than that of a double bond $(\mathrm{O}=\mathrm{O})$ but more than that of a single bond $(\mathrm{O}-\mathrm{O})$. In the light of the above statements, choose the correct answer from the options given below :

1. A.Statement I is false but Statement II is true
2. B.Both Statement I and Statement II are true
3. C.Statement I is true but Statement II is false
4. D.Both Statement I and Statement II are false

From the magnetic behaviour of $[{\mathrm{NiCl}}_4{]}^{2-}$ (paramagnetic) and $[\mathrm{Ni}(\mathrm{CO}{)}_4]$ (diamagnetic), choose the correct geometry and oxidation state.

1. A.$[{\mathrm{NiCl}}_4{]}^{2-}:\mathrm{Ni}(0)\text{, tetrahedral }[\mathrm{Ni}(\mathrm{CO}{)}_4]:\mathrm{Ni}(0)\text{, square planar}$
2. B.$[{\mathrm{NiCl}}_4{]}^{2-}:{\mathrm{Ni}}^{\mathrm{II}}\text{, tetrahedral }[\mathrm{Ni}(\mathrm{CO}{)}_4]:\mathrm{Ni}(0)\text{, tetrahedral}$
3. C.$[{\mathrm{NiCl}}_4{]}^{2-}:{\mathrm{Ni}}^{\mathrm{II}}\text{, tetrahedral }[\mathrm{Ni}(\mathrm{CO}{)}_4]:{\mathrm{Ni}}^{II}\text{, square planar}$
4. D.$[{\mathrm{NiCl}}_4{]}^{2-}:{\mathrm{Ni}}^{\mathrm{II}}\text{, square planar }[\mathrm{Ni}(\mathrm{CO}{)}_4]:\mathrm{Ni}(0)\text{, square planar}$

In which one of the following pairs the central atoms exhibit ${\text{sp}}^2$ hybridization ?

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

1. A.$\mathrm{II}>\mathrm{III}>\mathrm{I}$
2. B.$\mathrm{II}>\mathrm{I}>\mathrm{III}$
3. C.$\mathrm{III}>\mathrm{II}>\mathrm{I}$
4. D.$\mathrm{I}>\mathrm{II}>\mathrm{III}$

The correct increasing order for bond angles among $\mathrm{B}{\mathrm{F}}_3$, $\mathrm{P}{\mathrm{F}}_3$ and $\mathrm{Cl}{\mathrm{F}}_3$ is :

1. A.$\mathrm{B}{\mathrm{F}}_3=\mathrm{P}{\mathrm{F}}_3<\mathrm{Cl}{\mathrm{F}}_3$
2. B.$\mathrm{B}{\mathrm{F}}_3<\mathrm{P}{\mathrm{F}}_3<\mathrm{Cl}{\mathrm{F}}_3$
3. C.$\mathrm{Cl}{\mathrm{F}}_3<\mathrm{P}{\mathrm{F}}_3<\mathrm{B}{\mathrm{F}}_3$
4. D.$\mathrm{P}{\mathrm{F}}_3<\mathrm{B}{\mathrm{F}}_3<\mathrm{Cl}{\mathrm{F}}_3$

The shape of carbocation is :

1. A.tetrahedral
2. B.diagonal pyramidal
3. C.diagonal
4. D.trigonal planar

Number of molecules having bond order 2 from the following molecules is ______. ${\mathrm{C}}_2,{\mathrm{O}}_2,\mathrm{B}{\mathrm{e}}_2,\mathrm{L}{\mathrm{i}}_2,\mathrm{N}{\mathrm{e}}_2,{\mathrm{N}}_2,\mathrm{H}{\mathrm{e}}_2$

Given below are two statements : Statement I : ${\text{PF}}_5$ and ${\text{BrF}}_5$ both exhibit ${\text{sp}}^3\text{ d}$ hybridisation. Statement II : Both ${\text{SF}}_6$ and $[\text{Co}({\text{NH}}_3{)}_6{]}^{3+}$ exhibit ${\text{sp}}^3{\text{ d}}^2$ hybridisation. In the light of the above statements, choose the correct answer from the options given below :

1. A.Both Statement I and Statement II are false
2. B.Statement I is true but Statement II is false
3. C.Statement I is false but Statement II is true
4. D.Both Statement I and Statement II are true

Consider the following reactions $\text{NiS}+{\text{HNO}}_3+\text{HCl}\to \text{A}+\text{NO}+\text{S}+{\text{H}}_2\text{O}$ $\text{A}+{\text{NH}}_4\text{OH}+\begin{array}{c}{\text{H}}_3\text{C}-\text{C}=\text{N}-\text{OH}\\ |\\ {\text{H}}_3\text{C}-\text{C}=\text{N}-\text{OH}\end{array}\to \text{B}+{\text{NH}}_4\text{Cl}+{\text{H}}_2\text{O}$ The number of protons that do not involve in hydrogen bonding in the product B is ________.

Number of compounds from the following with zero dipole moment is ____. $\mathrm{HF},{\mathrm{H}}_2,{\mathrm{H}}_2\mathrm{S},\mathrm{C}{\mathrm{O}}_2,\mathrm{N}{\mathrm{H}}_3,\mathrm{B}{\mathrm{F}}_3,\mathrm{C}{\mathrm{H}}_4,\mathrm{CHC}{\mathrm{l}}_3,\mathrm{Si}{\mathrm{F}}_4,{\mathrm{H}}_2\mathrm{O},\mathrm{Be}{\mathrm{F}}_2$

Number of molecules/ions from the following in which the central atom is involved in $\mathrm{s}{\mathrm{p}}^3$ hybridization is ____. $\mathrm{N}{\mathrm{O}}_3^{-},\mathrm{BC}{\mathrm{l}}_3,\mathrm{Cl}{\mathrm{O}}_2^{-},\mathrm{Cl}{\mathrm{O}}_3^{-}$

1. A.2
2. B.4
3. C.1
4. D.3

Which one of the following molecules has maximum dipole moment?

1. A.${\mathrm{CH}}_4$
2. B.${\mathrm{NF}}_3$
3. C.${\mathrm{NH}}_3$
4. D.${\mathrm{PF}}_5$

The correct statement/s about Hydrogen bonding is/are A. Hydrogen bonding exists when H is covalently bonded to the highly electronegative atom. B. Intermolecular H bonding is present in $o$-nitro phenol C. Intramolecular H bonding is present in HF. D. The magnitude of H bonding depends on the physical state of the compound. E. H-bonding has powerful effect on the structure and properties of compounds Choose the correct answer from the options given below:

1. A.A, B, C only
2. B.A only
3. C.A, D, E only
4. D.A, B, D only

Number of compounds / species from the following with non-zero dipole moment is _________. ${\text{BeCl}}_2,{\text{BCl}}_3,{\text{NF}}_3,{\text{XeF}}_4,{\text{CCl}}_4,{\text{H}}_2\text{O},{\text{H}}_2\text{S},\text{HBr},{\text{CO}}_2,{\text{H}}_2,\text{HCl}$