Structural Isomerism – JEE Main Previous Year Questions with Solutions
JEE Main Previous Year Papers Questions of Chemistry With Solutions are available at eSaral.   Simulator Previous Years AIEEE/JEE Mains Questions
Q. The alkene that exhibits geometrical isomerism is :- (1) 2–butene (2) 2–methyl–2–butene (3) Propene (4) 2–methyl propene [AIEEE-2009]

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Sol. (1)

Q. The number of stereoisomers possible for a compound of the molecular formula CH3–CH=CH–CH(OH)–Me is :- (1) 4             (2) 6              (3) 3             (4) 2 [AIEEE-2009]

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Sol. (1) exhibits both geometrical as well as optical isomerism. Cis – R Trans – R Cis – S Trans – S

Q. Out of the following, the alkene that exhibits optical isomerism is : (1) 2-methyl-2-pentene (2) 3-methyl-2-pentene (3) 4-methyl-1-pentene (4) 3-methyl-1-pentene [AIEEE-2010]

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Sol. (4)

Q. Identify the compound that exhibits tautomerism :- (1) 2-Pentanone (2) Phenol (3) 2-Butene (4) Lactic acid [AIEEE-2011]

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Sol. (1)

Q. The IUPAC name of the following compounds is : (1) (Z) – 5 – hepten – 3 – yne (2) (Z) – 2 – hepten – 4 – yne (3) (E) – 5 – hepten – 3 – yne (4) (E) – 2 – hepten – 4 – yne [JEE-Main-2012]

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Sol. (4)

Q. Dipole moment is shown by :- (1) trans-2, 3-dichloro- 2-butene (2) 1, 2-dichlorobenzene (3) 1, 4-dichlorobenzene (4) trans-1, 2-dinitroethene [JEE-Main 2012]

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Sol. (2)

Q. Maleic acid and fumaric acids are :- (1) Tautomers (2) Chain isomers (5) Geometrical isomers (4) Functional isomers [JEE-Main 2012]

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Sol. (3)

Q. Monocarboxylic acids are functional isomers of : (1) Esters (2) Amines (3) Ethers (4) Alcohols [JEE-Main 2013]

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Sol. (1) Monocarboxylic acid and Esters $(-\mathrm{COO}-)$ has same general $(-\mathrm{COOH}) .$ Formula $\left[\mathrm{C}_{\mathrm{n}} \mathrm{H}_{2 \mathrm{n}} \mathrm{O}_{2}\right]$ but different FG, so are called functional group isomer.

Q. Arrange in the correct order of stability (decreasing order) for the following molecules: [JEE-Main 2013]

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Sol. (3)

Q. For which of the following molecule significant $\mu \neq 0$ [JEE-Main 2014]

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Sol. (2) Due to presence of $\ell . \mathrm{p}_{(\mathrm{s})}$ on oxygen and sulphur atom which are out of plane hence

Oxidation & Reduction – JEE Main Previous Year Questions with Solutions
JEE Main Previous Year Papers Questions of Chemistry With Solutions are available at eSaral.   Simulator   Previous Years AIEEE/JEE Main Questions
Q. Which of the following will change the colour of acidic dichromate solution. [JEE-MAINS 2013]

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Sol. (A)

Q. [JEE-MAINS 2013]

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Sol. (C)

Q. [JEE-MAINS 2013]

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Sol. (A)

Q. The most suitable reagent for the conversion of $\mathrm{R}-\mathrm{CH}_{2}-\mathrm{OH} \rightarrow \mathrm{R}-\mathrm{CHO}$ is :- (A) $\mathrm{CrO}_{3}$ (B) PCC (Pyridinium chlorochromate) (D) $\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ [JEE-MAINS 2014]

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Sol. (B)

IUPAC Nomenclature – JEE Main Previous Year Questions with Solutions
JEE Main Previous Year Papers Questions of Chemistry With Solutions are available at eSaral.   Simulator   Previous Years AIEEE/JEE Mains Questions
Q. The IUPAC name of neopentane is :- (1) 2–methylpropane (2) 2, 2–dimethylbutane (3) 2–methylbutane (4) 2, 2–dimethylpropane [AIEEE -2009]

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Sol. (4)

Q. The IUPAC name of the compound is :- (1) 1, 2-Epoxy propane (2) Propylene oxide (3) 1, 2–Oxo propane (4) 1, 2–Propoxide [AIEEE -2012(online]

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Sol. (1)

Chemical Bonding – JEE Main Previous Year Questions with Solutions
JEE Main Previous Year Papers Questions of Chemistry With Solutions are available at eSaral. Simulator   Previous Years AIEEE/JEE Mains Questions
Q. The bond dissociation energy of B–F in $\mathrm{BF}_{3}$ is 646 kJ $\mathrm{mol}^{-1}$whereas that of C–F in $\mathrm{CF}_{4}$ is 515 kJ mol–1. The correct reason for higher B–F bond dissociation energy as compared to that of C–F is :- (1) Significant $\mathrm{p} \pi-\mathrm{p} \pi$ interaction between B and F in $\mathrm{BF}_{3}$whereas there is not possibility of such interaction between C and F in $\mathrm{CF}_{4}$. (2) Lower degree of p – p interaction between B and F in $\mathrm{BF}_{3}$ than that between C and F in $\mathrm{CF}_{4}$ (3)Smaller size of B-atom as compared to that of C-atom (4) Stronger  bond between B and F in $\mathrm{BF}_{3}$ as compared to that between C and F in $\mathrm{CF}_{4}$ [AIEEE-2009]

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Sol. (1) Due to back bonding in BF3 molecule all B–F bond having partial double bond character.

Q. Using MO theory predict which of the following species has the shortest bond length ? (1) $\mathrm{o}_{2}^{-}$ (2) $\mathrm{O}_{2}^{2-}$ (3) $\mathrm{O}_{2}^{2+}$ (4) $\mathrm{O}_{2}^{+}$ [AIEEE-2009]

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Sol. (3)

Q. The hybridisation of orbitals of N atom in $\mathrm{NO}_{3}^{-}, \mathrm{NO}_{2}^{+}$ and $\mathrm{NH}_{4}^{+}$ are respectively:- [AIEEE-2011]

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Sol. (4)

Q. The structure of $\mathrm{IF}_{7}$ is :- (1) octahedral (2) pentagonal bipyramid (3) square pyramid (4) trigonal bipyramid [AIEEE-2011]

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Sol. (2)

Q. Among the following the maximum covalent character is shown by the compound :- (1) $\mathrm{AlCl}_{3}$ (2) $\mathrm{MgCl}_{2}$ (3) FeCl $_{2}$ (4) $\mathrm{SnCl}_{2}$ [AIEEE-2011]

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Sol. (1) $\mathrm{Al}^{+3}$ having highest polarizing power than other : having greater covalent character

Q. Which of the following has maximum number of lone pairs associated with Xe (1) $\mathrm{XeO}_{3}$ (2) $\mathrm{XeF}_{4}$ (3) XeF $_{6}$ (4) $\mathrm{XeF}_{2}$ [AIEEE-2011]

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Sol. (4)

Q. 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 [AIEEE-2011]

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Sol. (1) $\mathrm{Ca}^{+2}(\mathrm{C} \equiv \mathrm{C})^{2-}$

Q. The molecule having smallest bond angle is :- (1) $\mathrm{PCl}_{3}$ (2) $\mathrm{NCl}_{3}$ (4) $\mathrm{SbCl}_{3}$ [AIEEE-2012]

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Sol. (4) Bond angle order $\mathrm{NCl}_{3}>\mathrm{PCl}_{3}>\mathrm{AsCl}_{3}>\mathrm{SbCl}_{3}$

Q. In which of the following pairs the two species are not isostructural ? (1) $\mathrm{AIF}_{6}^{3-}$ and $\mathrm{SF}_{6}$ (3) $\mathrm{CO}_{3}^{2-}$ and $\mathrm{NO}_{3}^{-}$ (3) $\mathrm{PCl}_{4}^{+}$ and $\mathrm{SiCl}_{4}$ (4) $\mathrm{PF}_{5}$ and $\mathrm{BrF}_{5}$ [AIEEE-2012]

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Sol. (4)

Q. The number of S–S bonds in $\mathrm{SO}_{3}, \mathrm{S}_{2} \mathrm{O}_{3}^{2-}, \mathrm{S}_{2} \mathrm{O}_{6}^{2-}$ and $\mathrm{S}_{2} \mathrm{O}_{8}^{2-}$ respectively are :- (1) 1, 0, 1, 0 (2) 0, 1, 1, 0 (3) 1, 0, 0, 1 (4) 0, 1, 0, 1 [JEE-MAINS(Online) 2012]

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Sol. (2)

Q. Dipole moment is shown by :- (1) trans-2, 3-dichloro- 2-butene (2) 1, 2-dichlorobenzene (3) 1, 4-dichlorobenzene (4) trans-1, 2-dinitroethene [JEE-MAINS(Online) 2012]

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Sol. (2)

Q. Among the following species which two have trigonal bipyramidal shape ? [JEE-MAINS(Online) 2012]

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Sol. (Bonus)

Q. Among the following, the species having the smallest bond is :- (1) NO (2) $\mathrm{NO}^{+}$ (3) $\mathrm{O}_{2}$ (4) $\mathrm{NO}^{-}$ [JEE-MAINS(Online) 2012]

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Sol. (2)

Q. Based on lattice energy and other considerations, which one of the following alkali metal chloride is expected to have the highest melting point ? (1) RbCl (2) LiCl (3) KCl (4) NaCl [JEE-MAINS(Online) 2012]

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Sol. (4) Highest melting is of NaCl

Q. Which of the following has the square planar structure :- (1) $\mathrm{NH}_{4}^{+}$ (2) $\mathrm{CCl}_{4}$ (3) $\mathrm{XeF}_{4}$ (4) $\mathrm{BF}_{4}^{-}$ [JEE-MAINS(Online) 2012]

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Sol. (3) Hybridisation $\mathrm{Sp}^{3} \mathrm{d}^{2}$ Shape – square planar

Q. The compound of Xenon with zero dipole moment is :- (1) $\mathrm{XeO}_{3}$ (2) $\mathrm{XeO}_{2}$ (3) $\mathrm{XeF}_{4}$ (4) $\mathrm{XeOF}_{4}$ [JEE-MAINS(Online) 2012]

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Sol. (3)

Q. Among the following the molecule with the lowest dipole moment is :- (1) $\mathrm{CHCl}_{3}$ (2) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ (3) $\mathrm{CCl}_{4}$ (4) $\mathrm{CH}_{3} \mathrm{Cl}$ [JEE-MAINS(Online) 2012]

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Sol. (3) $\mathrm{CCl}_{4}<\mathrm{CHCl}_{3}<\mathrm{CH}_{2} \mathrm{Cl}_{2}<\mathrm{CH}_{3} \mathrm{Cl}(\text { Dipolar moment })$

Q. The formation of molecular complex $\mathrm{BF}_{3}-\mathrm{NH}_{3}$ results in a change in hybridisation of boron (1) from $\operatorname{sp}^{3}$ to $\mathrm{sp}^{3} \mathrm{d}$ (2) from $\operatorname{sp}^{2}$ to $\mathrm{dsp}^{2}$ (3) from $\operatorname{sp}^{3}$ to $\mathrm{sp}^{2}$ (4) from $\operatorname{sp}^{2}$ to $\mathrm{sp}^{3}$ [JEE-MAINS(Online) 2012]

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Sol. (4)

Q. Among the following chloro-compound having the lowest dipole moment is :- (1) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ (2) $\mathrm{CH}_{3} \mathrm{Cl}$ (3) (4)

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Sol. (1) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ has lowest dipole moment

Q. Which one of the following molecules is expected to exhibit diamagnetic behaviour ? (1) $\mathrm{C}_{2}$ (2) $\mathrm{N}_{2}$ (3) $\mathrm{O}_{2}$ (4) $\mathrm{S}_{2}$ [AIEEE-2013]

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Sol. (2) $\mathrm{N}_{2}$ is diamagnetic

Q. Which of the following is the wrong statement? (1) ONCl and $\mathrm{ONO}^{-}$ are not isoelectronic (2) $\mathrm{O}_{3}$ molecule is bent (3) Ozone is violet-black in solid state (4) Ozone is diamagnetic gas [JEE-maIN 2013]

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Sol. (1) Number of electron in ONCl an $\mathrm{ONO}^{-}$ is 32 & 24 respectively.

Q. In which of the following pairs of molecules/ions, both the species are not likely to exist ? (1) $\mathrm{H}_{2}^{+}, \mathrm{He}_{2}^{2-}$ (2) $\mathrm{H}_{2}^{-}, \mathrm{He}_{2}^{2-}$ (3) $\mathrm{H}_{2}^{2+}, \mathrm{He}_{2}$ (4) $\mathrm{H}_{2}^{-}, \mathrm{H} \mathrm{e}_{2}^{2+}$ [JEE-main 2013]

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Sol. (3) Bond order of $\mathrm{H}_{2}^{2+} \& \mathrm{He}_{2}$ is zero i.e. these molecule do not exist.

Q. Stability of the species $\mathrm{Li}_{2}, \quad \mathrm{Li}_{2}^{-}$ and $\mathrm{Li}_{2}^{+}$ increases in the order of :- (1) $\mathrm{Li}_{2}<\mathrm{Li}_{2}^{+}<\mathrm{Li}_{2}^{-}$ (2) $\mathrm{Li}_{2}^{-}<\mathrm{Li}_{2}^{+}<\mathrm{Li}_{2}$ (3) $\mathrm{Li}_{2}<\mathrm{Li}_{2}<\mathrm{Li}_{2}^{+}$ (4) $\mathrm{Li}_{2}^{-}<\mathrm{Li}_{2}<\mathrm{Li}_{2}^{+}$ [JEE-main 2013]

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Sol. (2)

Q. Trigonal bipyramidal geometry is shown by: (1) $\mathrm{XeO}_{3} \mathrm{F}_{2}$ (2) $\mathrm{XeOF}_{2}$ (3) $\left[\mathrm{XeF}_{8}\right]^{2-}$ [JEE-MAINS(Online) 2013]

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Sol. (1)

Q. In which of the following ionization processes the bond energy has increased and also the magnetic behaviour has changed from paramagnetic to diamagnetic ? (1) $\mathrm{NO} \rightarrow \mathrm{NO}^{+}$ (2) $\mathrm{O}_{2} \rightarrow \mathrm{O}_{2}^{+}$ (3) $\mathrm{N}_{2} \rightarrow \mathrm{N}_{2}^{+}$ ( 4) $\mathrm{C}_{2} \rightarrow \mathrm{C}_{2}^{+}$ [JEE-MAINS(Online) 2013]

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Sol. (1)

Q. Which one of the following molecules is polar? (1) $\mathrm{CF}_{4}$ (2) $\mathrm{SbF}_{5}$ (3) $\mathrm{IF}_{5}$ (4) $\mathrm{XeF}_{4}$ [JEE-MAINS(Online) 2013]

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Sol. (3)

Q. Oxidation state of sulphur in anions $\mathrm{SO}_{3,}^{2-} \mathrm{S}_{2} \mathrm{O}_{4}^{2-}$ and $\mathrm{S}_{2} \mathrm{O}_{6}^{2-}$ increases in the orders : (1) $\mathrm{S}_{2} \mathrm{O}_{6}^{2-}<\mathrm{S}_{2} \mathrm{O}_{4}^{2-}<\mathrm{SO}_{3}^{2-}$ (2) $\mathrm{SO}_{3}^{2-}<\mathrm{S}_{2} \mathrm{O}_{4}^{2-}<\mathrm{S}_{2} \mathrm{O}_{6}^{2-}$ (3) $\mathrm{S}_{2} \mathrm{O}_{4}^{2-}<\mathrm{SO}_{3}^{2-}<\mathrm{S}_{2} \mathrm{O}_{6}^{2-}$ (4) $\mathrm{S}_{2} \mathrm{O}_{4}^{2-}<\mathrm{S}_{2} \mathrm{O}_{6}^{2-}<\mathrm{SO}_{3}^{2-}$ [JEE-MAINS(Online) 2013]

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Sol. (3)

Q. Bond order normally gives idea of stability of a molecular species. All the molecules viz. $\mathrm{H}_{2}, \mathrm{Li}_{2}$ and $\mathrm{B}_{2}$ have the same bond order yet they are not equally stable. Their stability order is: (1) $\mathrm{Li}_{2}>\mathrm{H}_{2}>\mathrm{B}_{2}$ (2) $\mathrm{H}_{2}>\mathrm{B}_{2}>\mathrm{Li}_{2}$ (3) $\mathrm{B}_{2}>\mathrm{H}_{2}>\mathrm{Li}_{2}$ (4) $\mathrm{Li}_{2}>\mathrm{B}_{2}>\mathrm{H}_{2}$ [JEE-MAINS(Online) 2013]

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Sol. (2)

Q. The solubility order for alkali metal fluoride in water is : (1) $\mathrm{LiF}<\mathrm{NaF}<\mathrm{KF}<\mathrm{RbF}$ (2) $\mathrm{LiF}>\mathrm{NaF}>\mathrm{KF}>\mathrm{RbF}$ (3) $\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}<\mathrm{LiF}$ (4) $\mathrm{LiF}<\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}$ [JEE-MAINS(Online) 2013]

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Sol. (1) Solubility order LiF < NaF < KF < RbF

Q. $\mathrm{XeO}_{4}$ molecule is tetrahedral having : (1) Two p $\pi$ -d $\pi$ bonds (2) Four p $\pi$ – d $\pi$ bonds (3) One $\mathrm{p} \pi-\mathrm{d} \pi$ bond (4) Three p $\pi$ -d $\pi$ bonds [JEE-MAINS(Online) 2013]

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Sol. (2)

Q. Bond distance in HF is 9.17 × $10^{-11}$ m. Dipole moment of HF is 6.104 × 10–30 Cm. The percent ionic character in HF will be : (electron charge = 1.60 × $10^{-19}$ C) (1) 61.0% (2) 38.0% (3) 35.5% (4) 41.5% [JEE-MAINS(Online) 2013]

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Sol. (4)

Q. The shape of $\mathrm{IF}_{6}^{-}$ is : (1) Trigonally distorted octahedron (2) Pyramidal (3) Octahedral (4) Square antiprism [JEE-MAINS(Online) 2013]

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Sol. (1)

Q. Which has trigonal bipyramidal shape ? (1) $\mathrm{XeOF}_{4}$ (2) $\mathrm{XeO}_{3}$ (3) $\mathrm{XeO}_{3} \mathrm{F}_{2}$ (4) $\mathrm{XeOF}_{2}$ [JEE-MAINS(Online) 2013]

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Sol. (3)

Q. The catenation tendency of C, Si and Ge is in the order Ge < Si < C. The bond energies (in kJ $\mathrm{mol}^{-1}$) of C — C, Si —Si and Ge—Ge bonds are respectively : (1) 348, 260, 297 (2) 348, 297, 260 (3) 297, 348, 260 (4) 260, 297, 348 [JEE-MAINS(Online) 2013]

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Sol. (2) Catenation/Bond energy order C – C > Si – Si > Ge – Ge

Q. In which of the following sets, all the given species are isostructural ? (1) $\mathrm{BF}_{3}, \mathrm{NF}_{3}, \mathrm{PF}_{3}, \mathrm{AlF}_{3}$ (2) $\mathrm{PCl}_{3}, \mathrm{AlCl}_{3}, \mathrm{BCl}_{3}, \mathrm{SbCl}_{3}$ (3) $\mathrm{BF}_{4}^{-}, \mathrm{CCl}_{4}, \mathrm{NH}_{4}^{+}, \mathrm{PCl}_{4}^{+}$ (4) $\mathrm{CO}_{2}, \mathrm{NO}_{2}, \mathrm{ClO}_{2}, \mathrm{SiO}_{2}$ [JEE-MAINS(Online) 2013]

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Sol. (3) $\mathrm{BF}_{4}^{-}, \mathrm{CC}_{4}, \mathrm{NH}_{4}^{+}, \mathrm{PCl}_{4}^{+}$ are terahedral

Q. The internuclear distances in O —O bonds for O, $\mathrm{O}_{2}, \mathrm{O}^{-}$2 and O respectively are : (1) 1.49 Å, 1.21 Å, 1.12 Å, 1.30 Å (2) 1.30 Å, 1.49 Å, 1.12 Å, 1.21 (3) 1.12 Å, 1.21 Å, 1.30 Å, 1.49 Å (4) 1.21 Å, 1.12 Å, 1.49 Å, 1.30 Å [JEE-MAINS(Online) 2013]

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Sol. (3)

Q. Which one of the following properties is not shown by NO ? (1) It combines with oxygen to form nitrogen dioxide (2) It’s bond order is 2.5 (3) It is diamagnetic in gaseous state (4) It is a neutral oxide [JEE-main 2014]

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Sol. (3)

Q. For which of the following molecule significant $\mu \neq 0$ [JEE-main 2014]

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Sol. (2)

Q. The number and type of bonds in $\mathrm{C}_{2}^{2-} \mathrm{ion}$ in $\mathrm{CaC}_{2}$ are: (1) Two $\sigma$ bonds and one $\pi-$ bond (2) Two $\sigma$ bonds and two $\pi-$ bonds (3) One $\sigma$ bond and two $\pi-$ bonds (4) One $\sigma$ bond and one $\pi-$ bond [JEE-MAINS(Online) 2014]

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Sol. (3)

Q. For the compounds $\mathrm{CH}_{3} \mathrm{Cl}, \mathrm{CH}_{3} \mathrm{Br}, \mathrm{CH}_{3} \mathrm{I}$ and $\mathrm{CH}_{3} \mathrm{F}$ (1) $\mathrm{CH}_{3} \mathrm{F}<\mathrm{CH}_{3} \mathrm{Br}<\mathrm{CH}_{3} \mathrm{Cl}<\mathrm{CH}_{3} \mathrm{I}$ (2) $\mathrm{CH}_{3} \mathrm{F}<\mathrm{CH}_{3} \mathrm{Cl}<\mathrm{CH}_{3} \mathrm{Br}<\mathrm{CH}_{3} \mathrm{I}$ (3) $\mathrm{CH}_{3} \mathrm{Cl}<\mathrm{CH}_{3} \mathrm{Br}<\mathrm{CH}_{3} \mathrm{F}<\mathrm{CH}_{3} \mathrm{I}$, the correct order of increasing C-halogen bond length is : (4) $\mathrm{CH}_{3} \mathrm{F}<\mathrm{CH}_{3} \mathrm{I}<\mathrm{CH}_{3} \mathrm{Br}<\mathrm{CH}_{3} \mathrm{Cl}$ [JEE-MAINS(Online) 2014]

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Sol. (2)

Q. Which of the following has unpaired electron(s) ? (1) $\mathrm{O}_{2}^{-}$ (2) $\mathrm{N}_{2}^{2+}$ (3) $\mathrm{O}_{2}^{2-}$ (4) $\mathrm{N}_{2}$ [JEE-MAINS(Online) 2014]

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Sol. (1) $\mathrm{O}_{2}^{-}$ ha one unpaired electron

Q. In allene $\left(\mathrm{C}_{3} \mathrm{H}_{4}\right)$, the type(s) of hybridization of the carbon atoms is (are): (1) only sp $^{2}$ (2) $\mathrm{sp}^{2}$ and $\mathrm{sp}$ (3) sp and sp $^{3}$ (4) $\mathrm{sp}^{2}$ and $\mathrm{sp}^{3}$ [JEE-MAINS(Online) 2014]

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Sol. (2)

Q. Shapes of certain interhalogen compounds are stated below. Which one of them is not correctly stated? (1) IF $_{7}:$ Pentagonal bipyramid (2) BrF $_{5}:$ Trigonal bipyramid (4) $\mathrm{BrF}_{3}:$ Planar T-shaped [JEE-MAINS(Online) 2014]

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Sol. (2) $\mathrm{BrF}_{5}$ have square pyramidal shape.

Q. The correct order of bond dissociation energy among $\mathrm{N}_{2}, \mathrm{O}_{2}, \mathrm{o}_{2}^{-}$ is shown in which of the following arrangements? (1) $\mathrm{N}_{2}>\mathrm{O}_{2}>\mathrm{O}_{2}^{-}$ (2) $\mathrm{O}_{2}>\mathrm{O}_{2}^{-}>\mathrm{N}_{2}$ (3) $\mathrm{N}_{2}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}$ (4) $\mathrm{O}_{2}^{-}>\mathrm{O}_{2}>\mathrm{N}_{2}$ [JEE-MAINS(Online) 2014]

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Sol. (1)

Q. Which of the following molecules has two sigma$(\sigma)$ and two $\operatorname{pi}(\pi)$ bonds :- (1) HCN (2) $\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}$ (3) $\mathrm{N}_{2} \mathrm{F}_{2}$ (4) $\mathrm{C}_{2} \mathrm{H}_{4}$ [JEE-MAINS(Online) 2014]

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Sol. (1)

Q. Which one of the following molecules is paramagnetic? (1) NO ( 2) $\mathrm{O}_{3}$ (3) $\mathrm{N}_{2}$ (4) CO [JEE-MAINS(Online) 2014]

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Sol. (1) NO has unpaired e $^{-} \therefore$ paramagnetic is nature

Q. Amongst LiCl, RbCl, $\mathrm{BeCl}_{2}$ and $\mathrm{MgCl}_{2}$ the compounds with the greatest and the least ionic character, respectively are : (1) $\mathrm{RbCl}$ and $\mathrm{MgCl}_{2}$ (2) LiCl and RbCl (3) $\mathrm{MgCl}_{2}$ and $\mathrm{BeCl}_{2}$ (4) $\mathrm{RbCl}$ and $\mathrm{BeCl}_{2}$ [JEE-MAINS(Online) 2014]

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Sol. (4) RbCl has highest ionic & and $\mathrm{BeCl}_{2}$ is most covalent

Q. The species in which the N atom is in a state of sp hybridization is :- (1) $\mathrm{NO}_{2}$ (2) $\mathrm{NO}_{2}^{+}$ (3) $\mathrm{NO}_{2}^{-}$ (4) $\mathrm{NO}_{3}^{-}$ [JEE-MAINS 2016]

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Sol. (2)

Q. Which of the following species is not paramagnetic :- (1)NO (2) CO (3) $\mathrm{O}_{2}$ (4) $\mathrm{B}_{2}$ [JEE-MAINS 2017]

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Sol. (2)

Q. Total number of lone pair of electrons in $\mathrm{I}_{3}^{-} \mathrm{ion}$ is (1) 6 (2) 9 (3) 12 (4) 3 [JEE-MAINS 2018]

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Sol. (2)

Q. According to molecular orbital theory, which of the following will not be a viable molecule ? (1) $\mathrm{He}_{2}^{+}$ (2) $\mathrm{H}_{2}^{-}$ (3) $\mathrm{H}_{2}^{2-}$ (4) $\mathrm{He}_{2}^{2+}$ [JEE-MAINS 2018]

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Sol. (3)

Q. Which of the following compounds contain(s) no covalent bond(s) ? $\mathrm{KCl}, \mathrm{PH}_{3}, \mathrm{O}_{2}, \mathrm{B}_{2} \mathrm{H}_{6}, \mathrm{H}_{2} \mathrm{SO}_{4}$ $(1) \mathrm{KCl}, \mathrm{H}_{2} \mathrm{SO}_{4}$ (2) KC1 (3) $\mathrm{KCl}, \mathrm{B}_{2} \mathrm{H}_{6}$ (4) $\mathrm{KCl}, \mathrm{B}_{2} \mathrm{H}_{6}, \mathrm{PH}_{3}$ [JEE-MAINS 2018]

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Sol. (2)