Chemical Bonding

23 JEE Main questions · Chemistry

ChemistryJEE Main 21 Jan 2026, Shift 1·Q14·MCQ·Moderate
Open
VSEPR shapes and incomplete octet
Given below are two statements:
Statement I: The number of species among $\ce{SF4}$ , $\ce{NH4+}$ , $\ce{[NiCl4]^2-}$ , $\ce{XeF4}$ , $\ce{[PtCl4]^2-}$ , $\ce{SeF4}$ and $\ce{[Ni(CN)4]^2-}$ , that have tetrahedral geometry is 3.
Statement II: In the set [ $\ce{NO2}$ , $\ce{BeH2}$ , $\ce{BF3}$ , $\ce{AlCl3}$ ], all the molecules have incomplete octet around central atom.
In the light of the above statements, choose the correct answer from the options given below:
1. (1)Statement I is true but Statement II is false
2. (2)Both Statement I and Statement II are false
3. (3)Statement I is false but Statement II is true
4. (4)Both Statement I and Statement II are true
We corrected a printing error in the original paper
Source printed “[NiCl $_4$ ]” (charge missing), “[PtC1 $_4$ ] $^{2-}$ ” and “AIC1 $_3$ ” (digit 1 and capital I for l).
ChemistryJEE Main 21 Jan 2026, Shift 2·Q14·MCQ·Easy–moderate
Open
Covalent bond length comparison
The correct increasing order of C – H(A), C – O(B), C $=$ O(C) and C $\equiv$ N(D) bonds in terms of covalent bond length is:
1. (1)A $<$ B $<$ C $<$ D
2. (2)A $<$ D $<$ C $<$ B
3. (3)D $<$ C $<$ B $<$ A
4. (4)D $<$ C $<$ A $<$ B
ChemistryJEE Main 21 Jan 2026, Shift 2·Q19·MCQ·Easy–moderate
Open
Fajans rule covalent character
Given below are two statements :
Statement I : The correct order in terms of bond dissociation enthalpy is $\ce{Cl2}$ $>$ $\ce{Br2}$ $>$ $\ce{F2}$ $>$ $\ce{I2}$
Statement II : The correct trend in the covalent character of the metal halides is [ $\ce{SnCl4}$ $>$ $\ce{SnCl2}$ ], [ $\ce{PbCl4}$ $>$ $\ce{PbCl2}$ ] and [ $\ce{UF4}$ $>$ $\ce{UF6}$ ]
In the light of the above statements, choose the correct answer from the options given below :
1. (1)Statement I is true but Statement II is false
2. (2)Both Statement I and Statement II are true
3. (3)Statement I is false but Statement II is true
4. (4)Both Statement I and Statement II are false
ChemistryJEE Main 22 Jan 2026, Shift 1·Q2·MCQ·Easy–moderate
Open
Formal charge in lewis structure
The formal charges on the atoms marked as (1) to (4) in the Lewis representation of $\ce{HNO3}$ molecule respectively are
1. (1) $+1$ , 0, 0, $-1$
2. (2)0, $-1$ , 0, $+1$
3. (3)0, $+1$ , 0, $-1$
4. (4)0, 0, $-1$ , $+1$
We corrected a printing error in the original paper
Source printed “The formal changes” and “HnO $_3$ ”.
ChemistryJEE Main 22 Jan 2026, Shift 1·Q18·MCQ·Easy–moderate
Open
Hybridisation of trifluorides
Two p-block elements X and Y form fluorides of the type $\ce{EF3}$ . The fluoride compound $\ce{XF3}$ is a Lewis acid and $\ce{YF3}$ is a Lewis base. The hybridization of the central atoms of $\ce{XF3}$ and $\ce{YF3}$ respectively are
1. (1)Both sp $^3$
2. (2)sp $^2$ and sp $^3$
3. (3)sp $^3$ and sp $^2$
4. (4)Both sp $^2$
We corrected a printing error in the original paper
Source printed “form fluroides of the type”.
ChemistryJEE Main 22 Jan 2026, Shift 2·Q11·MCQ·Easy–moderate
Open
Dipole moment and lone pairs
Among $\ce{H2S}$ , $\ce{H2O}$ , $\ce{NF3}$ , $\ce{NH3}$ and $\ce{CHCl3}$ , identify the molecule (X) with lowest dipole moment value. The number of lone pairs of electrons present on the central atom of the molecule (X) is :
1. (1)2
2. (2)0
3. (3)1
4. (4)3
ChemistryJEE Main 23 Jan 2026, Shift 1·Q15·MCQ·Moderate
Open
Lone pairs and bond angle
Identify the molecule(X) with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among $\ce{HNO3}$ , $\ce{H2SO4}$ , $\ce{NF3}$ and $\ce{O3}$ . Choose the correct bond angle made by the central atom of the molecule (X).
1. (1)120 $^\circ$
2. (2)107 $^\circ$
3. (3)102 $^\circ$
4. (4)116 $^\circ$
ChemistryJEE Main 23 Jan 2026, Shift 2·Q13·MCQ·Moderate
Open
VSEPR shape of xeo2f2
Which statements are NOT TRUE about $\ce{XeO2F2}$ ?
- (A)It has a see-saw shape.
- (B)Xe has 5 electron pairs in its valence shell in $\ce{XeO2F2}$ .
- (C)The O–Xe–O bond angle is close to 180 $^\circ$ .
- (D)The F–Xe–F bond angle is close to 180 $^\circ$
- (E)Xe has 16 valence electrons in $\ce{XeO2F2}$ .
Choose the correct answer from the options given below.
1. (1)B, C and E only
2. (2)B and D only
3. (3)A and D only
4. (4)B, D and E only
ChemistryJEE Main 24 Jan 2026, Shift 1·Q4·MCQ·Easy–moderate
Open
Dipole moment bond order formal charge
Given below are statements about some molecules/ions.
Identify the CORRECT statements.
- (A)The dipole moment value of $\ce{NF3}$ is higher than that of $\ce{NH3}$ .
- (B)The dipole moment value of $\ce{BeH2}$ is zero.
- (C)The bond order of $\ce{O2^{2-}}$ and $\ce{F2}$ is same.
- (D)The formal charge on the central oxygen atom of ozone is $-1$ .
- (E)In $\ce{NO2}$ , all the three atoms satisfy the octet rule, hence it is very stable.
Choose the correct answer from the options given below :
1. (1)A, B, C, D & E
2. (2)B & C only
3. (3)B, C & D only
4. (4)A, C & D only
ChemistryJEE Main 24 Jan 2026, Shift 1·Q6·MCQ·Easy–moderate
Open
VSEPR shapes and hybridisation
Among the following, the CORRECT combinations are :
- (A) $\ce{IF3}$ $\rightarrow$ T-shaped (sp $^3$ d)
- (B) $\ce{IF5}$ $\rightarrow$ Square pyramidal (sp $^3$ d $^2$ )
- (C) $\ce{IF7}$ $\rightarrow$ Pentagonal bipyramidal (sp $^3$ d $^3$ )
- (D) $\ce{ClO4^-}$ $\rightarrow$ Square planar (sp $^2$ d)
Choose the correct answer from the options given below :
1. (1)A, B and C only
2. (2)A and B only
3. (3)A, B, C and D
4. (4)B, C and D Only
ChemistryJEE Main 24 Jan 2026, Shift 2·Q6·MCQ·Easy–moderate
Open
Molecular orbital bond order magnetism
Pair of species among the following having same bond order as well as paramagnetic character will be-
1. (1) $\ce{O2+}$ , $\ce{N2^2-}$
2. (2) $\ce{O2-}$ , $\ce{N2+}$
3. (3) $\ce{O2+}$ , $\ce{N2-}$
4. (4) $\ce{O2-}$ , $\ce{N2-}$
ChemistryJEE Main 28 Jan 2026, Shift 1·Q10·MCQ·Moderate
Open
VSEPR shapes and bond order
Given below are two statements:
Statement I: The number of species among $\ce{BF4^-}$ , $\ce{SiF4}$ , $\ce{XeF4}$ and $\ce{SF4}$ , that have unequal E–F bond lengths is two. Here, E is the central atom.
Statement II: Among $\ce{O2^-}$ , $\ce{O2^{2-}}$ , $\ce{F2}$ and $\ce{O2^+}$ , $\ce{O2^-}$ has the highest bond order.
In the light of the above statements, choose the correct answer from the options given below
1. (1)Both Statement I and Statement II are false
2. (2)Both Statement I and Statement II are true
3. (3)Statement I is true but Statement II is false
4. (4)Statement I is false but Statement II is true

ChemistryJEE Main 28 Jan 2026, Shift 2·Q12·MCQ·Easy–moderate

VSEPR shapes of xenon compounds

Match List-I with List-II according to shape.

List-I		List-II
A.	$\ce{XeO3}$	I.	$\ce{BrF5}$
B.	$\ce{XeF2}$	II.	$\ce{NH3}$
C.	$\ce{XeO2F2}$	III.	$\ce{[I3]-}$
D.	$\ce{XeOF4}$	IV.	$\ce{SF4}$

Choose the correct answer from the options given below :

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

ChemistryJEE Main 2 Apr 2026, Shift 1·Q3·MCQ·Easy–moderate
Open
Molecular orbital bond order
Given below are two statements :
Statement (I) : The correct sequence of bond lengths in the following species is :
$\ce{O2+}$ $<$ $\ce{O2}$ $<$ $\ce{O2-}$ $<$ $\ce{O2^2-}$
Statement (II) : The correct sequence of number of unpaired electrons in the following species is :
$\ce{O2}$ $>$ $\ce{O2+}$ $>$ $\ce{O2-}$ $>$ $\ce{O2^2-}$
In the light of the above statements, choose the correct answer from the options given below :
1. (1)Both Statement I and Statement II are true
2. (2)Both Statement I and Statement II are false
3. (3)Statement I is true but Statement II is false
4. (4)Statement I is false but Statement II is true
ChemistryJEE Main 2 Apr 2026, Shift 2·Q3·MCQ·Easy–moderate
Open
VSEPR shapes of isostructural species
$\ce{SF4}$ is isostructural with :
- (A) $\mathrm{BrF}_4^{\ominus}$
- (B) $\ce{CH4}$
- (C) $\mathrm{IF}_4^{\oplus}$
- (D) $\ce{XeF4}$
- (E) $\ce{XeO2F2}$
Choose the correct answer from the options given below :
1. (1)C only
2. (2)C and E only
3. (3)A and D only
4. (4)B and E only
ChemistryJEE Main 4 Apr 2026, Shift 1·Q21·Numerical·Easy–moderate
Open
Lewis structure bond pairs
According to Lewis theory, the total number of $\sigma$ bond-pairs and lone pair of electrons around the central atom of $\ce{XeO6^4-}$ ion is .
ChemistryJEE Main 4 Apr 2026, Shift 2·Q3·MCQ·Easy–moderate
Open
Molecular orbital pi antibonding
Which of the following pictorial diagram most correctly represents the $\pi^*$ ( $\pi$ – antibonding) molecular orbital between two atoms if the internuclear axis is taken to be in the z-direction ( $\xrightarrow{\text{z--axis}}$ ) ?
1. (1)
2. (2)
3. (3)
4. (4)
ChemistryJEE Main 5 Apr 2026, Shift 1·Q21·Numerical·Easy–moderate
Open
Hybridisation of central atom
Consider the following species
$\ce{BrF5}$ , $\ce{XeF5^-}$ , $\ce{BF4^-}$ , $\ce{ICl4^-}$ , $\ce{XeF4}$ , $\ce{SF4}$ , $\ce{NH4^+}$ , $\ce{ClF3}$ , $\ce{XeF2}$ , $\ce{ICl2^-}$
Number of species having sp $^3$ d hybridized central atom is
ChemistryJEE Main 5 Apr 2026, Shift 2·Q3·MCQ·Easy
Open
Covalent radius and bond length
The covalent radii of atoms A and B are $r_\mathrm{A}$ and $r_\mathrm{B}$ , respectively. The covalent bond length and total length of AB molecule are respectively :
1. (1) $(r_\mathrm{A} + r_\mathrm{B})$ , $2(r_\mathrm{A} + r_\mathrm{B})$
2. (2) $\dfrac{1}{2}(r_\mathrm{A} + r_\mathrm{B})$ , $(r_\mathrm{A} + r_\mathrm{B})$
3. (3) $(r_\mathrm{A} + r_\mathrm{B})$ , $(r_\mathrm{A} + r_\mathrm{B})$
4. (4) $2(r_\mathrm{A} + r_\mathrm{B})$ , $\dfrac{1}{2}(r_\mathrm{A} + r_\mathrm{B})$
ChemistryJEE Main 6 Apr 2026, Shift 1·Q4·MCQ·Moderate
Open
Lewis structures of isoelectronic species
The pairs among
A = [ $\ce{SO3^2-}$ , $\ce{CO3^2-}$ ], B = [ $\ce{O2^2-}$ , $\ce{F2}$ ], C = [ $\ce{CN-}$ , $\ce{CO}$ ], D = [ $\ce{NH3}$ , $\ce{H3O+}$ ] and E = [ $\ce{MnO4^2-}$ , $\ce{CrO4^2-}$ ] that do not have similar Lewis dot structure are :
1. (1)A, B and E
2. (2)A and E
3. (3)B, C and D
4. (4)C and D
ChemistryJEE Main 6 Apr 2026, Shift 2·Q3·MCQ·Moderate
Open
Octet rule exceptions and lone pairs
Given below are two statements:
Statement I : The number of compounds among $\ce{SO2}$ , $\ce{SO3}$ , $\ce{SF4}$ , $\ce{SF6}$ and $\ce{H2S}$ in which sulphur does not obey the Octet rule is 3.
Statement II : Among [ $\ce{H2O}$ , $\ce{ClF3}$ , $\ce{SF4}$ ], [ $\ce{NH3}$ , $\ce{BrF5}$ , $\ce{SF4}$ ], [ $\ce{BrF5}$ , $\ce{ClF3}$ , $\ce{XeF4}$ ] and [ $\ce{XeF4}$ , $\ce{ClF3}$ , $\ce{H2O}$ ], the number of sets in which all the molecules have one lone pair of electrons on the central atom is 1.
In the light of the above statements, choose the correct answer from the options given below :
1. (1)Both Statement I and Statement II are true
2. (2)Both Statement I and Statement II are false
3. (3)Statement I is true but Statement II is false
4. (4)Statement I is false but Statement II is true
We corrected a printing error in the original paper
Source printed options (3) and (4) as “Statement I is true Statement II is false” and “Statement I is false Statement II is true”.
ChemistryJEE Main 6 Apr 2026, Shift 2·Q9·MCQ·Easy–moderate
Open
Bond angle trends
Given below are two statements :
Statement I : $\ce{F2O}$ $<$ $\ce{H2O}$ $<$ $\ce{Cl2O}$ is the correct trend in terms of bond angle.
Statement II : $\ce{SiF4}$ , $\ce{SnF4}$ and $\ce{PbF4}$ are ionic in nature.
In the light of the above statements, choose the correct answer from the options given below :
1. (1)Both Statement I and Statement II are true
2. (2)Both Statement I and Statement II are false
3. (3)Statement I is true but Statement II is false
4. (4)Statement I is false but Statement II is true
ChemistryJEE Main 8 Apr 2026, Shift 2·Q3·MCQ·Easy–moderate
Open
VSEPR shapes of interhalogen ions
Bromine trifluoride autoionizes to form $\mathrm{BrF_2^{\oplus}}$ and $\mathrm{BrF_4^{\ominus}}$ . The shapes of the cation and anion are respectively , and .
1. (1)bent, square planar
2. (2)linear, square planar
3. (3)bent, see-saw
4. (4)linear, tetrahedral