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Given below are two statements:

Statement I: The number of species among \( \mathrm{BF_4^-} \), \( \mathrm{SiF_4} \), \( \mathrm{XeF_4} \) and \( \mathrm{SF_4} \), that have unequal \( \mathrm{E\!-\!F} \) bond lengths is two. Here, \( \mathrm{E} \) is the central atom.

Statement II: Among \( \mathrm{O_2^-} \), \( \mathrm{O_2^{2-}} \), \( \mathrm{F_2} \) and \( \mathrm{O_2^+} \), \( \mathrm{O_2^-} \) has the highest bond order.

In the light of the above statements, choose the correct answer from the options given below

\( \mathrm{SF_4} \) is isostructural with:

A. \( \mathrm{BrF_4^-} \) B. \( \mathrm{CH_4} \) C. \( \mathrm{IF_4^+} \) D. \( \mathrm{XeF_4} \) E. \( \mathrm{XeO_2F_2} \)

Choose the correct answer from the options given below:

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 ?

According to Lewis theory, the total number of \( \sigma \) bond-pairs and lone pair of electrons around the central atom of \( \text{XeO}_6^{4-} \) ion is ________.

Given below are two statements:
Statement I : The number of pairs among \([\mathrm{SiO_2}, \mathrm{CO_2}] , [\mathrm{SnO}, \mathrm{SnO_2}] , [\mathrm{PbO}, \mathrm{PbO_2}] \) and \([\mathrm{GeO}, \mathrm{GeO_2}]\), which contain oxides that are both amphoteric is \( 2 \).
Statement II : \( \mathrm{BF_3} \) is an electron deficient molecule, can act as a Lewis acid, forms adduct with \( \mathrm{NH_3} \) and has a trigonal planar geometry.
In the light of the above statements, choose the correct answer from the options given below:

Given below are two statements:
Statement (I): The correct sequence of bond lengths in the following species is: \( \mathrm{O_2^{+}} < \mathrm{O_2} < \mathrm{O_2^{-}} < \mathrm{O_2^{2-}} \)
Statement (II): The correct sequence of number of unpaired electrons in the following species is: \( \mathrm{O_2} > \mathrm{O_2^{+}} > \mathrm{O_2^{-}} > \mathrm{O_2^{2-}} \)
In the light of the above statements, choose the correct answer from the options given below:

CORRECT order of stability for the following is:
\( \mathrm{CH_2 = CH^-} \), \( \mathrm{CH_3 - CH_2^-} \), \( \mathrm{CH \equiv C^-} \)

Among the following, the CORRECT combinations are

\( \text{A.}\ \mathrm{IF_3} \rightarrow \text{T-shaped}\ (sp^3d) \)
\( \text{B.}\ \mathrm{IF_5} \rightarrow \text{Square pyramidal}\ (sp^3d^2) \)
\( \text{C.}\ \mathrm{IF_7} \rightarrow \text{Pentagonal bipyramidal}\ (sp^3d^3) \)
\( \text{D.}\ \mathrm{ClO_4^-} \rightarrow \text{Square planar}\ (sp^2d) \)

Choose the correct answer from the options given below:

Among \( \text{H}_2\text{S}, \text{H}_2\text{O}, \text{NF}_3, \text{NH}_3 \) and \( \text{CHCl}_3, \) 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:

Pair of species among the following having same bond order as well as paramagnetic character will be:

\\( A=[\\mathrm{SO_3^{2-}},\\,\\mathrm{CO_3^{2-}}],\\; B=[\\mathrm{O_2^{2-}},\\,\\mathrm{F_2}],\\; C=[\\mathrm{CN^-},\\,\\mathrm{CO}],\\; D=[\\mathrm{NH_3},\\,\\mathrm{H_3O^+}] \\) and \\( E=[\\mathrm{MnO_4^{2-}},\\,\\mathrm{CrO_4^{2-}}] \\) that do not have similar Lewis dot structure are:

Consider the following species:
\( \mathrm{BrF_5} \), \( \mathrm{XeF_5^-} \), \( \mathrm{BF_4^-} \), \( \mathrm{ICl_4^-} \), \( \mathrm{XeF_4} \), \( \mathrm{SF_4} \), \( \mathrm{NH_4^+} \), \( \mathrm{ClF_3} \), \( \mathrm{XeF_2} \), \( \mathrm{ICl_2^-} \)
Number of species having \( sp^3d \) hybridized central atom is ______.

The correct increasing order of C–H (A), C–O (B), C=O (C) and C≡N (D) bonds in terms of covalent bond length is:

Given below are two statements:
Statement I: The number of species among \( \mathrm{SF_4} \), \( \mathrm{NH_4^+} \), \( [\mathrm{NiCl_4}]^{2-} \), \( \mathrm{XeF_4} \), \( [\mathrm{PtCl_4}]^{2-} \), \( \mathrm{SeF_4} \) and \( [\mathrm{Ni(CN)_4}]^{2-} \), that have tetrahedral geometry is \( 3 \).
Statement II: In the set \( [\,\mathrm{NO_2}, \mathrm{BeH_2}, \mathrm{BF_3}, \mathrm{AlCl_3}\,] \), 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:

Given below are statements about some molecules/ions.
Identify the CORRECT statements.
A. The dipole moment value of \( \mathrm{NF_3} \) is higher than that of \( \mathrm{NH_3} \).
B. The dipole moment value of \( \mathrm{BeH_2} \) is \( 0 \).
C. The bond order of \( \mathrm{O_2^{2-}} \) and \( \mathrm{F_2} \) is same.
D. The formal charge on the central oxygen atom of ozone is \( -1 \).
E. In \( \mathrm{NO_2} \), all the three atoms satisfy the octet rule, hence it is very stable.
Choose the correct answer from the options given below:

Which statements are NOT TRUE about \( \mathrm{X_e O_{2}F_{2}} \)?
A. It has a see-saw shape.
B. Xe has \( 5 \) electron pairs in its valence shell in \( \mathrm{XeO_{2}F_{2}} \).
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 \( \mathrm{X_e O_{2}F_{2}} \).
Choose the correct answer from the options given below:

Bromine trifluoride autoionizes to form \( \mathrm{BrF_{2}^{\oplus}} \) and \( \mathrm{BrF_{4}^{\oplus}} \). The shapes of the cation and anion are respectively ______ and ______

As compared with chlorocyclohexane, which of the following statements correctly apply to chlorobenzene?
A. The magnitude of negative charge is more on chlorine atom.
B. The C—Cl bond has partial double bond character.
C. C—Cl bond is less polar.
D. C—Cl bond is longer due to repulsion between delocalised electrons of the aromatic ring and lone pairs of electrons of chlorine.
E. The C—Cl bond is formed using \( sp^2 \) hybridised orbital of carbon
Choose the correct answer from the options given below:

The formal charges on the atoms marked as \((1)\) to \((4)\) in the Lewis representation of \( \mathrm{HNO_3} \) molecule respectively are:

Identify the molecule \( (X) \) with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among \( \mathrm{HNO_3} \), \( \mathrm{H_2SO_4} \), \( \mathrm{NF_3} \) and \( \mathrm{O_3} \). Choose the correct bond angle made by the central atom of the molecule \( (X) \).

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JEE Main 2026 8th April Evening Shift

Bromine trifluoride autoionizes to form \( \mathrm{BrF_{2}^{\oplus}} \) and \( \mathrm{BrF_{4}^{\oplus}} \). The shapes of the cation and anion are respectively ______ and ______