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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 non-zero dipole moment and highest number of lone-pairs of electrons on the central atom is:

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 \( \mathrm{O=O} \) (double bond) but less than that of a single (\( \mathrm{O-O} \)) 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 (\( \mathrm{O=O} \)) but more than that of a single bond (\( \mathrm{O-O} \)).
In the light of the above statements, choose the correct answer from the options given below:

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

Match the List-I with List-II.

Choose the correct answer from the options given below:

The number of molecules/ions that show linear geometry among the following is ____________.
\( \mathrm{SO_2}, \mathrm{BeCl_2}, \mathrm{CO_2}, \mathrm{N_3^-}, \mathrm{NO_2}, \mathrm{F_2O}, \mathrm{XeF_2}, \mathrm{NO_2^+}, \mathrm{I_3^-}, \mathrm{O_3} \)

Arrange the following compounds in increasing order of their dipole moment:
\( \mathrm{HBr} \), \( \mathrm{H_2S} \), \( \mathrm{NF_3} \) and \( \mathrm{CHCl_3} \)

Which of the following statement is true with respect to \( \mathrm{H_2O} \), \( \mathrm{NH_3} \) and \( \mathrm{CH_4} \)?
(A) The central atoms of all the molecules are \( sp^3 \) hybridized.
(B) The H–O–H, H–N–H and H–C–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 \( \mathrm{CH_4} < \mathrm{NH_3} < \mathrm{H_2O} \).
(D) Both \( \mathrm{H_2O} \) and \( \mathrm{NH_3} \) are Lewis acids and \( \mathrm{CH_4} \) is a Lewis base.
(E) A solution of \( \mathrm{NH_3} \) in \( \mathrm{H_2O} \) is basic. In this solution \( \mathrm{NH_3} \) and \( \mathrm{H_2O} \) act as Lowry-Bronsted acid and base respectively.
Choose the correct answer from the options given below:

Consider \( 'n' \) is the number of lone pair of electrons present in the equatorial position of the most stable structure of \( \mathrm{ClF_{3}} \). The ions from the following with \( 'n' \) number of unpaired electrons are:
A. \( \mathrm{V}^{3+} \) B. \( \mathrm{Ti}^{3+} \) C. \( \mathrm{Cu}^{2+} \) D. \( \mathrm{Ni}^{2+} \) E. \( \mathrm{Ti}^{2+} \)
Choose the correct answers from the options given below:
(\( 1 \)) A and C Only (\( 2 \)) B and D Only (\( 3 \)) A, D and E Only (\( 4 \)) B and C Only

Total number of non-bonded electrons present in \( \mathrm{NO_2^-} \) ion based on Lewis theory is ______.

\( 2.8 \times 10^{-3} \, \text{mol} \) of \( \mathrm{CO_2} \) is left after removing \( 10^{21} \) molecules from its '\( x \)' \( \text{mg} \) sample. The mass of \( \mathrm{CO_2} \) taken initially is:
[Given: \( N_A = 6.02 \times 10^{23} \, \text{mol}^{-1} \)]

In \(SO_2\), \(NO_2^{-}\) and \(N_3^{-}\) the hybridizations at the central atom are respectively:

Which of the following linear combination of atomic orbitals will lead to formation of molecular orbitals in homonuclear diatomic molecules [internuclear axis in \( z \)-direction]?
(A) \( 2p_z \) and \( 2p_x \) (B) \( 2s \) and \( 2p_x \)
(C) \( 3d_{xy} \) and \( 3d_{x^2-y^2} \) (D) \( 2s \) and \( 2p_z \)
(E) \( 2p_z \) and \( 3d_{x^2-y^2} \)
Choose the correct answer from the options given below:

The molecules having square pyramidal geometry are:

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JEE Main 2025 22nd Jan Evening Shift

Arrange the following compounds in increasing order of their dipole moment:
\( \mathrm{HBr} \), \( \mathrm{H_2S} \), \( \mathrm{NF_3} \) and \( \mathrm{CHCl_3} \)