Which of the following molecules(s) show/s paramagnetic behavior? (A) O2 (B) N2 (C) F2 (D) S2 (E) Cl2 Choose the…

Q: Which of the following molecules(s) show/s paramagnetic behavior? (A) O2 (B) N2 (C) F2 (D) S2 (E) Cl2 Choose the correct answer from the options given below:

Paramagnetism Presence of at least one unpaired electron in the molecular orbitals. According to Molecular Orbital Theory (MOT): * O2 has 16 electrons. Its outer configuration contains two unpaired electrons in the anti-bonding orbitals: pi*2px = pi*2py. Thus, it is paramagnetic. * S2 belongs to the same oxygen family group and shares an analogous valence configuration with two unpaired electrons in its anti-bonding pi^* orbitals. Hence, it is also paramagnetic. * N2 (14e-), F2 (18e-), and Cl2 (

Year	2026	2025	2024	Total
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Year

2026

2025

2024

Total

Questions

Solution & Explanation

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Paramagnetism $\implies$ Presence of at least one unpaired electron in the molecular orbitals.

Core Logic

According to Molecular Orbital Theory (MOT):

$O₂$ $O_2$ has 16 electrons. Its outer configuration contains two unpaired electrons in the anti-bonding orbitals: $π 2pₓ = π 2py$ $\pi^{}_{2p_x} = \pi^{}_{2p_y}$. Thus, it is paramagnetic.
$S₂$ $S_2$ belongs to the same oxygen family group and shares an analogous valence configuration with two unpaired electrons in its anti-bonding $π^*$ $\pi^*$ orbitals. Hence, it is also paramagnetic.
$N₂$ $N_2$ (14e-), $F₂$ $F_2$ (18e-), and $Cl₂$ $Cl_2$ (34e-) have completely paired electronic systems and behave diamagnetically.

Pattern Recognition

Both $O₂$ $O_2$ and $S₂$ $S_2$ contain 2 unpaired electrons in their highest occupied molecular orbitals, making them classic examples of paramagnetic diatomic species.

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Class 11 Chemistry: Chemical Bonding and Molecular Structure

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Q77 jee_main_2024_31_jan_morning Molecular Orbital Theory

The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals A. have the same energy B. have the minimum overlap C. have same symmetry about the molecular axis D. have different symmetry about the molecular axis Choose the most appropriate from the options given below:

A. $A, B, C only$ $\text{A, B, C only}$
B. $A and C only$ $\text{A and C only}$
C. $B, C, D only$ $\text{B, C, D only}$
D. $B and D only$ $\text{B and D only}$

Solution

Core Logic

Conditions for the linear combination of atomic orbitals (LCAO) to form molecular orbitals:

The combining atomic orbitals must have the same or nearly the same energy.
The combining atomic orbitals must have the same symmetry about the molecular axis.
The combining atomic orbitals must overlap to the maximum extent (not minimum).

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Class 11 Chemistry: Chemical Bonding and Molecular Structure

Q85 jee_main_2024_31_jan_morning Hybridization

The number of species from the following in which the central atom uses

sp³

hybrid orbitals in its bonding is

NH₃, SO₂, SiO₂, BeCl₂, CO₂, H₂O, CH₄, BF₃

Numerical Answer. Answer: 4 to 4

Solution

Core Logic

Analyzing the hybridization of the central atom in each species:

$NH₃$ $NH_3$: 3 bp + 1 lp = 4 electron domains $arrow sp³$ $\rightarrow sp^3$
$SO₂$ $SO_2$: 2 bp + 1 lp = 3 electron domains $arrow sp²$ $\rightarrow sp^2$
$SiO₂$ $SiO_2$: A giant covalent network where each Si is bonded to 4 oxygens tetrahedrally $arrow sp³$ $\rightarrow sp^3$
$BeCl₂$ $BeCl_2$: 2 bp + 0 lp = 2 electron domains $arrow sp$ $\rightarrow sp$
$CO₂$ $CO_2$: 2 bp + 0 lp = 2 electron domains $arrow sp$ $\rightarrow sp$
$H₂O$ $H_2O$: 2 bp + 2 lp = 4 electron domains $arrow sp³$ $\rightarrow sp^3$
$CH₄$ $CH_4$: 4 bp + 0 lp = 4 electron domains $arrow sp³$ $\rightarrow sp^3$
$BF₃$ $BF_3$: 3 bp + 0 lp = 3 electron domains $arrow sp²$ $\rightarrow sp^2$

Total species with $sp³$ $sp^3$ hybridization: $NH₃, SiO₂, H₂O, CH₄$ $NH_3, SiO_2, H_2O, CH_4$. Total count = 4.

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Class 11 Chemistry: Chemical Bonding and Molecular Structure

Which of the following molecules(s) show/s paramagnetic behavior? (A) $O₂$ $O_2$ (B) $N₂$ $N_2$ (C) $F₂$ $F_2$ (D) $S₂$ $S_2$ (E) $Cl₂$ $Cl_2$ Choose the correct answer from the options given below:

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More Chemical Bonding and Molecular Structure Previous-Year Questions — Page 9

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Which of the following molecules(s) show/s paramagnetic behavior? (A) O₂$O_2$ (B) N₂$N_2$ (C) F₂$F_2$ (D) S₂$S_2$ (E) Cl₂$Cl_2$ Choose the correct answer from the options given below:

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Which of the following molecules(s) show/s paramagnetic behavior? (A) $O₂$ $O_2$ (B) $N₂$ $N_2$ (C) $F₂$ $F_2$ (D) $S₂$ $S_2$ (E) $Cl₂$ $Cl_2$ Choose the correct answer from the options given below: