Chemical Bonding and Molecular Structure Class 11 Worksheet with Answers

Valence Bond Theory

Subtopic

Valence Bond Theory under Chemical Bonding and Molecular Structure for Grade 11 ICSE.

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1.
$Which of the following is a limitation of the simple Valence Bond Theory (Heitler-London model)?$
A. $It explains bond formation$
B. $It explains bond energy$
C. $O_2$
D. $It uses the concept of overlap$
2.
$CH_2=CH_2$
A. $4$
B. $5$
C. $6$
D. $3$
3.
$\sigma$
A. $Two s-orbitals$
B. $One s and one p orbital$
C. $Two p-orbitals (axially)$
D. $All of the above$
4.
$F_2$
A. $s-s$
B. $p-p$
C. $s-p$
D. $p-p$
5.
$sp^3d^2$
A. $d_{xy}$
B. $d_{x^2-y^2}$
C. $d_{xz}$
D. $d_{xy}$
6.
$sp^2$
A. $CO_2$
B. $BeCl_2$
C. $SO_2$
D. $H_2O$
7.
$The concept of 'overlapping of atomic orbitals' was first introduced by:$
A. $Linus Pauling$
B. $Heitler and London$
C. $Lewis$
D. $Kossel$
8.
$C_6H_6$
A. $The energy of the actual molecule and the energy of the most stable canonical structure$
B. $sp^2$
C. $\pi$
D. $C-C$
9.
$AX_4$
A. $sp^3$
B. $dsp^2$
C. $sp^3d^2$
D. $sp^3d$
10.
$sp$
A. $BeCl_2$
B. $CO_2$
C. $XeF_2$
D. $C_2H_2$

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VSEPR Theory

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VSEPR Theory under Chemical Bonding and Molecular Structure for Grade 11 ICSE.

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1.
$A central atom with 6 bond pairs and 0 lone pairs forms an Octahedral shape. What is the bond angle between any two adjacent bonds?$
A. $120^{\circ}$
B. $109.5^{\circ}$
C. $90^{\circ}$
D. $180^{\circ}$
2.
$Which of these molecules has the smallest bond angle?$
A. $CH_{4}$
B. $NH_{3}$
C. $H_{2}O$
D. $BF_{3}$
3.
$XeF_{6}$
A. $4$
B. $5$
C. $6$
D. $7$
4.
$What is the shape of a molecule with steric number 2 and no lone pairs?$
A. $Bent$
B. $Linear$
C. $Trigonal planar$
D. $Tetrahedral$
5.
$SeF_{4}$
A. $Tetrahedral$
B. $Seesaw$
C. $Square planar$
D. $Trigonal pyramidal$
6.
$Which of the following molecules is non-polar due to its symmetrical VSEPR shape?$
A. $NF_{3}$
B. $SF_{4}$
C. $XeF_{4}$
D. $ClF_{3}$
7.
$NH_{2}^{-}$
A. $Linear$
B. $Bent$
C. $Trigonal planar$
D. $Tetrahedral$
8.
$XeF_{4}$
A. $Tetrahedral, 0 lone pairs$
B. $Square planar, 2 lone pairs$
C. $See-saw, 1 lone pair$
D. $Octahedral, 2 lone pairs$
9.
$XeF_{2}$
A. $ICl_{2}^{-}$
B. $I_{3}^{+}$
C. $SCl_{2}$
D. $ClO_{2}^{-}$
10.
$PCl_{5}$
A. $All P-Cl bonds are of equal length.$
B. $Axial bonds are longer than equatorial bonds.$
C. $Equatorial bonds are longer than axial bonds.$
D. $Bond lengths depend on the temperature.$

Download the worksheet for Chemical Bonding and Molecular Structure - VSEPR Theory to practice offline. It includes additional chapter-level practice questions.

Hybridization

Subtopic

Hybridization under Chemical Bonding and Molecular Structure for Grade 11 ICSE.

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1.
$SO_2$
A. $sp$
B. $sp^2$
C. $sp^3$
D. $sp^3d$
2.
$sp^3d^2$
A. $120^\circ$
B. $109.5^\circ$
C. $90^\circ$
D. $180^\circ$
3.
$Which type of bond is formed by the overlapping of hybrid orbitals?$
A. $Pi bond$
B. $Sigma bond$
C. $Hydrogen bond$
D. $Electrovalent bond$
4.
$PCl_3$
A. $sp^2$
B. $sp^3$
C. $sp^3d$
D. $sp$
5.
$XeOF_4$
A. $sp^3d$
B. $sp^3d^2$
C. $sp^3d^3$
D. $sp^3$
6.
$\pi$
A. $Unhybridized p-orbitals$
B. $sp^2$
C. $s-orbitals$
D. $Both B and C$
7.
$NH_2^-$
A. $sp^2$
B. $sp^3$
C. $sp$
D. $sp^3d$
8.
$NH_3$
A. $Fluorine atoms increase the p-character of the N-F bonds$
B. $Fluorine atoms increase the s-character of the N-F bonds$
C. $NF_3$
D. $Steric repulsion between Fluorine atoms is less than Hydrogen$
9.
$Cl_2O_7$
A. $sp^2$
B. $sp^3$
C. $sp^3d$
D. $sp^3d^2$
10.
$TeCl_4$
A. $sp^3$
B. $sp^3d$
C. $sp^3d^2$
D. $sp^2$

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Molecular Orbital Theory

Subtopic

Molecular Orbital Theory under Chemical Bonding and Molecular Structure for Grade 11 ICSE.

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1.
$\pi 2p_x$
A. $Hund's Rule$
B. $Aufbau Principle$
C. $Pauli's Exclusion Principle$
D. $Heisenberg's Uncertainty Principle$
2.
$The total number of molecular orbitals formed is always:$
A. $Half the number of combining atomic orbitals$
B. $Double the number of combining atomic orbitals$
C. $Equal to the number of combining atomic orbitals$
D. $Dependent on the number of valence electrons$
3.
$\pi$
A. $O_2$
B. $N_2$
C. $C_2$
D. $Be_2$
4.
$N_2^+$
A. $2$
B. $2.5$
C. $3$
D. $3.5$
5.
$What is the relationship between the bond order and the bond dissociation energy?$
A. $Bond order is inversely proportional to bond dissociation energy$
B. $Bond order is directly proportional to bond dissociation energy$
C. $There is no relationship between them$
D. $Bond order is equal to the square of bond dissociation energy$
6.
$F_2$
A. $O_2^{2-}$
B. $O_2^-$
C. $N_2^{2-}$
D. $O_2$
7.
$B_2$
A. $\sigma_{1s}^2 \sigma_{1s}^{*2} \sigma_{2s}^2 \sigma_{2s}^{*2} \pi_{2p_x}^1 \pi_{2p_y}^1$
B. $\sigma_{1s}^2 \sigma_{1s}^{*2} \sigma_{2s}^2 \sigma_{2s}^{*2} \sigma_{2p_z}^2$
C. $\sigma_{1s}^2 \sigma_{1s}^{*2} \sigma_{2s}^2 \sigma_{2s}^{*2} \pi_{2p_x}^2$
D. $\sigma_{1s}^2 \sigma_{1s}^{*2} \sigma_{2s}^2 \sigma_{2s}^{*2} \sigma_{2p_z}^1 \pi_{2p_x}^1$
8.
$N_2$
A. $10$
B. $8$
C. $6$
D. $4$
9.
$Which of the following exhibits a bond order of 0.5?$
A. $H_2^+$
B. $He_2^+$
C. $H_2^-$
D. $All of these$
10.
$Which molecular orbital has two nodal planes passing through the internuclear axis?$
A. $None of these$
B. $\sigma_{2s}$
C. $\pi_{2p}$
D. $\sigma_{2p_z}$

Download the worksheet for Chemical Bonding and Molecular Structure - Molecular Orbital Theory to practice offline. It includes additional chapter-level practice questions.

Chemical Bonding and Molecular Structure

Valence Bond Theory

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VSEPR Theory

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Hybridization

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Molecular Orbital Theory

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