Chemical bonding is the study of chemical connections between atoms or molecules. This chapter explains why certain atoms can only combine to create new products and why they need to be arranged in a particular way. One of the theories that can thoroughly explain all of the events is VSEPR. Other theories include valence bond theory and molecular orbital theory.
Download Class 11 Chemistry Worksheet on Chapter 4, Chemical Bonding and Molecular Structure Set 3 PDF.
CBSE Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure – Set 3
Q-1: Which of the following possesses an expanded octet?
a) IF7
b) SF6
c) BrF5
d) All of the above
Q-2: Strongly electronegative element B contrasts with strongly electropositive element A. Both are divalent. The resulting compound would be
a) A→B
b) A2+B2-
c) A2-B2+
d) A-B
Q-3: Which of the following compounds shows the highest lattice energy?
a) CsCl
b) KCl
c) RbCl
d) NaCl
Q-4: Which one of the following molecules is formed by p-p overlapping?
a) I2
b) HBr
c) H2S
d) PH3
Q-5: Which of the following H-bonds has the greatest impact on a molecule’s physical characteristics?
a) Intramolecular H-bond
b) Intermolecular H-bond
c) Both of the above
d) All H-bonds
Q-6: State the crucial conditions that must be met for a molecule to undergo hybridisation.
Q-7: Describe why CH4 has a tetrahedral geometry rather than a square planar geometry with a carbon atom in the centre and four H atoms at each corner.
Q-8: What is the reason for the existence of KHF2 but not KHCl2?
Q-9: Give reasons for the following.
a) AlF3 is a high melting solid, whereas SiF4 is a gas.
b) Covalent bonds are directional bonds, while ionic bonds are non-directional.
c) The HSH bond angle in H2S is closer to 90o than the HOH bond angle in H2O.
Q-10: Which of the following has a larger dipole moment? Explain.
1-Butyne or 1-Butene
Q-11:
a) Arrange the following in the order of increasing bond strength F2, N2, O2 and Ne2.
b) Give two resonating structures of N2O that satisfies the octet rule.
Q-12: Using VSEPR theory, identify the type of hybridisation and draw the structure of OF2.
Q-13: Define a single covalent bond and a double covalent bond.
Q-14: Why, in the case of polyatomic molecules, the measurement of bond strength is complicated?
Q-15: Represent diagrammatically the bond moments and the resultant dipole moments in
i) SO3
ii) Cis and trans forms of C2H2Cl2
Q-16: You are given the electronic configuration of five neutral atoms – X, Y, Z, U, and V.
X – 1s2 2s2 2p6 3s2
Y – 1s2 2s2 2p6 3s1
Z – 1s2 2s2 2p1
U – 1s2 2s2 2p5
V – 1s2 2s2 2p6
Write the empirical formula of the substance containing
i) X and U
ii) Y and U
iii) Only U
iv) Only V
Q-17: State whether the atomic orbitals in the list below have positive or negative overlaps.
Q-18: Can the 3pz orbital of one atom combine with the 3py orbital of another atom?
Q-19: Consider the structure and answer the following questions.
a) Which atoms in the structure have the same hybrid state?
b) Arrange the atoms C2, C3 and C5 in decreasing order of s-character of bonding orbitals.
Q-20: Calculate the formal charge of Cl in HClO4.
Download the PDF to access answers to the Chemistry Worksheet for Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure Set – 3.
