The ideas that eventually helped define the nature of chemical bonding were developed early in the 20th century, following the discovery of the electron and the development of quantum mechanics as a theoretical framework for describing the behaviour of electrons in atoms. Chemical bonds are any interactions that cause atoms to join together to form molecules, ions, crystals, and other stable species that make up the familiar materials of daily life.
Download the Class 11 Chemistry Worksheet on Chapter 4 Chemical Bonding and Molecular Structure Set 5 PDF.
CBSE Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure – Set 5
Q-1:Two atoms are connected by a double bond, which shares
a) 2 electrons
b) 1 electron
c) 4 electrons
d) All electrons
Q-2: Which of the following ionic compounds would have the greatest distance between the cation and anion centres in crystals?
a) LiI
b) CsF
c) CsI
d) LiF
Q-3: Which of the following molecules stabilises by removing the electron?
a) C2
b) O2
c) N2
d) H2
Q-4: The number of angles of 109o28’ present in CH4 is
a) 4
b) 2
c) 6
d) 8
Q-5: In a regular square bipyramidal AX5, the number of X-A-X bonds at 180o is
a) One
b) Two
c) Four
d) Three
Q-6: Why does an ionic bond form between two elements with such a large electronegativity difference?
Q-7: The boiling point drops significantly when we transition from HF to HCl, but it rises when we reach HBr and HI. Why?
Q-8: State the difference between bonding and antibonding molecular orbitals.
Q-9: Why cannot a single bond be a pi bond?
Q-10: Why is glycerol more viscous than ethanol?
Q-11: Describe why p-hydroxybenzaldehyde is a high melting solid and o-hydroxybenzaldehyde is a liquid at room temperature.
Q-12: What are the conditions for the H-bonding to occur?
Q-13: Predict whether each of the following molecules is polar or nonpolar.
a) PCl5
b) H2O
c) CH4
d) SO3
Q-14: What significant effects does lattice enthalpy have?
Q-15: Account for the following.
a) N2 has higher bond dissociation energy than NO.
b) N2+ is not a diamagnetic substance.
Q-16: What are the main postulates of VSEPR theory, or Valence Shell Electron Pair Repulsion?
Q-17: The dipole moment of LiH is 1.964 × 10-29 Cm, and the interatomic distance between the Li and H in the molecule is 1.596 Å. Calculate the percentage ionic character of the molecule.
Q-18: Using the VSEPR theory, identify the type of hybridisation and draw the structure of NF3. What are the oxidation states of F and N?
Q-19: Explain the concept of valence electrons using silicon (atomic number 14) as an example.
Q-20: Answer the following questions:
a) What energy change will occur when an atom transforms into a molecule?
b) What kind of orbitals can overlap each other to create a covalent bond?
c) Identify the method typically used to determine electron affinity or lattice energy.
d) From the following, select the compounds that contain ionic, covalent, and coordinate bonds:
MgCl2, CH4, HCl, NH4+, and O3
Download the PDF to access answers to the Chemistry Worksheet for Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure Set – 5.
