Question 1
Which type of hybridisation results in a linear molecular geometry?
A. sp
B. sp2
C. sp3
D. d2sp3
Question 2
In the molecule of methane (CH4), the carbon atom undergoes:
A. sp hybridisation
B. sp2 hybridization
C. sp3 hybridization
D. d2sp3 hybridization
Question 3
Which of the following molecules has a trigonal planar shape due to hybridisation?
A. BeCl2
B. BF3
C. CH4
D. PCl5
Question 4
The bond angles in a molecule with sp2 hybridisation are:
A. 90°
B. 109.5°
C. 120°
D. 180°
Question 5
Which molecule does NOT exhibit sp3 hybridisation?
A. CH4
B. NH3
C. H2O
D. CO2
Question 6
a) Explain the process of hybridisation and its significance in the formation of covalent bonds. [3]
b) Differentiate between sp, sp2, and sp3 hybridisation in terms of the number of atomic orbitals involved and the resulting molecular geometry. [3]
Question 7
a) Describe the bond angles and molecular shapes associated with sp2 and sp3 hybridised molecules. [3]
b) Why is hybridisation important in explaining the shapes of molecules? [2]
Question 8
a) What is the significance of pi (π) bonds in terms of electron distribution and molecular structure? [3]
b) Given a molecule with a triple bond, explain the types of bonds (sigma and pi) present and their formation. [3]
Question 9
a) Explain the concept of formal charge and its significance in determining the most stable Lewis structure for a molecule. [3]
b) For the molecule CO3^2-, calculate the formal charge on the central carbon atom. [2]
c) How does the concept of resonance relate to the carbonate ion (CO3^2-)? [3]
Question 10
a) Describe the difference between sigma (σ) and pi (π) bonds in terms of their formation and electron distribution. [3]
b) In ethene (C2H4), how many sigma and pi bonds are present? [2]
c) Explain why rotation around a pi bond is restricted, using ethene as an example. [3]