Which type of hybridisation results in a linear molecular geometry?

A. sp

B. sp2

C. sp3

D. d2sp3

In the molecule of methane (CH4), the carbon atom undergoes:

A. sp hybridisation

B. sp2 hybridization

C. sp3 hybridization

D. d2sp3 hybridization

Which of the following molecules has a trigonal planar shape due to hybridisation?

A. BeCl2

B. BF3

C. CH4

D. PCl5

The bond angles in a molecule with sp2 hybridisation are:

A. 90°

B. 109.5°

C. 120°

D. 180°

Which molecule does NOT exhibit sp3 hybridisation?

A. CH4

B. NH3

C. H2O

D. CO2

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]

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]

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]

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]

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]

The hybridisation of the central atom in SF6 is:

A. sp

B. sp2

C. sp3

D. d2sp3

Which of the following is NOT a characteristic of hybrid orbitals?

A. They are formed by the mixing of atomic orbitals.

B. They are always equivalent in energy.

C. They can explain the geometry of molecules.

D. They result in the formation of pi bonds.

In which of the following molecules is the central atom's hybridisation sp?

A. CH4

B. SO2

C. BeCl2

D. NH3

The importance of hybridisation in chemistry is:

A. It explains the shapes of molecules.

B. It predicts the reactivity of molecules.

C. It determines the polarity of molecules.

D. All of the above.

Which type of hybridisation results in a tetrahedral molecular geometry?

A. sp

B. sp2

C. sp3

D. d2sp3

a) What is the geometry and bond angle associated with sp hybridisation? [2]

b) Explain the importance of hybridisation in determining the geometry of molecules like methane (CH4). [3]

c) For a molecule with the formula AX3E, where A is the central atom, X represents bonded atoms, and E represents a lone pair, what type of hybridisation is expected and what is the molecular shape? [3]

a) Describe the concept of resonance and its importance in molecules like benzene (C6H6). [3]

b) How does the presence of resonance structures affect the stability of a molecule? [2]

c) Given that benzene has alternating single and double bonds in its structure, explain why all the carbon-carbon bond lengths in benzene are equivalent. [3]

a) Describe the formation of sp hybrid orbitals in terms of the combination of atomic orbitals. [2]

b) Given a molecule with a central atom undergoing sp hybridisation, predict its molecular geometry and bond angle. [2]

c) Explain the significance of formal charge in determining the most stable resonance structure for a molecule. [3]

d) For the molecule NO3^-, calculate the formal charge on the central nitrogen atom. [3]

a) Differentiate between sp2 and sp3 hybridisation in terms of the number of atomic orbitals involved and the resulting hybrid orbitals. [3]

b) For a molecule with the formula AX3, where A is the central atom and X represents bonded atoms, predict the type of hybridisation and the molecular shape. [2]

c) Explain the importance of pi bonds in determining the rotation and flexibility of molecules. [3]

d) In ethyne (C2H2), how many sigma and pi bonds are present? [2]

a) Describe the concept of resonance structures and their importance in explaining the electron distribution in molecules. [3]

b) For the molecule SO3, how does resonance contribute to its structure? [3]

c) Explain the geometry and bond angles associated with sp3 hybridisation. [2]

d) Using ammonia (NH3) as an example, describe the effect of lone pairs on molecular geometry in sp3 hybridised molecules. [2]