Question

Match List I with List II:

Choose the correct answer from the options given below:

• A. A-I, B-IV, C-III, D-II
• B. A-IV, B-II, C-III, D-I
• C. A-IV, B-I, C-II, D-III
• D. A-II, B-I, C-IV, D-III

Hint:

Remember that the hybridization and geometry of a molecule are largely determined by the number of bonding and lone pairs on the central atom. For compounds with xenon, the hybridization can often be sp\textsuperscript{3}, sp\textsuperscript{3d}, or sp\textsuperscript{3d\textsuperscript{2}} depending on the number of bonds and lone pairs.

Answer 1

The Correct Option is D

To determine the molecular geometry, the number of electron pairs (bonding and lone) around the central Xenon atom must be calculated for each molecule.

A. XeO₃

• Xenon possesses 8 valence electrons. Each oxygen atom donates 2 electrons for bonding. Consequently, Xenon forms 3 double bonds with the 3 oxygen atoms, leaving one lone pair. The total number of electron pairs around Xenon is 4 (3 bonding pairs + 1 lone pair).

• This configuration results in sp³ hybridization. The presence of a lone pair leads to a pyramidal geometry.

B. XeF₂

• Xenon has 8 valence electrons. Each fluorine atom contributes 1 electron for bonding. Therefore, Xenon forms 2 single bonds with the 2 fluorine atoms, leaving three lone pairs. The total electron pairs around Xenon are 5 (2 bonding pairs + 3 lone pairs).

• This configuration yields sp³d hybridization. To minimize repulsion, the three lone pairs occupy equatorial positions, resulting in a linear geometry.

C. XeOF₄

• Xenon contains 8 valence electrons. Each fluorine atom contributes 1 electron for bonding, and oxygen contributes 2 electrons for bonding. Thus, Xenon forms 4 single bonds with the 4 fluorine atoms and 1 double bond with the oxygen atom, leaving one lone pair. The total electron pairs around Xenon are 6 (5 bonding pairs + 1 lone pair).

• This configuration results in sp³d² hybridization. With one lone pair, the geometry is square pyramidal.

D. XeF₆

• Xenon has 8 valence electrons. Each fluorine atom contributes 1 electron for bonding. Consequently, Xenon forms 6 single bonds with the 6 fluorine atoms, leaving one lone pair. The total electron pairs around Xenon are 7 (6 bonding pairs + 1 lone pair).

• Due to steric hindrance, the molecule does not adopt an octahedral geometry. According to the VSEPR model, the molecule is predicted to have a distorted octahedral geometry. The central Xenon atom has seven electron pairs (6 bonds and 1 lone pair), causing its geometry to be distorted octahedral.

Matching the compounds with their geometries:

A (XeO₃) - II (sp³ pyramidal)

B (XeF₂) - I (sp³d linear)

C (XeOF₄) - IV (sp³d² square pyramidal)

D (XeF₆) - III (sp³d distorted octahedral)

The correct match is (4) A-II, B-I, C-IV, D-III