Question

Match List-I with List-II:

List-I ( Types of hybridisation )		List-II ( Distribution of hybrid orbitals in space )
A	sp$^3$	(I)	Trigonal bipyramidal
B	dsp$^2$	(II)	Octahedral
C	sp$^3$d	(III)	Tetrahedral
D	sp$^3$d$^2$	(IV)	Square Planar

Choose the correct answer from the options given below:

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

Answer 1

The Correct Option is D

To solve the problem of matching the types of hybridization with their corresponding distribution of hybrid orbitals in space, we need to understand the characteristics of each hybrid and its typical geometry. 

• sp³ hybridization: This configuration involves one s and three p orbitals mixing to form four equivalent hybrid orbitals that are oriented tetrahedrally. Thus, the match for sp³ is (III) Tetrahedral.
• dsp² hybridization: Involves one d, one s, and two p orbitals. This configuration typically results in a square planar geometry. Thus, the match for dsp² is (IV) Square Planar.
• sp³d hybridization: This involves one s, three p, and one d orbital, resulting in five equivalent hybrid orbitals oriented in a trigonal bipyramidal geometry. Therefore, the match for sp³d is (I) Trigonal bipyramidal.
• sp³d² hybridization: Comprising one s, three p, and two d orbitals, it forms six equivalent hybrid orbitals arranged in an octahedral geometry. The match for sp³d² is (II) Octahedral.

The correct matching is therefore:

• A-III (sp³ - Tetrahedral)
• B-IV (dsp² - Square Planar)
• C-I (sp³d - Trigonal bipyramidal)
• D-II (sp³d² - Octahedral)

Therefore, the correct answer is: A-III, B-IV, C-I, D-II.

Answer 2

The correct matches are:

• sp^3 hybridization corresponds to a tetrahedral arrangement (III).
• dsp^2 corresponds to a square planar arrangement (IV).
• sp^3d corresponds to a trigonal bipyramidal geometry (I).
• sp^3d^2 corresponds to an octahedral geometry (II).

These arrangements are based on the number of bonding and lone pairs around the central atom. The geometry is influenced by the concept of VSEPR theory (Valence Shell Electron Pair Repulsion theory), which states that electron pairs around a central atom arrange themselves to minimize repulsion, leading to specific molecular shapes.

For example:

• sp^3 hybridization leads to a tetrahedral shape because four electron pairs (either bonding or lone pairs) surround the central atom, which results in a 109.5° bond angle.
• dsp^2 hybridization typically results in a square planar geometry, where the electron pairs arrange themselves in a flat plane, with 90° angles between them.
• sp^3d hybridization produces a trigonal bipyramidal geometry, with five electron pairs around the central atom, positioned in equatorial and axial positions.
• sp^3d^2 hybridization forms an octahedral shape, where six electron pairs are arranged around the central atom, creating 90° bond angles.