This chapter explains the concept of orbital hybridization, its role in determining molecular geometry, and its importance in chemical bonding. It is a key topic in school and undergraduate chemistry, essential for Class 11–12 students, competitive exam aspirants, and undergraduate learners, bridging atomic theory with molecular structure.
In this section, you will study:
Concept of hybridization and types of hybrid orbitals (sp, sp², sp³, sp³d, sp³d²)
Formation of sigma (σ) and pi (π) bonds
VSEPR theory and prediction of molecular shapes
Hybridization in simple molecules and complex organic compounds
Relationship between hybridization, bond angles, and molecular geometry
Examples of hybridization in functional groups and aromatic systems
NCERT-aligned explanations, diagrams, MCQs, and exam-oriented questions
The content is structured to build conceptual clarity, improve visual and spatial understanding, and prepare students for school examinations, NEET, JEE, and undergraduate assessments.
Develop a strong foundation in chemical bonding by mastering hybridization to predict molecular shapes, bond types, and chemical reactivity.
Q. In which of the following compounds does the central atom exhibit sp3d2 hybridization?
A.
SF6
B.
XeF4
C.
NH3
D.
CCl4
Solution
In SF6 (sulfur hexafluoride), the sulfur atom is sp3d2 hybridized, allowing it to form six sigma bonds with fluorine atoms.
