University:
University of Phoenix
Course:
CHM 150 | General Chemistry I
Academic year:

2023
Views:

131

Pages:

24
Author:

Natasha Acevedo

Hybridisation Definition: The process of intermixing of two or more orbitals of an atom having nearly the same energy to form the same number of equivalent orbitals (with the same energy, shape, and size) is called hybridisation. Hybridising Orbitals: Orbitals taking part in hybridisation. Hybrid Orbitals: Orbitals formed after hybridisation. Conditions for Hybridisation: The hybridising orbitals should have nearly the same energy. Only the orbitals of one atom take part in hybridisation. Steps for Hybridisation: Promotion/Excitation of Electron: The electron from the orbital having paired electrons gets excited to a vacant orbital (not compulsory). Reorientation of Orbitals: The hybridising orbitals intermix together and reorient to form hybrid orbitals. Types of Hybridisation sp Hybridisation (Linear Hybridisation): Involves the intermixing of one s orbital and one p orbital of an atom to form two equivalent sp hybrid orbitals. These hybrid orbitals orient themselves linearly with an angle of 180°. Each sp hybrid orbital carries 50% s and 50% p character. Example: BeCl₂ (AB₂ type). sp² Hybridisation (Trigonal Hybridisation): Involves the intermixing of one s orbital and two p orbitals of an atom to form three equivalent sp² hybrid orbitals. These hybrid orbitals orient themselves trigonal with an angle of 120° between them. Each sp² hybrid orbital carries 33.3% s and 66.7% p character. Example: BF₃ (AB₃ type). sp³ Hybridisation (Tetrahedral Hybridisation): Involves the intermixing of one s and three p orbitals of an atom to form four equivalent sp³ hybrid orbitals. These hybrid orbitals orient themselves tetrahedrally with a bond angle of 109.5°. Each sp³ hybrid orbital carries 25% s and 75% p character. Example: CH₄ (AB₄ type), NH₃ (AB₃E type), H₂O (AB₂E₂ type). Examples Explained: BeCl₂: Be undergoes sp hybridisation with its 1s and 2p orbitals to form linear BeCl₂. BF₃: B undergoes sp² hybridisation to form trigonal planar BF₃ with bond angles of 120°. CH₄: C undergoes sp³ hybridisation with its 1s and 3p orbitals to form tetrahedral CH₄. NH₃: N undergoes sp³ hybridisation. Out of four hybrid orbitals, three form bonds with H atoms, and one remains as a lone pair, giving NH₃ a pyramidal shape. H₂O: O undergoes sp³ hybridisation. Two hybrid orbitals form bonds with H atoms, and the other two remain as lone pairs, giving H₂O a bent/angular shape.