NEETClass 11thClass 12thClass 12th PlusJEEClass 11thClass 12thClass 12th PlusClass 6-10Class 6thClass 7thClass 8thClass 9thClass 10thOnline CoursesDistance LearningInternational OlympiadNEETClass 11thClass 12thClass 12th PlusJEE (Main+Advanced)Class 11thClass 12thClass 12th PlusJEE MainClass 11thClass 12thClass 12th PlusClass 6-10Class 6thClass 7thClass 8thClass 9thClass 10thKCET/MHT-CETKCETMHT-CETNEET2025202420232022JEE20262025202420232022Class 6-10JEE MainPrevious Year PapersSample PapersMock TestResultAnalysisSyllabusExam DatePercentile PredictorAnswer KeyCounsellingEligibilityExam PatternJEE MathsJEE ChemistryJEE PhysicsJEE AdvancedPrevious Year PapersSample PapersMock TestResultAnalysisSyllabusExam DateAnswer KeyEligibilityExam PatternRank PredictorNEETPrevious Year PapersSample PapersMock TestResultAnalysisSyllabusExam DateCollege PredictorAnswer KeyRank PredictorCounsellingEligibilityExam PatternBiologyNCERT SolutionsClass 6Class 7Class 8Class 9Class 10Class 11Class 12TextbooksCBSEClass 12Class 11Class 10Class 9Class 8Class 7Class 6SubjectsSyllabusNotesSample PapersQuestion PapersICSEClass 10Class 9Class 8Class 7Class 6State BoardBiharKarnatakaMadhya PradeshMaharashtraTamilnaduWest BengalUttar PradeshOlympiadMathsScienceEnglishSocial ScienceNSOIMONMTCTALLENTEXASATInstant Online ScholarshipAIOT(NEET)ALLEN for SchoolsAbout ALLENBlogsNewsCareersRequest a call backBook a demo
Hybridization of NH3
The hybridization of NH₃ (ammonia) involves the combination of one nitrogen (N) atom's 2s orbital and three 2p orbitals to form four equivalent sp³ hybrid orbitals. This hybridization allows ammonia to form four sigma bonds with hydrogen atoms, resulting in its characteristic tetrahedral molecular geometry. Let’s discuss this in detail.
1.0Hybridization of Ammonia
In detail, the hybridization of ammonia (NH₃) involves the combination of atomic orbitals on the nitrogen atom to form hybrid orbitals suitable for bonding with hydrogen atoms. Let's break down the process:
- Atomic Orbitals of Nitrogen: Nitrogen has five valence electrons, distributed in one 2s orbital and three 2p orbitals (px, py, pz). Electronic Configuration of Nitrogen Atom is 1s2 2s2 2p3
- Promotion of Electrons: One of the electrons in the 2s orbital is promoted to the empty 2p orbital, resulting in four half-filled orbitals. This process allows for the maximum bonding capability of nitrogen.
- Hybridization: The combination of one 2s orbital and three 2p orbitals leads to the formation of four equivalent sp³ hybrid orbitals. These hybrid orbitals are directed towards the corners of a tetrahedron, providing the optimal arrangement for bonding with hydrogen atoms.
- Bond Formation: Ammonia has three hydrogen atoms, and each hydrogen atom shares its electron with one of the sp³ hybrid orbitals of nitrogen. This results in the formation of three sigma (σ) bonds.
The molecular geometry of NH₃ is tetrahedral, with the nitrogen atom at the center and three hydrogen atoms surrounding it. The bond angle in between the hydrogen atoms is around 1070.
2.0Molecular Geometry and Bond Angles of Ammonia
The molecular geometry of ammonia (NH₃) is trigonal pyramidal. The nitrogen atom is at the center, and three hydrogen atoms surround it. Since there is a lone pair on nitrogen, the molecule's shape deviates from the ideal tetrahedral angle.
Bond Angles: The ideal bond angle for a tetrahedral arrangement is 109.50. However, in ammonia, the bond angle is slightly less than this due to the lone pair's presence. The bond angle in NH₃ is approximately 1070.