The hybridization of an atom in trimethylamine is

English Biology
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the hybridization of an atom in trimethylamine is

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The Hybridization of an Atom in Trimethylamine

Answer:

Trimethylamine (chemical formula N(CH₃)₃) consists of a nitrogen atom bonded to three methyl groups. To determine the hybridization of the nitrogen atom in trimethylamine, we need to analyze its molecular structure, bonding, and electronic configuration.

Step-by-Step Explanation of Hybridization in Trimethylamine

  1. Electron Configuration of Nitrogen:
    Nitrogen (atomic number 7) has the electron configuration:

    1s^2 2s^2 2p^3

    The valence shell consists of 2s and 2p orbitals.

  2. Bonding Structure in Trimethylamine:
    The nitrogen atom in trimethylamine is covalently bonded to three methyl groups via single bonds (C-N bonds) and has one lone pair of electrons. This gives the nitrogen atom a total of four regions of electron density (three bonds + one lone pair).

  3. Electron Geometry Determination:
    According to VSEPR (Valence Shell Electron Pair Repulsion) theory, when there are four regions of electron density around an atom, the electron geometry is tetrahedral.

  4. Hybridization:
    To accommodate four regions of electron density, the nitrogen atom undergoes sp³ hybridization. This involves mixing one s orbital and three p orbitals to form four equivalent sp³ hybrid orbitals, which are arranged tetrahedrally.

  5. Bonding Arrangement:

    • Three of the sp³ hybrid orbitals on nitrogen overlap with the sp³ orbitals of the three adjacent carbon atoms (from methyl groups) to form sigma bonds.
    • The fourth sp³ hybrid orbital contains a lone pair of electrons.

  6. Final Molecular Geometry:
    The molecular geometry of trimethylamine is trigonal pyramidal, because the lone pair on nitrogen slightly pushes the bonded atoms away, reducing bond angles from the ideal tetrahedral angle (109.5°) to approximately 107°.

Summary Table

Property Trimethylamine (N(CH₃)₃)
Central Atom Nitrogen (N)
Regions of Electron Density 4 (Three bonds + One lone pair)
Electron Geometry Tetrahedral
Hybridization of Nitrogen sp³
Molecular Geometry Trigonal Pyramidal
Bond Angle ~107°

Key Points to Remember

  1. Hybridization is determined by the number of regions of electron density around the atom.
  2. Trimethylamine’s nitrogen atom has 4 regions of electron density and adopts sp³ hybridization.
  3. Due to the lone pair, the molecular geometry is trigonal pyramidal instead of tetrahedral.

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