Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. b. NH3

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Identify the central atom in the molecule NH3, which is nitrogen (N).

Determine the number of valence electrons for nitrogen (5 electrons) and hydrogen (1 electron each for 3 hydrogens).

Count the total number of electron pairs around the nitrogen atom, including both bonding pairs and lone pairs. NH3 has 3 N-H bonds and 1 lone pair on nitrogen.

Determine the hybridization of the nitrogen atom. With 4 electron pairs (3 bonding pairs and 1 lone pair), the hybridization is sp^3.

Sketch the NH3 molecule showing the sp^3 hybrid orbitals on nitrogen overlapping with the 1s orbitals of hydrogen to form sigma (σ) bonds. Label each N-H bond as a σ bond.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of NH3 (ammonia), the nitrogen atom undergoes sp3 hybridization, resulting in four equivalent sp3 hybrid orbitals that arrange themselves in a tetrahedral geometry, with one orbital containing a lone pair of electrons.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that lead to the formation of molecules. In NH3, nitrogen forms three sigma (σ) bonds with hydrogen atoms through the overlap of sp3 hybrid orbitals with the 1s orbitals of hydrogen. The molecular geometry of NH3 is trigonal pyramidal due to the presence of the lone pair, which influences the spatial arrangement of the bonded hydrogen atoms.

Orbital Overlap Theory

Orbital overlap theory explains how atomic orbitals combine to form molecular orbitals, which are responsible for bonding. In NH3, the overlap of the nitrogen's sp3 hybrid orbitals with the hydrogen's 1s orbitals creates strong sigma bonds. This theory helps visualize the bonding interactions and the resulting molecular structure, emphasizing the importance of orbital orientation and overlap in determining bond strength and angles.

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