Textbook Question
Which hybridization scheme allows the formation of at least one p bond? sp3, sp2, sp3d2
Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
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Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 61b
Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 61bChapter 10, Problem 61b
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 10.6 and 10.7. b. NH3
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Identify the central atom in NH_3, which is nitrogen (N).
Determine the number of valence electrons for nitrogen and hydrogen. Nitrogen has 5 valence electrons, and each hydrogen has 1 valence electron.
Count the total number of electron domains around the nitrogen atom. In NH_3, there are three N-H bonds and one lone pair, making a total of four electron domains.
Based on the number of electron domains, determine the hybridization of the nitrogen atom. Four electron domains correspond to sp^3 hybridization.
Sketch the NH_3 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 ammonia (NH3), the nitrogen atom undergoes sp3 hybridization, resulting in four equivalent sp3 hybrid orbitals that arrange themselves in a tetrahedral geometry to minimize electron pair repulsion.
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Hybridization
Bonding and Molecular Geometry
Bonding refers to the interactions between atoms that result in the formation of molecules. In NH3, the nitrogen atom forms three sigma bonds with hydrogen atoms and has one lone pair of electrons. The presence of the lone pair affects the molecular geometry, leading to a trigonal pyramidal shape due to the repulsion between the lone pair and the bonding pairs.
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Orbital Overlap Theory
Orbital overlap theory explains how atomic orbitals combine to form bonds in molecules. In NH3, the sp3 hybrid orbitals of nitrogen overlap with the 1s orbitals of hydrogen atoms to form sigma bonds. This overlap is crucial for bond formation, as it allows for the sharing of electron density between the bonded atoms, resulting in stable molecular structures.
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Related Practice
Textbook Question
Which hybridization scheme allows the central atom to form more than four bonds? sp3, sp3d, sp2
Textbook Question
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 10.6 and 10.7. a. CCl4
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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 10.6 and 10.7. c. OF2 d. CO2
Textbook Question
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 10.6 and 10.7.a. CH2Br2 b. SO2 c. NF3 d. BF3
Textbook Question
Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7.
a. COCl2 (carbon is the central atom)
b. BrF5
c. XeF2