What is the hybridization of the indicated atom in each of the following?
d.
e.
f.

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Step 1: Identify the atom indicated by the arrow in each structure (A, B, and C). In A, the arrow points to the nitrogen atom in the nitrile group. In B, the arrow points to the nitrogen atom in the imine group. In C, the arrow points to the oxygen atom in the ether group.

Step 2: Determine the number of regions of electron density (bonds and lone pairs) around the indicated atom. For A, the nitrogen in the nitrile group is triple-bonded to carbon and has one lone pair. For B, the nitrogen in the imine group is double-bonded to carbon and has one lone pair. For C, the oxygen in the ether group is single-bonded to two carbons and has two lone pairs.

Step 3: Use the number of regions of electron density to determine the hybridization. For A, the nitrogen has two regions of electron density (one triple bond and one lone pair), indicating sp hybridization. For B, the nitrogen has three regions of electron density (one double bond, one single bond, and one lone pair), indicating sp2 hybridization. For C, the oxygen has four regions of electron density (two single bonds and two lone pairs), indicating sp3 hybridization.

Step 4: Recall the geometry associated with each hybridization. sp hybridization corresponds to linear geometry, sp2 hybridization corresponds to trigonal planar geometry, and sp3 hybridization corresponds to tetrahedral geometry.

Step 5: Summarize the hybridization for each indicated atom: A (sp), B (sp2), and C (sp3).

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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 concept in organic chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to form covalent bonds in molecules. The type of hybridization (sp, sp2, sp3) depends on the number of sigma bonds and lone pairs around the central atom, influencing the geometry and reactivity of the molecule.

Types of Hybridization

The main types of hybridization include sp, sp2, and sp3. sp hybridization occurs when one s and one p orbital mix, resulting in two linear orbitals, typically seen in alkynes. sp2 hybridization involves one s and two p orbitals, forming three trigonal planar orbitals, common in alkenes. sp3 hybridization combines one s and three p orbitals, creating four tetrahedral orbitals, typical in alkanes.

Determining Hybridization

To determine the hybridization of an atom, count the number of sigma bonds and lone pairs attached to it. For example, if an atom forms four sigma bonds and has no lone pairs, it is sp3 hybridized. If it has three sigma bonds and one lone pair, it is sp3 hybridized as well, while two sigma bonds and two lone pairs indicate sp hybridization. This analysis is crucial for understanding molecular geometry and reactivity.

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Draw a skeletal structure for each of the compounds.

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Textbook Question

For each of the following molecules, indicate the hybridization of each carbon and give the approximate values of all the bond angles: