Question

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle.

Short answer

To determine the hybridization for each pair of hybrid orbitals, compare their characteristic angles with the angles associated with sp, sp2, and sp3 hybridizations. Specifically, look for angles close to 180° for sp hybridization, 120° for sp2 hybridization, and 109.5° for sp3 hybridization. Determine the most suitable hybridization for each pair based on these comparisons.

Step-by-step solution

Pair 1:

To find the hybridization, compare the given angle with the characteristic angles of sp, sp2, and sp3 hybridizations: - sp hybridization: linear geometry with a characteristic angle of 180° - sp2 hybridization: trigonal planar geometry with a characteristic angle of 120° - sp3 hybridization: tetrahedral geometry with a characteristic angle of 109.5° Now, compare the angle of the given pair with these characteristic angles, and determine which hybridization is the most suitable.

Pair 2:

Repeat the same process as in Pair 1. Compare the angle of the given pair with the characteristic angles of sp, sp2, and sp3 hybridizations. Determine the most suitable hybridization based on this comparison.

Pair 3:

Repeat the same process as in Pair 1 and Pair 2. Compare the angle of the given pair with the characteristic angles of sp, sp2, and sp3 hybridizations. Determine the most suitable hybridization based on this comparison.

Key concepts

sp hybridization

Sp hybridization is an essential concept in molecular geometry, helping us understand how atoms bond in linear structures. When an atom undergoes sp hybridization, it mixes one s orbital with one p orbital. This results in two equivalent sp hybrid orbitals. These orbitals are oriented in such a way that they form a straight line, creating a 180° bond angle between them. This linear arrangement minimizes electron-pair repulsions, following VSEPR theory rules.

You often find sp hybridization in simple diatomic molecules or molecules with a triple bond. A classic example is acetylene ( C_2H_2 ), where sp hybridization allows the carbon atoms to form a triple bond.

Characteristics of sp hybridization include:

• A central atom with two regions of electron density.
• Linear molecular geometry.
• Bond angles of 180°.

Recognizing these traits can help you determine if an atom in a molecule is likely to exhibit sp hybridization and analyze molecular structure effectively.

sp2 hybridization

Sp2 hybridization occurs when one s orbital and two p orbitals blend to form three identical sp2 hybrid orbitals. These orbitals lie in a plane, resulting in a trigonal planar arrangement with 120° angles between them.

This formation is particularly useful for understanding molecules with a double bond. A well-known example is ethene ( C_2H_4 ), where each carbon atom in the double bond region forms sp2 hybrid orbitals.

Main features of sp2 hybridization include:

• A central atom with three regions of electron density.
• Trigonal planar molecular geometry.
• Bond angles of 120°.

Identifying these properties in a molecule can help you understand the distribution of electrons and the molecular shape. Sp2 hybridization is crucial when studying molecules with planar structures and double bonds.

sp3 hybridization

Sp3 hybridization involves the mixing of one s orbital with three p orbitals to form four equivalent sp3 hybrid orbitals. These orbitals point toward the corners of a tetrahedron, resulting in a tetrahedral molecular geometry. The bond angles are approximately 109.5°.

This type of hybridization is what you'll find in many organic compounds, such as methane ( CH_4 ). Here, each carbon atom uses sp3 hybridization to form four sigma bonds with hydrogen atoms.

Key aspects of sp3 hybridization include:

• A central atom with four regions of electron density.
• Tetrahedral molecular geometry.
• Bond angles of about 109.5°.

Understanding sp3 hybridization helps in predicting molecular shapes and bond formations, especially in saturated hydrocarbons and other tetrahedrally coordinated compounds. Recognizing these can assist in visualizing complex molecular structures with ease.