Which hybridization scheme allows the central atom to form more than four bonds? sp³, sp³d, sp²

Name: Chemistry: A Molecular Approach
Author: Tro
ISBN: 9780137832217

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Identify the hybridization schemes given: \(sp^3\), \(sp^3d\), and \(sp^2\).

Understand that \(sp^3\) hybridization involves one s orbital and three p orbitals, allowing for a maximum of four bonds.

Recognize that \(sp^2\) hybridization involves one s orbital and two p orbitals, allowing for a maximum of three bonds.

Consider \(sp^3d\) hybridization, which involves one s orbital, three p orbitals, and one d orbital, allowing for more than four bonds.

Conclude that \(sp^3d\) hybridization allows the central atom to form more than four bonds, typically up to five bonds.

Key Concepts

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

Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals can accommodate the bonding requirements of a central atom, allowing it to form covalent bonds with surrounding atoms. The type of hybridization (e.g., sp, sp2, sp3) determines the geometry and number of bonds that can be formed.

Types of Hybridization

Different types of hybridization correspond to different bonding scenarios. For example, sp3 hybridization involves one s and three p orbitals, allowing for four equivalent bonds, typically seen in tetrahedral geometries. In contrast, sp3d hybridization includes one s, three p, and one d orbital, enabling the formation of five bonds, as seen in trigonal bipyramidal geometries.

Coordination Number

The coordination number refers to the number of bonds formed by a central atom in a molecule. It is crucial for understanding the hybridization scheme, as a higher coordination number indicates the ability to form more bonds. For instance, a central atom with sp3d hybridization can achieve a coordination number of five, allowing it to bond with five other atoms.

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Coordination Numbers

Related Practice

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 11.6 and 11.7. a. CCl4

Textbook Question

Write orbital diagrams (boxes with arrows in them) to represent the electron configurations of carbon before and after sp hybridization.

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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 11.6 and 11.7. c. OF2

Textbook Question

Write orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in SF₂. Circle the electrons involved in bonding. Draw a three-dimensional sketch of the molecule and show orbital overlap. What bond angle do you expect from the unhybridized orbitals? How well does valence bond theory agree with the experimentally measured bond angle of 98.2° ?

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

Which hybridization scheme allows the central atom to form more than four bonds? sp3, sp3d, sp2

Key Concepts

Hybridization

Types of Hybridization

Coordination Number

Which hybridization scheme allows the central atom to form more than four bonds? sp³, sp³d, sp²