Problem 9 Describe the geometry and bond a... [FREE SOLUTION]

Chapter 14: Problem 9

Describe the geometry and bond angles when a carbon atom forms four single bonds.

Short Answer

Expert verified

A carbon atom with four single bonds has a tetrahedral geometry with bond angles of 109.5 degrees.

Step by step solution

Identify the Hybridization

When a carbon atom forms four single bonds, it undergoes sp3 hybridization. This means one s orbital mixes with three p orbitals to form four equivalent sp3 hybrid orbitals.

Determine the Molecular Geometry

The four sp3 hybrid orbitals arrange themselves as far apart as possible to minimize electron pair repulsion. This leads to a tetrahedral molecular geometry.

Calculate the Bond Angles

In a tetrahedral geometry, the bond angles are approximately 109.5 degrees. This angle is the result of the symmetric distribution of the hybrid orbitals around the central carbon atom.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Hybridization

Hybridization is a fundamental concept in chemistry that explains how atomic orbitals mix to form new, hybrid orbitals that can then be used to form chemical bonds. In simple terms, it's like taking separate ingredients and blending them together to make a new dish. For carbon, when it forms four single covalent bonds, it undergoes a process known as sp3 hybridization.

During sp3 hybridization, one s orbital and three p orbitals in the carbon atom merge to generate four identical sp3 hybrid orbitals. These hybrid orbitals have the same shape and energy level, enabling the carbon atom to form stable bonds with four other atoms.

This hybridization allows the efficient overlap of orbitals, leading to strong and stable covalent bonds.
It also provides a framework for understanding bond angles and molecular geometry.

Tetrahedral Geometry

When you hear the term 'tetrahedral geometry,' think of a simple pyramid with a triangular base and a peak. This is the geometric shape formed when carbon undergoes sp3 hybridization, as it creates a perfect scenario for minimizing electron pair repulsion.

In this configuration, the four sp3 hybrid orbitals of carbon arrange themselves as far from each other as possible. Imagine these orbitals as extending towards the four corners of a tetrahedron, ensuring they are evenly distributed in space.

This three-dimensional shape is common for molecules with a central atom making four bonds.
The symmetry of this geometry provides molecules with certain physical and chemical properties, like stability and minimized electron cloud distortion.

Bond Angles

Bond angles are critical in understanding the shape and nature of molecular structures. In a perfect tetrahedral geometry, the bond angles are ideally 109.5 degrees. This angle is a direct result of the spatial arrangement of the sp3 hybrid orbitals.

A bond angle of 109.5 degrees represents the most energetically favorable and stable configuration for molecules like methane, which contains a central carbon atom with four bonds.

The equal distribution of bonds at this angle reduces steric hindrance, which is basically the crowding of molecules or atoms.
These angles help predict how a molecule will interact chemically and physically with others.

Understanding why bond angles are 109.5 degrees can assist in predicting the behavior of more complex molecules with similar hybridization and geometric arrangements.

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91影视

Describe the geometry and bond angles when a carbon atom forms four single bonds.

Short Answer

Step by step solution

Identify the Hybridization

Determine the Molecular Geometry

Calculate the Bond Angles

Key Concepts

Hybridization

Tetrahedral Geometry

Bond Angles

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