Chapter 9: Problem 27
What is the angle between the following two hybrid orbitals on the same atom: (a) \(s p\) and \(s p\) hybrid orbitals, (c) \(s p^{3}\) and \(s p^{3}\) hybrid (b) \(s p^{2}\) and \(s p^{2}\) hybrid orbitals, orbitals?
Short Answer
Expert verified
(a) 180°, (b) 120°, (c) 109.5°.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
molecular geometry
Molecular geometry is a fundamental aspect of chemistry that describes the three-dimensional arrangement of atoms within a molecule. This arrangement is not random but is dictated by the types of bonds and interactions between atoms. Understanding molecular geometry helps predict molecule behavior and reactivity. It's like the blueprint of a molecule, influencing properties such as boiling and melting points.
To grasp this concept, you must be familiar with terms like bond angles, which are specific angles between bonds on a single atom. These bond angles are crucial because they determine the molecule's shape and therefore its function. For example, different shapes like linear, tetrahedral, and trigonal planar are results of different hybridizations. This orientation is then key to understanding how molecules interact in chemical reactions.
In essence, molecular geometry sets the stage for everything that happens in a molecule. It's what makes a molecule flexible or rigid, reactive or stable.
To grasp this concept, you must be familiar with terms like bond angles, which are specific angles between bonds on a single atom. These bond angles are crucial because they determine the molecule's shape and therefore its function. For example, different shapes like linear, tetrahedral, and trigonal planar are results of different hybridizations. This orientation is then key to understanding how molecules interact in chemical reactions.
In essence, molecular geometry sets the stage for everything that happens in a molecule. It's what makes a molecule flexible or rigid, reactive or stable.
linear configuration
A linear configuration is one of the simplest molecular shapes possible. It occurs when three atoms are in a straight line. This configuration is common in molecules containing sp hybridized atoms, where a central atom forms two bonds.
In a linear shape, the bond angle is perfectly 180 degrees. This wide angle allows for separation of electron clouds, minimizing electron pair repulsion which is crucial in VSEPR theory (Valence Shell Electron Pair Repulsion theory).
Examples of molecules with such configuration include carbon dioxide (CO_2) and acetylene (C_2H_2). In both cases, the molecules exhibit straight-line geometry due to these bond angles, allowing them to interact distinctively with other molecules in their environment.
In a linear shape, the bond angle is perfectly 180 degrees. This wide angle allows for separation of electron clouds, minimizing electron pair repulsion which is crucial in VSEPR theory (Valence Shell Electron Pair Repulsion theory).
Examples of molecules with such configuration include carbon dioxide (CO_2) and acetylene (C_2H_2). In both cases, the molecules exhibit straight-line geometry due to these bond angles, allowing them to interact distinctively with other molecules in their environment.
tetrahedral shape
The tetrahedral shape is a classic molecular geometry that occurs when a central atom forms four bonds directed towards the corners of a tetrahedron. This results in a bond angle of approximately 109.5 degrees, which is observed in sp3 hybridization.
In tetrahedral geometry, the central atom's bonds are equidistant, providing optimal spacing to minimize repulsions between electron pairs—a key point of VSEPR theory. A common example of a molecule with tetrahedral geometry is methane (CH_4), where the carbon atom is at the center with hydrogen atoms at the vertices of the tetrahedron.
This shape is not only common but also significant in determining the properties and reactivity of various organic and inorganic compounds. It explains why molecules like methane are stable and how they interact during chemical reactions.
In tetrahedral geometry, the central atom's bonds are equidistant, providing optimal spacing to minimize repulsions between electron pairs—a key point of VSEPR theory. A common example of a molecule with tetrahedral geometry is methane (CH_4), where the carbon atom is at the center with hydrogen atoms at the vertices of the tetrahedron.
This shape is not only common but also significant in determining the properties and reactivity of various organic and inorganic compounds. It explains why molecules like methane are stable and how they interact during chemical reactions.
sp hybridization
SP hybridization is a type of atomic orbital hybridization used to describe the bonding in molecules with linear geometry. When an s orbital merges with a p orbital, two equivalent sp hybrid orbitals form.
This hybridization results in two orbits oriented at 180 degrees, reflecting a linear configuration. Such arrangements are typical in molecules such as acetylene (C_2H_2), where the carbon atoms are sp hybridized, forming triple bonds with each other and linear bonds with hydrogen atoms.
Understanding sp hybridization is crucial for grasping how pi bonds and sigma bonds form and maintain molecular stability. This knowledge helps predict molecular shapes and answer questions about molecular orientation in complex structures.
This hybridization results in two orbits oriented at 180 degrees, reflecting a linear configuration. Such arrangements are typical in molecules such as acetylene (C_2H_2), where the carbon atoms are sp hybridized, forming triple bonds with each other and linear bonds with hydrogen atoms.
Understanding sp hybridization is crucial for grasping how pi bonds and sigma bonds form and maintain molecular stability. This knowledge helps predict molecular shapes and answer questions about molecular orientation in complex structures.
sp2 hybridization
SP2 hybridization occurs when one s orbital and two p orbitals on the same atom combine, forming three sp2 hybrid orbitals. These hybrid orbitals are oriented in a trigonal planar structure, with bond angles of 120 degrees.
This type of hybridization is common in molecules where central atoms form double bonds, such as ethylene (C_2H_4). Here, the carbon atoms are sp2 hybridized, allowing for planar geometry and maintaining stability through the formation of pi bonds.
SP2 hybridization plays a crucial role in organic chemistry, determining how molecules stack, react, and seasonally interact. It informs molecular geometry predictions, particularly in understanding flat molecules like benzene and its derivatives, which contributes to their characteristic stability and reactivity.
This type of hybridization is common in molecules where central atoms form double bonds, such as ethylene (C_2H_4). Here, the carbon atoms are sp2 hybridized, allowing for planar geometry and maintaining stability through the formation of pi bonds.
SP2 hybridization plays a crucial role in organic chemistry, determining how molecules stack, react, and seasonally interact. It informs molecular geometry predictions, particularly in understanding flat molecules like benzene and its derivatives, which contributes to their characteristic stability and reactivity.
