Chapter 8: Problem 55
Structure of \(\mathrm{H}_{2} \mathrm{O}_{2}\) is: (a) Planar (b) Linear (c) Non planar (d) Three dimensional
Short Answer
Expert verified
(c) Non planar
Step by step solution
01
Understanding the Problem
We need to determine the geometric structure of the hydrogen peroxide molecule, \(\mathrm{H}_2\mathrm{O}_2\). This involves understanding the shape and arrangement of its atoms in space.
02
Analyzing the Molecular Structure
The molecular formula \(\mathrm{H}_2\mathrm{O}_2\) indicates two hydrogen atoms and two oxygen atoms. The oxygen atoms form a single bond with each hydrogen and are linked by a peroxide bond (O-O).
03
Investigating Molecular Geometry
Hydrogen peroxide is known to have a skewed or "gauche" conformation as opposed to a flat or linear one due to the repulsion between lone pairs of oxygen atoms. The bond angles do not allow for a planar configuration, as there are torsional angles involved.
04
Conclusion of Analysis
The structure based on the VSEPR theory and experimental data suggests that the peroxide linkage and the bonds lead to a non-planar structure due to the repulsion between lone pairs and the geometry around the peroxide bond.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Hydrogen Peroxide Structure
Hydrogen peroxide, with the formula \(\mathrm{H}_2\mathrm{O}_2\), is an interesting molecule because of its structure. The molecule has two oxygen atoms and two hydrogen atoms. Each hydrogen is bonded to one of the oxygen atoms with a single bond. Moreover, the two oxygen atoms are connected by an O-O bond, called a peroxide bond.
This structure is not linear or flat, but rather it adopts a distinctive non-planar shape. Due to interactions and specific bond angles, the hydrogen peroxide molecule takes a twisted form. This non-planar configuration is often referred to as a "gauche" conformation.
Understanding this twisted shape is vital, as it significantly impacts the molecule's properties and reactivity. The molecule's ability to form a skewed structure is largely due to the dynamics of the bonds and electron pair repulsions, which we will explore next.
This structure is not linear or flat, but rather it adopts a distinctive non-planar shape. Due to interactions and specific bond angles, the hydrogen peroxide molecule takes a twisted form. This non-planar configuration is often referred to as a "gauche" conformation.
Understanding this twisted shape is vital, as it significantly impacts the molecule's properties and reactivity. The molecule's ability to form a skewed structure is largely due to the dynamics of the bonds and electron pair repulsions, which we will explore next.
VSEPR Theory
VSEPR Theory, which stands for Valence Shell Electron Pair Repulsion Theory, is a model used to predict the geometry of molecules. It's based on the premise that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion.
In the case of hydrogen peroxide, VSEPR Theory helps explain why the molecule is not planar. The oxygen atoms in \(\mathrm{H}_2\mathrm{O}_2\) each have lone pairs of electrons. These lone pairs exert repulsive forces on each other. To minimize these forces, the atoms are pushed into a non-linear arrangement.
This theory is pivotal for grasping why molecules like hydrogen peroxide have such specific shapes. The ideas of VSEPR allow chemists to predict and understand molecular geometry and the influence of electron pair repulsion on molecular structure.
In the case of hydrogen peroxide, VSEPR Theory helps explain why the molecule is not planar. The oxygen atoms in \(\mathrm{H}_2\mathrm{O}_2\) each have lone pairs of electrons. These lone pairs exert repulsive forces on each other. To minimize these forces, the atoms are pushed into a non-linear arrangement.
This theory is pivotal for grasping why molecules like hydrogen peroxide have such specific shapes. The ideas of VSEPR allow chemists to predict and understand molecular geometry and the influence of electron pair repulsion on molecular structure.
Molecular Geometry
Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. For hydrogen peroxide, its geometry is influenced by the presence of single bonds between hydrogen and oxygen, as well as the peroxide bond.
The non-planar structure of \(\mathrm{H}_2\mathrm{O}_2\) is influenced by steric effects and electronic interactions, which affect the overall shape. These effects cause the molecule to adopt a bent alignment, leading to what is often described as an angular or "gauche" configuration.
Understanding the molecular geometry is crucial because it helps in predicting the physical and chemical properties of compounds. The angles and distances between the atoms define how the molecule interacts with others and behaves in reactions, making molecular geometry an essential concept in chemistry.
The non-planar structure of \(\mathrm{H}_2\mathrm{O}_2\) is influenced by steric effects and electronic interactions, which affect the overall shape. These effects cause the molecule to adopt a bent alignment, leading to what is often described as an angular or "gauche" configuration.
Understanding the molecular geometry is crucial because it helps in predicting the physical and chemical properties of compounds. The angles and distances between the atoms define how the molecule interacts with others and behaves in reactions, making molecular geometry an essential concept in chemistry.
Lone Pair Repulsion
Lone pair repulsion plays a significant role in the shape of hydrogen peroxide. Lone pairs are pairs of valence electrons that are not shared with another atom and are found solely on an atom.
In \(\mathrm{H}_2\mathrm{O}_2\), each oxygen atom has lone pairs. These lone pairs repel each other strongly, more so than bonded pairs of electrons. This repulsion is responsible for the molecule adopting a bent or non-planar structure.
It's essential to recognize the impact of lone pair repulsion on a molecule's structure, as it is a common factor that influences the geometry of many molecular systems. When predicting molecular shapes, accounting for these repulsive forces is key to understanding why molecules adopt specific spatial arrangements.
In \(\mathrm{H}_2\mathrm{O}_2\), each oxygen atom has lone pairs. These lone pairs repel each other strongly, more so than bonded pairs of electrons. This repulsion is responsible for the molecule adopting a bent or non-planar structure.
It's essential to recognize the impact of lone pair repulsion on a molecule's structure, as it is a common factor that influences the geometry of many molecular systems. When predicting molecular shapes, accounting for these repulsive forces is key to understanding why molecules adopt specific spatial arrangements.
