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Chapter 10: Problem 1

How is the geometry of a molecule defined and why is the study of molecular geometry important?

Short Answer

Expert verified
Molecular geometry, approximately defined by the bonding and non-bonding electron pairs in the outer shell of the central atom, provides insight into the 3D arrangement of atoms in a molecule. Studying this is critical as the physical and chemical properties of a molecule—such as polarity, reactivity, phase of matter, color, magnetism, and biological activity—are largely determined by its geometry.

Step by step solution

01

Define Molecular Geometry

Molecular geometry pertains to the three-dimensional arrangement of atoms in a molecule. It can be defined by the positions of the nuclei and, more specifically, by the bonding and non-bonding electron pairs in the valence shell of the central atom.
02

Explain Influencing Factors

The geometry of a molecule is primarily influenced by the Valence Shell Electron Pair Repulsion (VSEPR) theory, which states that electron pairs arrange themselves around the central atom to minimize repulsion.
03

Describe Various Types of Molecular Geometry

There are several types of molecular geometries such as linear, bent, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral, among others. Each of these geometries is determined by the number of bonding and non-bonding electron pairs around the central atom.
04

Discuss Importance of Molecular Geometry

Studying molecular geometry is important because the spatial arrangement of a molecule can greatly impact its physical and chemical properties. This includes polarity, reactivity, phase of matter, color, magnetism, and biological activity. Therefore, understanding molecular geometry can provide valuable insight into how molecules interact with each other and their environments.

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Most popular questions from this chapter

Predict the geometry of the following molecules using the VSEPR method: (a) \(\mathrm{HgBr}_{2}\), (b) \(\mathrm{N}_{2} \mathrm{O}(\mathrm{ar}-\) rangement of atoms is \(\mathrm{NNO}\) ), (c) \(\mathrm{SCN}^{-}\) (arrangement of atoms is \(\mathrm{SCN}\) ).

In the trigonal bipyramidal arrangement, why does a lone pair occupy an equatorial position rather than an axial position?

Draw the Lewis structure of mercury(II) bromide. Is this molecule linear or bent? How would you establish its geometry?

Predict the geometry of the following molecules and ion using the VSEPR model: (a) \(\mathrm{CBr}_{4},\) (b) \(\mathrm{BCl}_{3}\) (c) \(\mathrm{NF}_{3}\), (d) \(\mathrm{H}_{2} \mathrm{Se},\) (e) \(\mathrm{NO}_{2}^{-}\).

Draw three Lewis structures for compounds with the formula \(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{~F}_{2} .\) Indicate which of the compound(s) are polar.
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