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Chapter 10: Problem 145

Use the \(\mathrm{NH}_{3}\) molecule as an example to explain the difference between molecular geometry and electron-group geometry.

Short Answer

Expert verified
The electron-group geometry of ammonia (\(NH_{3}\)) is tetrahedral as it accounts for all electron domains (three single bonds and one lone pair of electrons). However, the molecular geometry is trigonal pyramidal which includes only the positions of the nitrogen and hydrogen atoms and excludes non-bonding electrons.

Step by step solution

01

Representation of ammonia molecule

Start by representing the ammonia molecule as \(NH_{3}\). This consists of one Nitrogen (N) atom and three Hydrogen (H) atoms. Nitrogen in the middle forms three single bonds with three hydrogen atoms. Nitrogen also has one lone pair of electrons remaining.
02

Defining Electron-group geometry

For identifying the electron-group geometry, all electron domains (bonding and non-bonding) should be considered. In the ammonia molecule, there are 4 electron domains: 3 from the bond with Hydrogen atoms and 1 from the lone pair of electrons. According to VSEPR theory, this describes a tetrahedral electron-group geometry.
03

Defining Molecular geometry

When we look at the molecular geometry, we only consider the atoms themselves, not the non-bonding electron pairs. In the case of ammonia, when ignoring the lone pair, the shape formed by the nitrogen and hydrogen atoms is a trigonal pyramidal not tetrahedral.
04

Comparison between Electron-group and molecular geometries

With the information above, it's clear that the electron-group geometry (tetrahedral) involves all electron domains including bonding and non-bonding. However, the molecular geometry (trigonal pyramidal) only accounts for the positioning of atoms, excluding non-bonding electrons. So the main difference is whether or not non-bonding electrons are factored into the geometry.

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Most popular questions from this chapter

Draw Lewis structures for two different molecules with the formula \(\mathrm{C}_{3} \mathrm{H}_{4}\). Is either of these molecules linear? Explain.

In which of the following species is it necessary to employ an expanded valence shell to represent the Lewis structure: $\mathrm{PO}_{4}^{3-}, \mathrm{PI}_{3}, \mathrm{ICl}_{3}, \mathrm{OSCl}_{2}, \mathrm{SF}_{4}, \mathrm{ClO}_{4} ?$ Explain your choices.

Which of the following molecules would you expect to have a resultant dipole moment \((\mu) ;\) (a) \(\mathrm{F}_{2}\), (b) \(\mathrm{NO}_{2}\) (c) \(\mathrm{BF}_{3},\) (d) \(\mathrm{HBr},\) (e) \(\mathrm{H}_{2} \mathrm{CCl}_{2}\), (f) \(\mathrm{SiF}_{4},\) (g) OCS? Explain.

A \(0.325 \mathrm{g}\) sample of a gaseous hydrocarbon occupies a volume of \(193 \mathrm{mL}\) at \(749 \mathrm{mmHg}\) and \(26.1^{\circ} \mathrm{C}\). Determine the molecular mass, and write a plausible condensed structural formula for this hydrocarbon.

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.
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