Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 11: Problem 92

The bond angle in \(\mathrm{H}_{2} \mathrm{Se}\) is best described as (a) between \(109^{\circ}\) and \(120^{\circ} ;\) (b) less than in \(\mathrm{H}_{2} \mathrm{S} ;\) (c) less than in \(\mathrm{H}_{2} \mathrm{S},\) but not less than \(90^{\circ} ;(\mathrm{d})\) less than \(90^{\circ}\)

Short Answer

Expert verified
The bond angle in \(\mathrm{H}_{2} \mathrm{Se}\) is between \(109^{\circ}\) and \(120^{\circ}\), hence option (a) in the original problem is the most accurate

Step by step solution

01

Understand the Electron Pair Repulsion Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a simple, qualitative model that allows us to predict the geometry of polyatomic ions, molecules, and atoms based on the repulsion between electrons in the outer shell of atoms. It assumes that the molecule or ion will adopt a shape that minimizes the repulsion between electrons in the valence shell of that atom.
02

Identify the Molecular Structure of $\mathrm{H}_{2} \mathrm{Se}$ and $\mathrm{H}_{2}\mathrm{S}$

Both \(\mathrm{H}_{2} \mathrm{Se}\) and \(\mathrm{H}_{2}\mathrm{S}\) are nonpolar and fall under the AX2E (where A is the central atom, X is a terminal atom, and E stands for a lone pair of electrons on the central atom) category based on VSEPR theory. In these structures, the central atom (Se or S) is bonded to two hydrogen atoms and has two lone pairs of electrons.
03

Determine the Theoretical Bond Angle for AX2E Structures

In an AX2E structure, the ideal bond angle would be \(109.5^{\circ}\), but due to the presence of the lone pair electrons on the central atom, there is more repulsion between the lone pair and the bonding pairs. This causes the bonding pairs to squeeze together. As such, the bond angle is slightly less than \(109.5^{\circ}\). Therefore the bond angle in \(\mathrm{H}_{2} \mathrm{Se}\) and \(\mathrm{H}_{2}\mathrm{S}\) will be less than \(109.5^{\circ}\).
04

Compare the Bond Angles of $\mathrm{H}_{2} \mathrm{Se}$ and $\mathrm{H}_{2}\mathrm{S}$

H2Se has larger central atom (Se) than H2S (S), thus the size of S is smaller than that of Se which means Se has inner shells that shield the lone pairs more than the smaller S atom. Therefore the lone pair in Se is more diffuse. This makes the bond angle in H2Se larger than in H2S

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A conjugated hydrocarbon has an alternation of double and single bonds. Draw the molecular orbitals of the \(\pi\) system of 1,3,5 -hexatriene. If the energy required to excite an electron from the HOMO to the LUMO corresponds to a wavelength of \(256 \mathrm{nm},\) do you expect the wavelength for the corresponding excitation in 1,3,5,7 -octatetraene to be a longer or shorter wavelength?

From this list of terms-electrical conductor, insulator, semiconductor- -choose the one that best characterizes each of the following materials: (a) stainless steel; (b) solid sodium chloride; (c) sulfur; (d) germanium; (e) seawater; (f) solid iodine.

For each of the species \(\mathrm{C}_{2}^{+}, \mathrm{O}_{2}^{-}, \mathrm{F}_{2}^{+},\) and \(\mathrm{NO}^{+}\) (a) Write the molecular orbital diagram (as in Example \(11-6)\) (b) Determine the bond order, and state whether you expect the species to be stable or unstable. (c) Determine if the species is diamagnetic or paramagnetic; and if paramagnetic, indicate the number of unpaired electrons.

Explain why the electrical conductivity of a semiconductor is significantly increased if trace amounts of either donor or acceptor atoms are present, but is unchanged if both are present in equal number.

In which of the following ions would you expect to find delocalized molecular orbitals: (a) \(\mathrm{HCO}_{2}^{-} ;\) (b) \(\mathrm{CO}_{3}^{2-}\) (c) \(\mathrm{CH}_{3}^{+} ?\) Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free