Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 24

Use valence bond theory to explain the bonding in \(\mathrm{Cl}_{2}\) and \(\mathrm{HCl}\). Show how the atomic orbitals overlap when a bond is formed

Short Answer

Expert verified
In Cl2, a covalent bond forms through the overlap of the half-filled 3p atomic orbitals of each Cl atom, which allows two unpaired electrons to pair up. In HCl, the bond forms when the half-filled 1s orbital of H overlaps with the half-filled 3p orbital of Cl, and their single electrons pair up.

Step by step solution

01

Understanding Valence Bond Theory

Valence Bond Theory (VBT) essentially posits that a covalent bond is formed between two atoms through the overlap of half-filled atomic orbitals. Each of these half-filled orbitals contains one unpaired electron. When overlapped, these two unpaired electrons can pair up and create a bond.
02

Bonding in Cl2

Chlorine (Cl) has 7 electrons in its outermost shell. For Cl2, two Cl atoms form a bond by overlapping their half-filled 3p atomic orbitals. This overlap allows the two unpaired electrons (one from each Cl) to pair up and form a covalent bond. This results in the Cl2 molecule being stable.
03

Bonding in HCl

In the case of HCl, Hydrogen (H) has one electron in its K shell, and Chlorine (Cl) has 7 electrons in its outermost shell, with one unpaired electron in the 3p orbital. The bond between H and Cl forms when the half-filled 1s orbital of H overlaps with the half-filled 3p orbital of Cl. The single electron from H and the unpaired electron from Cl then pair up within this overlapped region, forming a covalent bond.
04

Graphical Representation

To visually understand this, it can help to draw the atomic orbitals for each atom before the bond forms and then after the overlap occurs. For Cl2, two 3p orbitals (each with an unpaired electron) will overlap, while for HCl, the 1s orbital of H (with 1 electron) will overlap with the 3p orbital of Cl (with an unpaired electron).

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

The formation of \(\mathrm{H}^{+}\) from two \(\mathrm{H}\) atoms is an energetically favorable process. Yet statistically there is less than a 100 percent chance that any two \(\mathrm{H}\) atoms will undergo the reaction. Apart from energy considerations, how would you account for this observation based on the electron spins in the two \(\mathrm{H}\) atoms?

Specify which hybrid orbitals are used by carbon atoms in these species: (a) \(\mathrm{CO},\) (b) \(\mathrm{CO}_{2},\) (c) \(\mathrm{CN}^{-}\).

Predict the bond angles for these molecules: (a) \(\mathrm{BeCl}_{2},\) (b) \(\mathrm{BCl}_{3},\) (c) \(\mathrm{CCl}_{4},\) (d) \(\mathrm{CH}_{3} \mathrm{Cl}\) (e) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) (arrangement of atoms: \(\mathrm{ClHgHgCl}\) ), (f) \(\mathrm{SnCl}_{2}\) (g) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (h) \(\mathrm{SnH}_{4}\).

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line). What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

Consider the reaction $$ \mathrm{BF}_{3}+\mathrm{NH}_{3} \longrightarrow \mathrm{F}_{3} \mathrm{~B}-\mathrm{NH}_{3} $$ Describe the changes in hybridization (if any) of the \(B\) and \(N\) atoms as a result of this reaction
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

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