Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 11: Problem 107

Construct a concept map that connects the ideas of molecular orbital theory.

Short Answer

Expert verified
The concept map starts with the central idea of 'Molecular Orbital Theory'. This branches out into 'Atomic Orbitals', 'Molecular Orbitals', 'Bonding', 'Anti-bonding'. 'Atomic Orbitals' further divide into 's orbital', 'p orbital' etc. 'Molecular Orbitals' further branch out into 'σ bonds' and 'π bonds'. 'Bonding' and 'Anti-bonding' are shown as forming through the overlap of Atomic Orbitals. Energy levels are shown in relation to 'Bonding' and 'Anti-bonding'.

Step by step solution

01

List key concepts

Start by listing the key concepts: Molecular Orbital Theory, Atomic Orbitals, Molecular Orbitals, Bonding, Anti-bonding, Sigma (σ) bonds, Pi (π) bonds.
02

Draw primary lines

Draw a line from the central concept 'Molecular Orbital Theory' to each related concept, like Atomic Orbitals, Molecular Orbitals, Bonding, Anti-bonding.
03

Add details

Under each of these branches, add the finer details. For instance, from 'Atomic Orbitals', add further lines branching to 's orbital', 'p orbital', etc. Similarly, from 'Molecular Orbitals', create further branches to 'σ bonds', 'π bonds'.
04

Illustrate Bonding and Anti-bonding

Elaborate on how 'Bonding' and 'Anti-bonding' form via overlap of Atomic Orbitals. Draw a line from 'Bonding' to 'Atomic Orbitals', and from 'Anti-bonding' to 'Atomic Orbitals'.
05

Indicate Energy Levels

Indicate energy levels for bonding and anti-bonding orbitals. Draw upwards and downwards pointing arrows from 'Bonding' and 'Anti-bonding' respectively.

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

Write Lewis structures for the following molecules, and then label each \(\sigma\) and \(\pi\) bond. (a) \(\mathrm{HCN} ;\) (b) \(\mathrm{C}_{2} \mathrm{N}_{2}\) (c) \(\mathrm{CH}_{3} \mathrm{CHCHCCl}_{3} ;\) (d) HONO.

The anion \(I_{4}^{2-}\) is linear, and the anion \(I_{5}^{-}\) is V-shaped, with a \(95^{\circ}\) angle between the two arms of the V. For the central atoms in these ions, propose hybridization schemes that are consistent with these observations.

Construct a molecular orbital diagram for \(\mathrm{HF}\), and label the molecular orbitals as bonding, antibonding, or nonbonding.

The paramagnetism of gaseous \(\mathrm{B}_{2}\) has been established. Explain how this observation confirms that the \(\pi_{2 p}\) orbitals are at a lower energy than the \(\sigma_{2 p}\) orbital for \(\mathrm{B}_{2}\)

The molecule formamide, \(\mathrm{HCONH}_{2}\), has the approximate bond angles \(\mathrm{H}-\mathrm{C}-\mathrm{O}, 123^{\circ} ; \mathrm{H}-\mathrm{C}-\mathrm{N}, 113^{\circ}\) \(\mathrm{N}-\mathrm{C}-\mathrm{O}, 124^{\circ} ; \mathrm{C}-\mathrm{N}-\mathrm{H}, 119^{\circ} ; \mathrm{H}-\mathrm{N}-\mathrm{H}, 119^{\circ}\) The \(\mathrm{C}-\mathrm{N}\) bond length is \(138 \mathrm{pm}\). Two Lewis structures can be written for this molecule, with the true structure being a resonance hybrid of the two. Propose a hybridization and bonding scheme for each structure.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

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