Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 8

Comment upon the statement: A fully filled orbital can participate in bonding.

Short Answer

Expert verified
Generally, fully filled orbitals do not participate in bonding as they are stable and cannot accept more electrons. However, under certain conditions like during the formation of coordination compounds, an electron can be excited to an unfilled orbital which can then engage in bonding.

Step by step solution

01

Understanding Orbitals

Orbitals are regions of space around a nucleus where electrons are most likely to be found. Each orbital can hold up to two electrons. Orbitals can be classified into s, p, d, and f types.
02

Concept of Fully Filled Orbitals

A fully filled orbital is one that contains the maximum number of electrons that it can hold. For example, a 2p orbital is fully filled when it contains six electrons.
03

Participation of Fully Filled Orbitals in Bonding

Typically, partially filled orbitals (those orbitals which are not completely filled) participate in bonding because they can accommodate more electrons. A completely filled orbital does not readily participate in bonding, because it is already stable and has no room to accept more electrons.
04

Exceptions to the Rule

However, under certain conditions, fully filled orbitals can participate in bonding. This usually happens when elements go through excitation, where an electron from a filled orbital is excited to an unfilled orbital. Then, this unfilled orbital can participate in bonding. An example of this is seen in the formation of coordination compounds.

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

Discuss the concept of resonance. Draw resonance structure for the following molecules or ions: (a) NO (b) \(\mathrm{CO}_{3}^{2-}\) (c) \(\mathrm{CO}\)

Compare the bond angles in the following molecules: (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{NH}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{O}\)

Differentiate between bonding and antibonding molecular orbitals.

A nonpolar molecule may have polar bonds. Justify the statement with the help of suitable example.

Differentiate between electrovalency and covalency with the help of suitable examples.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

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