Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 4

What trend in atomic radius is observed moving down a group in the periodic table? Explain why this trend exists.

Short Answer

Expert verified
Moving down a group in the periodic table, the atomic radius increases. This is due to the addition of electron shells which are significantly further away from the nucleus and exert more electron-electron repulsion, minimizing the effect of increased nuclear charge.

Step by step solution

01

Understanding Atomic Radius

The atomic radius refers to the size of an atom, generally measured from the centre of the nucleus to the boundary of the electron cloud. It varies in a predictable way across the periodic table.
02

Analyzing the Periodic Table Structure

The periodic table is structured into groups (vertical columns) and periods (horizontal rows). When you move down a group, you're essentially adding a layer of electrons around the nucleus.
03

Defining the Trend

As we go down the group in the periodic table, the atomic radius increases. This is because with each new period, an additional electron shell is added. Despite the increase in nuclear charge, each new level is significantly further away from the nucleus, and the additional electron-electron repulsion in this new shell outweighs the pull of the increased nuclear charge.

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

Why does the core charge increase moving from left to right across a period in the periodic table - for example, from boron to carbon to oxygen?

What trend in atomic radius is observed moving from left to right across a period? Explain why this trend exists.

What are three characteristics of an atom (or ion) that must be considered in determining its relative radius?

\(\mathrm{F}\) and \(\mathrm{F}^{-}\) have identical core charges and the valence shell is \(\mathrm{n}=2\) in both cases. Explain why the radius of \(\mathrm{F}^{-}\) is larger than the radius of \(\mathrm{F}\).

Provide a shell model diagram for \(\mathrm{K}^{+}\) showing all electrons explicitly and then show how the core charge for \(\mathrm{K}^{+}\) was calculated.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear 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