Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 118

Compare the atomic size of the following two magnesium isotopes: \({ }^{24} \mathrm{Mg}\) and \({ }^{26} \mathrm{Mg}\).

Short Answer

Expert verified
The atomic sizes of \(^{24}\mathrm{Mg}\) and \(^{26}\mathrm{Mg}\) are essentially the same because the atomic size is determined by the number of electron shells, not the number of neutrons. Both have the same number of electron shells, hence the same atomic size.

Step by step solution

01

Identify the Isotopes

Firstly, the two atoms to be compared are identified as different isotopes of magnesium: \(^{24}\mathrm{Mg}\) and \(^{26}\mathrm{Mg}\). They are isotopes because they have the same number of protons (which is the atomic number) but different number of neutrons.
02

Revisit the Atomic Structure

It's necessary to recall the basic atomic structure. The atomic size, or atomic radius, is determined by the area that surrounds the nucleus where there is a high probability of finding an electron. The number of electron shells primarily determine this, which are decided by the atomic number (number of protons).
03

Determine Atomic Size

Considering that the atomic number of magnesium is 12, both \(^{24}\mathrm{Mg}\) and \(^{26}\mathrm{Mg}\) have 12 protons and 12 electrons. As a result, they both have the same number of electron shells. The atomic size is mainly determined by the number of electron shells, not the number of neutrons.
04

Compare Atomic Sizes

Since \(^{24}\mathrm{Mg}\) and \(^{26}\mathrm{Mg}\) both have the same number of electron shells, they have essentially the same atomic size. The number of neutrons doesn't affect the atomic size, so the additional neutrons in \(^{26}\mathrm{Mg}\) do not make it larger than \(^{24}\mathrm{Mg}\).

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

Define the following terms: (a) \(\alpha\) particle, (b) \(\beta\) particle, (c) \(\gamma\) ray, (d) X ray.

Pair the following species that contain the same number of electrons: \(\mathrm{Ar}, \mathrm{Sn}^{4+}, \mathrm{F}^{-}, \mathrm{Fe}^{3+}, \mathrm{P}^{3-}, \mathrm{V}, \mathrm{Ag}^{+}, \mathrm{N}^{3-}\)

What do we call atoms of the same elements with different mass numbers?

Predict the formula and name of a binary compound formed from the following elements: (a) \(\mathrm{Na}\) and \(\mathrm{H},\) (b) \(\mathrm{B}\) and \(\mathrm{O},\) (c) \(\mathrm{Na}\) and \(\mathrm{S},\) (d) \(\mathrm{Al}\) and \(\mathrm{F},(\mathrm{e}) \mathrm{F}\) and \(\mathrm{O},\) (f) \(\mathrm{Sr}\) and \(\mathrm{Cl}\).

Define the following terms: acids, bases, oxoacids, oxoanions, and hydrates.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic 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