Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 2

Describe what all isotopes of magnesium have in common and also how are they different.

Short Answer

Expert verified
All isotopes of magnesium have the same atomic number, which is 12, meaning they all have 12 protons. The isotopes of magnesium differ in their number of neutrons, thereby differing in their atomic masses. The three naturally occurring isotopes of magnesium are Magnesium-24, Magnesium-25, and Magnesium-26, with 12, 13, and 14 neutrons, respectively.

Step by step solution

01

Understand What Isotopes Are

Isotopes are variations of the same element that have the same number of protons, but a different number of neutrons. This results in isotopes having the same atomic number but different atomic masses.
02

Identify the Common Traits of Magnesium Isotopes

All isotopes of magnesium have the same atomic number, which is 12. This means they all have 12 protons in their atomic nuclei, which is the defining characteristic of the element magnesium.
03

Discern the Differences between Magnesium Isotopes

The difference among the isotopes of magnesium lies in the number of neutrons in the nucleus. For instance, the three naturally occurring isotopes of magnesium are Magnesium-24, Magnesium-25, and Magnesium-26, which have 12, 13, and 14 neutrons respectively. So, although they all are magnesium, they have different atomic masses.

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

What is the mass (in amu) of a) \(100^{12} \mathrm{C}\) atoms? b) \(100^{13} \mathrm{C}\) atoms?

Which has more atoms: \(1.008 \mathrm{~g}\) of hydrogen or \(39.95 \mathrm{~g}\) of argon? Explain your reasoning.

Give two interpretations of the number "12.011" found below the symbol for carbon on the periodic table.

Without using a calculator, a) Which weighs more, 18 elephants or two dozen elephants? b) Which weighs more, \(5.136 \times 10^{23}\) sodium atoms or one mole of sodium atoms?

For any large collection of (randomly selected) chlorine atoms: a) What is the average atomic mass of chlorine in amu? b) What is the average mass of a chlorine atom in grams?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

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