Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 7

The diameter of a neutral helium atom is about \(1 \times 10^{2} \mathrm{pm}\). Suppose that we could line up helium atoms side by side in contact with one another. Approximately how many atoms would it take to make the distance from end to end \(1 \mathrm{~cm} ?\)

Short Answer

Expert verified
Approximately \(10^{12}\) helium atoms would be needed to make up a distance of 1 cm when placed side by side in contact with each other.

Step by step solution

01

Convert the distance to same unit

The diameter of the helium atom is given in picometers (pm) while the desired total distance is given in centimeters (cm). To compare the two and establish how many atoms fit into the given distance, they need to be in the same units. Consider that \(1 \mathrm{m} = 10^{12} \mathrm{~pm}\) and \(1 \mathrm{m} = 10^{2} \mathrm{~cm}\), then convert 1 cm to picometers: \(1 \mathrm{~cm} = 1 \mathrm{~cm} \times \frac{10^{2} \mathrm{~m}}{1 \mathrm{~cm}} \times \frac{10^{12} \mathrm{~pm}}{1 \mathrm{~m}} = 10^{14} \mathrm{~pm}\)
02

Calculate number of atoms

Now, the total distance and the diameter of one atom are both in picometers. Divide the total distance by the diameter of one atom to find out how many atoms can fit into the distance: Number of atoms = Total distance (in pm) / Diameter of one atom (in pm) = \(10^{14} \mathrm{~pm} / (1 \times 10^{2} \mathrm{~pm}) = 10^{12}\)

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 do all atoms of an element have the same atomic number, although they may have different mass numbers? What do we call atoms of the same element with different mass numbers? Explain the meaning of each term in the symbol \({ }_{Z}^{A} \mathrm{X}\).

Describe the changes in properties (from metals to nonmetals or from nonmetals to metals) as we move (a) down a periodic group and (b) across the periodic table.

A monatomic ion has a charge of +2 . The nucleus of the parent atom has a mass number of \(55 .\) If the number of neutrons in the nucleus is 1.2 times that of the number of protons, what is the name and symbol of the element?

Give two examples of each of the following: (a) a diatomic molecule containing atoms of the same element, (b) a diatomic molecule containing atoms of different elements, (c) a polyatomic molecule containing atoms of the same element, (d) a polyatomic molecule containing atoms of different elements.

Give an example of a case in which two molecules have different molecular formulas but the same empirical formula.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Nuclear 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