/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 9 Dalton assumed that all atoms of... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 1: Problem 9

Dalton assumed that all atoms of the same element were identical in all their properties. Explain why this assumption is not valid.

Short Answer

Expert verified
Dalton's assumption that all atoms of the same element are identical in all their properties is not valid due to the existence of isotopes. Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons, resulting in different atomic masses. For example, carbon-12 and carbon-14 are isotopes of carbon with different atomic masses. The presence of isotopes with varying properties within the same element disproves Dalton's assumption and has significantly advanced our understanding of atomic structure, playing a crucial role in various applications such as nuclear energy, medicine, and radiocarbon dating.

Step by step solution

01

Introduce Dalton's Atomic Theory

Dalton's Atomic Theory states that all matter is composed of atoms, and these atoms can be distinguished by their properties. He also assumed that all atoms of a particular element were identical in all their properties, including their atomic weights.
02

Introduce isotopes

The term "isotope" refers to atoms of the same element that have the same number of protons but different numbers of neutrons. This causes the isotopes to have different atomic masses.
03

Provide examples of isotopes

Examples of isotopes include carbon-12 and carbon-14, which are both isotopes of carbon. Carbon-12 has six protons and six neutrons, while carbon-14 has six protons and eight neutrons.
04

Discuss how isotopes disprove Dalton's assumption

Since isotopes of the same element have different numbers of neutrons, they have different atomic masses. This means that their properties are not identical, disproving Dalton's assumption that all atoms of the same element are identical in all their properties.
05

Explain the importance of isotopes in the modern understanding of atomic structure

The discovery and study of isotopes have significantly advanced our understanding of atomic structure, as it has led to the development of more complex and accurate models of atomic behavior. Understanding isotopes is crucial for various applications, including nuclear energy, medicine, and dating ancient artifacts using radiocarbon dating.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

Reaction of \(2.0 \mathrm{L}\) of hydrogen gas with \(1.0 \mathrm{L}\) of oxygen gas yields 2.0 L of water vapor. All gases are at the same temperature and pressure. Show how these data support the idea that oxygen gas is a diatomic molecule. Must we consider hydrogen to be a diatomic molecule to explain these results?

This problem is designed to incorporate several concepts and techniques into one situation. You have gone back in time and are working with Dalton on a table of relative masses. Following are his data. \(0.602 \mathrm{g}\) gas A reacts with \(0.295 \mathrm{g}\) gas \(\mathrm{B}\) \(0.172 \mathrm{g}\) gas \(\mathrm{B}\) reacts with \(0.401 \mathrm{g}\) gas \(\mathrm{C}\) \(0.320 \mathrm{g}\) gas \(\mathrm{A}\) reacts with \(0.374 \mathrm{g}\) gas \(\mathrm{C}\) a. Assuming simplest formulas \((\mathrm{AB}, \mathrm{BC}, \text { and } \mathrm{AC}),\) construct a table of relative masses for Dalton. b. Knowing some history of chemistry, you tell Dalton that if he determines the volumes of the gases reacted at constant temperature and pressure, he need not assume simplest formulas. You collect the following data: 6 volumes gas \(A+1\) volume gas \(B \rightarrow 4\) volumes product 1 volume gas \(\mathrm{B}+4\) volumes gas \(\mathrm{C} \rightarrow 4\) volumes product 3 volumes gas \(A+2\) volumes gas \(C \rightarrow 6\) volumes product Write the simplest balanced equations, and find the actual relative masses of the elements. Explain your reasoning.

If the volume of a proton is similar to the volume of an electron, how will the densities of these two particles compare to each other?

A sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) contains \(2.02 \mathrm{g}\) of hydrogen, \(32.07 \mathrm{g}\) of sulfur, and \(64.00 \mathrm{g}\) of oxygen. How many grams of sulfur and grams of oxygen are present in a second sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) containing 7.27 g of hydrogen?

A combustion reaction involves the reaction of a substance with oxygen gas. The complete combustion of any hydrocarbon (binary compound of carbon and hydrogen) produces carbon dioxide and water as the only products. Octane is a hydrocarbon that is found in gasoline. Complete combustion of octane produces 8 liters of carbon dioxide for every 9 liters of water vapor (both measured at the same temperature and pressure). What is the ratio of carbon atoms to hydrogen atoms in a molecule of octane?
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

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.