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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.

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Most popular questions from this chapter

Which (if any) of the following can be determined by knowing the number of protons in a neutral element? Explain your answer. a. the number of neutrons in the neutral element b. the number of electrons in the neutral element c. the name of the element

Write the atomic symbol \(\left(\frac{4}{2} X\right)\) for each of the following isotopes. a. \(Z=8,\) number of neutrons \(=9\) b. the isotope of chlorine in which \(A=37\) c. \(Z=27, A=60\) d. number of protons \(=26,\) number of neutrons \(=31\) e. the isotope of I with a mass number of 131 f. \(Z=3,\) number of neutrons \(=4\)

For lighter, stable isotopes, the ratio of the mass number to the atomic number is close to a certain value. What is the value? What happens to the value of the mass number to atomic number ratio as stable isotopes become heavier?

In a combustion reaction, \(46.0 \mathrm{g}\) of ethanol reacts with \(96.0 \mathrm{g}\) of oxygen to produce water and carbon dioxide. If \(54.0 \mathrm{g}\) of water is produced, what mass of carbon dioxide is produced?

When hydrogen is burned in oxygen to form water, the composition of water formed does not depend on the amount of oxygen reacted. Interpret this in terms of the law of definite proportion.
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