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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

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?

Write the atomic symbol \(\left(\frac{1}{2} X\right)\) for each of the isotopes described below. a. number of protons \(=27,\) number of neutrons \(=31\) b. the isotope of boron with mass number 10 c. \(Z=12, A=23\) d. atomic number \(53,\) number of neutrons \(=79\) e. \(Z=20,\) number of neutrons \(=27\) f. number of protons \(=29,\) mass number 65

In Section 1-1 of the text, the concept of a chemical reaction was introduced with the example of the decomposition of water, represented as follows: Use ideas from Dalton's atomic theory to explain how the above representation illustrates the law of conservation of mass.

The isotope of an unknown element, \(\mathrm{X},\) has a mass number of 79\. The most stable ion of this isotope has 36 electrons and has a \(2-\) charge. Which of the following statements is(are) true? For the false statements, correct them. a. This ion has more electrons than protons in the nucleus. b. The isotope of \(X\) contains 38 protons. c. The isotope of \(X\) contains 41 neutrons. d. The identity of \(\mathrm{X}\) is strontium, \(\mathrm{Sr}\).

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?
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