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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

An element's most stable ion has a \(2+\) charge. If the ion of element \(\mathrm{X}\) has a mass number of 230 and has 86 electrons, what is the identity of the element, and how many neutrons does it have?

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What number of protons and neutrons is contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, what number of electrons is present? a. \(\frac{235}{92} \mathrm{U}\) b. \(_{13}^{2} \mathrm{Al}\) c. \(\frac{57}{26} \mathrm{Fe}\) d. \(\frac{208}{82} \mathrm{Pb}\) e. \(\frac{86}{32} \mathrm{Rb}\) f. \(\frac{41}{20} \mathrm{Ca}\)

You have two distinct gaseous compounds made from element \(\mathrm{X}\) and element Y. The mass percents are as follows: Compound I: \(30.43 \%\) X, \(69.57 \%\) Y Compound II: \(63.64 \% \mathrm{X}, 36.36 \% \mathrm{Y}\) In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas \(\mathrm{X}^{\prime \prime}+2\) volumes "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound I 2 volumes "gas \(\mathrm{X}^{\prime \prime}+1\) volume "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element \(X\) and element Y.
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