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Chapter 1: Problem 8

One of the best indications of a useful theory is that it raises more questions for further experimentation than it originally answered. Does this apply to Dalton's atomic theory? Give examples.

Short Answer

Expert verified
Yes, Dalton's atomic theory raises more questions for further experimentation than it originally answered. While it initially explained elemental combinations and conservation of mass, it also prompted new questions regarding atomic structure, isotopes, chemical bonds, and properties of different elements. These questions led to advancements in modern atomic theory, subatomic particles, chemical bonds, and the periodic table.

Step by step solution

01

Dalton's atomic theory consists of five main postulates: 1. Elements consist of tiny particles called atoms. 2. The atoms of a given element are identical in size, mass, and properties, while atoms of different elements have different properties. 3. Atoms cannot be created, divided, or destroyed during a chemical reaction. 4. Atoms combine in whole number ratios to form compounds. 5. In chemical reactions, atoms are rearranged, combined, or separated, but not created or destroyed. Now, let's analyze whether this theory raises more questions for further experimentation than it originally answered, providing examples. #Step 2: Initial questions answered by Dalton's Atomic Theory#

The main questions that Dalton's atomic theory originally answered were: 1. Why do elements combine in whole number ratios to form compounds? 2. How can we explain the conservation of mass in chemical reactions? These questions were fundamental during the time when the theory was developed (early 19th century) and helped scientists improve their understanding of chemical reactions and compounds. #Step 3: New questions and limitations raised from the theory#
02

While Dalton's atomic theory was groundbreaking at its time, it also raised many new questions and highlighted some limitations that led to further experimentation and development. Some of these include: 1. What is the internal structure of atoms? Dalton's theory does not explain the existence of subatomic particles like electrons, protons, and neutrons. 2. How can we explain the behavior of isotopes? Isotopes, having different masses, contradict the second postulate of Dalton's theory. 3. How do atoms combine? The theory does not provide an explanation of the nature of chemical bonds or how they form between atoms. 4. Why do atoms of different elements have different properties? This question led scientists to investigate and discover the periodic table and quantum mechanics. #Step 4: Conclusion on the usefulness of Dalton's Atomic Theory#

Considering the questions raised and the limitations highlighted in Dalton's atomic theory, it can be said that the theory has been useful in furthering experimentation and development in the field of chemistry. It paved the way for the development of modern atomic theory, which now incorporates the understanding of subatomic particles, isotopes, chemical bonds, and periodicity of elements. Although the theory has its limitations, it provided a solid foundation for the advancement of science and our comprehension of atomic structure.

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Most popular questions from this chapter

A sample of chloroform is found to contain \(12.0 \mathrm{g}\) of carbon, \(106.4 \mathrm{g}\) of chlorine, and \(1.01 \mathrm{g}\) of hydrogen. If a second sample of chloroform is found to contain \(30.0 \mathrm{g}\) of carbon, what is the total mass of chloroform in the second sample?

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?

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

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?

Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen that combines with \(1.00 \mathrm{g}\) of nitrogen for each compound is \(1.44 \times 10^{-1} \mathrm{g}\) \(2.16 \times 10^{-1} \mathrm{g},\) and \(2.40 \times 10^{-2} \mathrm{g},\) respectively. Show how these data illustrate the law of multiple proportions.
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