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Chapter 2: Problem 98

Which of the following statements is(are) true? For the false statements, correct them. a. All particles in the nucleus of an atom are charged. b. The atom is best described as a uniform sphere of matter in which electrons are embedded. c. The mass of the nucleus is only a very small fraction of the mass of the entire atom. d. The volume of the nucleus is only a very small fraction of the total volume of the atom. e. The number of neutrons in a neutral atom must equal the number of electrons.

Short Answer

Expert verified
a. False. Corrected statement: "Protons in the nucleus of an atom are positively charged, and neutrons are uncharged particles." b. False. Corrected statement: "The atom is best described as electrons orbiting around a dense, positively charged nucleus." c. False. Corrected statement: "The mass of the nucleus accounts for almost the entire mass of the atom." d. True. No correction needed. e. False. Corrected statement: "The number of protons in a neutral atom must equal the number of electrons."

Step by step solution

01

Determine the charge status of particles in the nucleus

The nucleus of an atom contains protons, which have a positive charge and neutrons, which are uncharged particles. Since neutrons are not charged, this statement is false. The corrected statement is: "Protons in the nucleus of an atom are positively charged, and neutrons are uncharged particles." #b. The atom is best described as a uniform sphere of matter in which electrons are embedded.#
02

Describe the structure of an atom

This statement refers to the "plum pudding" model of an atom, which has been debunked. The correct model is the Rutherford's "nuclear" model, in which electrons orbit around a dense, positively charged nucleus. Thus, the statement is false. The corrected statement is: "The atom is best described as electrons orbiting around a dense, positively charged nucleus." #c. The mass of the nucleus is only a very small fraction of the mass of the entire atom.#
03

Compare the mass of the nucleus to the mass of the atom

This statement is false. In reality, the mass of the nucleus is almost equal to the mass of the entire atom, since both protons and neutrons, which are located in the nucleus, have much larger masses compared to the electrons that orbit the nucleus. The corrected statement is: "The mass of the nucleus accounts for almost the entire mass of the atom." #d. The volume of the nucleus is only a very small fraction of the total volume of the atom.#
04

Compare the volume of the nucleus to the volume of the atom

This statement is true. The nucleus occupies a very tiny space compared to the overall volume of the atom. The vast majority of the atom's volume is occupied by the electron cloud, where the electrons orbit the nucleus. No correction is needed for this statement. #e. The number of neutrons in a neutral atom must equal the number of electrons.#
05

Compare the number of neutrons to the number of electrons in a neutral atom

This statement is false. In a neutral atom, the number of electrons equals the number of protons, as their charges balance each other out. The number of neutrons does not have to be equal to the number of electrons. The corrected statement is: "The number of protons in a neutral atom must equal the number of electrons."

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Most popular questions from this chapter

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

A single molecule has a mass of \(7.31 \times 10^{-23}\) g. Provide an example of a real molecule that can have this mass. Assume the elements that make up the molecule are made of light isotopes where the number of protons equals the number of neutrons in the nucleus of each element.

Section 2.3 describes the postulates of Dalton’s atomic theory. With some modifications, these postulates hold up very well regarding how we view elements, compounds, and chemical reactions today. Answer the following questions concerning Dalton’s atomic theory and the modifications made today. a. The atom can be broken down into smaller parts. What are the smaller parts? b. How are atoms of hydrogen identical to each other, and how can they be different from each other? c. How are atoms of hydrogen different from atoms of helium? How can H atoms be similar to He atoms? d. How is water different from hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$even though both compounds are composed of only hydrogen and oxygen? e. What happens in a chemical reaction, and why is mass conserved in a chemical reaction?

What number of protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, what number of electrons are present? a. \(^{235}_{92} \mathrm{U}\) b. \(_{13}^{27} \mathrm{Al}\) c. \(_{26}^{57} \mathrm{Fe}\) d. \(_{82}^{208} \mathrm{Pb}\) e. \(_{37}^{86} \mathrm{Rb}\) f. \(_{20}^{41} \mathrm{Ca}\)

Why is the term “sodium chloride molecule” incorrect whereas the term “carbon dioxide molecule” is correct?
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