Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Chapter 1, Problem 22P
The last “missing” element from the first six periods was promethium, which was finally discovered in 1947 among the fission products of uranium. Determine (a) the ratio of the number of neutrons in a 145Pm nucleus to the number of protons, and (b) the number of electrons in a single promethium atom.
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Chapter 1 Solutions
Principles of Modern Chemistry
Ch. 1 - Classify the following materials as substances or...Ch. 1 - Classify the following materials as substances or...Ch. 1 - A 17th-century chemist wrote of the “simple bodies...Ch. 1 - Since 1800, almost 200 sincere but erroneous...Ch. 1 - A sample of ascorbic acid (vitamin C) is...Ch. 1 - A sample of a compound synthesized and purified in...Ch. 1 - Nitrogen (N) and silicon (Si) form two binary...Ch. 1 - Iodine (I) and fluorine (F) form a series of...Ch. 1 - Vanadium (V) and oxygen (O) form a series of...Ch. 1 - Prob. 10P
Ch. 1 - Prob. 11PCh. 1 - Prob. 12PCh. 1 - Pure nitrogen dioxide (NO2) forms when dinitrogen...Ch. 1 - Gaseous methanol (CH3OH) reacts with oxygen (O2)...Ch. 1 - In J. J. Thompson’s experiment depicted in Figures...Ch. 1 - In the problem 15 above, what is vy , the...Ch. 1 - The natural abundances and isotopic masses of the...Ch. 1 - The natural abundances and isotopic masses of the...Ch. 1 - Prob. 19PCh. 1 - More than half of all the atoms in naturally...Ch. 1 - The isotope of plutonium used for nuclear fission...Ch. 1 - The last “missing” element from the first six...Ch. 1 - Prob. 23PCh. 1 - In 1982, the production of a single atom of...Ch. 1 - Prob. 25PCh. 1 - Prob. 26PCh. 1 - Compute the relative molecular masses of the...Ch. 1 - Prob. 28PCh. 1 - Suppose that a person counts out gold atoms at the...Ch. 1 - A gold atom has a diameter of 2.881010m . Suppose...Ch. 1 - The vitamin A molecule has the formula C20H30O ,...Ch. 1 - Arrange the following in order of increasing mass:...Ch. 1 - Mercury is traded by the “flask,” a unit that has...Ch. 1 - Gold costs $400 per troy ounce, and...Ch. 1 - Aluminum oxide (Al2O3) occurs in nature as a...Ch. 1 - Prob. 36PCh. 1 - Soft wood chips weighing 17.2 kg are placed in an...Ch. 1 - In a reproduction of the Millikan oil-drop...Ch. 1 - A rough estimate of the radius of a nucleus is...Ch. 1 - In a neutron star, gravity causes the electrons to...Ch. 1 - Prob. 41APCh. 1 - Naturally occurring rubidium (Rb) consists of two...Ch. 1 - A sample of a gaseous binary compound of boron and...
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- 2.10 Which isotope in each pair contains more neutrons? (A) 35Cl or 33S, (b) 19F or 19Ne, (c) 63Cu or 65Zn, (d) 126I or 127Tearrow_forwardThough the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of 24, 25, 26, 28, 29, and 30. How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.arrow_forward2-31 Tin-118 is one of the isotopes of tin. Name the isotopes of tin that contain two, three, and six more neutrons than tin-118.arrow_forward
- 2.86 For some uses, the relative abundance of isotopes must be manipulated. For example, a medical technique called boron neutron capture therapy needs a higher fraction of 10B than occurs naturally to achieve its best efficiency. What would happen to the atomic weight of a sample of boron that had been enriched in 10B? Explain your answer in terms of the concept of a weighted average.arrow_forwardIn what way are isotopes of a given element always different? In what way(s) are they always the same?arrow_forward2-27 If each atom in Problem 2-26 acquired two more neutrons, what element would each then be?arrow_forward
- 2.19 Naturally occurring uranium consists of two isotopes, whose masses and abundances are shown below: Only 235U can be used as fuel in a nuclear reactor, so uramium for use in the nuclear industry must be enriched in this isotope. If a sample of enriched uranium has an atomic weight of 235.684 amu, what percentage of 235LT is present?arrow_forwardWhy do we not necessarily expect the number of neutrons in the nucleus of an atom to be the same as the number of protons?arrow_forward2-85 The mass of a proton is 1.67 × 10-24g. The mass of a grain of salt is 1.0 × 10-2g. How many protons would it take to have the same mass as a grain of salt?arrow_forward
- 2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?arrow_forwardFill in the following table:arrow_forwardWhat is the charge of the nucleus of element 89?arrow_forward
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