1. Element X has 3 isotopes with masses of 15.990 amu (abundance 99.0%), 14.00 amu (abundance (0.500%) and 17.564 amu (0.500 %). a. Without doing any math, based on the percent abundance values, predict the average isotopic mass. Justify your answer. b. Calculate the average isotopic mass of Element X. SHOW SET UP c. Using your answer from part b), identify Element X from the periodic table: d. How many protons and neutrons are there in the nucleus of the most abundant species of X? How many protons and neutrons are possible for an isotope of X?

1. Element X has 3 isotopes with masses of 15.990 amu (abundance 99.0%), 14.00 amu (abundance (0.500%) and 17.564 amu (0.500 %). a. Without doing any math, based on the percent abundance values, predict the average isotopic mass. Justify your answer. b. Calculate the average isotopic mass of Element X. SHOW SET UP c. Using your answer from part b), identify Element X from the periodic table: d. How many protons and neutrons are there in the nucleus of the most abundant species of X? How many protons and neutrons are possible for an isotope of X?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter2: Atoms, Molecules, And Ions

Section: Chapter Questions

Problem 23E: Average atomic masses listed by JUPAC are based on a study of experimental results. Bromine has two...

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An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.
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How would you expect the chemical properties of isotopes of the same element to compare to each other? Explain your answer.
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Neon is an inert gas with three stable isotopes. It is used in gas lasers and in advertising signs. Its isotopes and their abundances are: Ne-20 19.9924 amu 90.51% Ne-21 20.9938 amu 0.27% Ne-22 21.9914 amu 9.22% What is the average atomic mass of neon?
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The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
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Average atomic masses listed by JUPAC are based on a study of experimental results. Bromine has two isotopes 79Br and 81Br, whose masses (78.9 183 and 80.9 163 amu) and abundances (50.69% and 49.3 1%) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.