9. naturally occurring isotopes as follows: On the planet Melmac, in a galaxy far, far away, argon has three Isotope Mass (amu) Natural Abundance (%) Argon-40 Argon-38 Argon-36 39.962 37.963 74.20 15.15 35.968 10.65 What is the relative atomic mass of argon on Melmac? What famous alien called the planet Melmac home?

9. naturally occurring isotopes as follows: On the planet Melmac, in a galaxy far, far away, argon has three Isotope Mass (amu) Natural Abundance (%) Argon-40 Argon-38 Argon-36 39.962 37.963 74.20 15.15 35.968 10.65 What is the relative atomic mass of argon on Melmac? What famous alien called the planet Melmac home?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 37E: An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with mass...

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An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with mass 205.9745 u, 22.10% of an isotope with mass 206.9759 u, and 52.40% of an isotope with mass 207.Y766 u. Calculate the average atomic mass, and identify the element.
How would you expect the chemical properties of isotopes of the same element to compare to each other? Explain your answer.
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.
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?
. The elements with atomic numbers of 93 or greater are referred to as the _________ elements.
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.
Bromine has two occuring isotopes: 79Br with atomic mass 78.9183 and 81Br with atomic mass 80.9163. Without using a calculator, what would you estimate the % abundance of Br-79 to be?
Naturally occurring silver (Ag) consists of two isotopes. One of the isotopes has a mass of 106.90509 amu and 51.84% abundance. What is the atomic mass of the other isotope?
A semiconducting material is composed of 52 g of Ga, 9.5 g of Al, and 112 g of As. Which element has the largest number of atoms in this material?
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution W the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?
Which of the following are isotopes of element X, the atomic number for which is 9: 919X, 920X, 189X, and 921X?