None 18. A recently discovered element J has three naturally occurring isotopes with the following %abundances and masses:%abundance75.00%9.000%16.00%mass (amu)53.0054.0055.00Determine the average atomic mass of J.a. 53.41 amub. 54.00 amuc. 5,341 amud. 163.0 amu

Step 1:Find the average atomic mass of element J: To find the average atomic mass of element J, we…

Answered: 18. A recently discovered element J has…

Chemistry

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Chapter3: Stoichiometry

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Problem 42E: The element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of...

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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.
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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These questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.
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Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible.
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18. A recently discovered element J has three naturally occurring isotopes with the following %abundances and masses: %abundance 75.00% 9.000% 16.00% mass (amu) 53.00 54.00 55.00 Determine the average atomic mass of J. a. 53.41 amu b. 54.00 amu c. 5,341 amu d. 163.0 amu