2. There are two isotopes of rubidium, as seen in the chart below, yet the atomic mass of rubidium on the periodic table is 85.47 g/mol. Explain why and show how this occurs. (2 marks) Isotope Exact Mass Percent Abundance Rb - 85 84.91 72.2 Rb - 87 86.91 27.8
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We have two isotopes of rubidium: Rb-85 with an exact mass of 84.91 g/mol and a percent abundance of 72.2%, and Rb-87 with an exact mass of 86.91 g/mol and a percent abundance of 27.8%. Show more…
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Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass $=84.9118$ amu; abundance $=72.15 \%$ ) and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85$\%$ ). Calculate the atomic weight of rubidium.
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Rubidium has two naturally occurring isotopes, Rb-85 with a mass of 84.91179 amu and Rb-87 with a mass of 86.90918 amu. Calculate the atomic weight of rubidium. Why do the two isotopes of rubidium have different masses?
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