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Questions 31 through 36: Percentage abundances and atomic masses (u) of the natural
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Introductory Chemistry: An Active Learning Approach
- The natural abundances and isotopic masses of the element neon (Ne) are Calculate the atomic mass of naturally occurring neon.arrow_forwardWhich of the following are isotopes of element X, the atomic number for which is 9: 919X, 920X, 189X, and 921X?arrow_forwardQuestions 31 through 36: Percentage abundances and atomic masses (u) of the natural isotopes of an element are given. a Calculate the atomic mass of each element from these data. b Using other information that is available to you, identify the element. Percentage Abundance Atomic Mass (u) 69.09 62.9298 30.91 64.9278arrow_forward
- Argon has three naturally occurring isotopes: 0.3336% 36Ar, 0.063% 38Ar, and 99.60% 40Ar. Estimate the average atomic mass of argon. If the masses of the isotopes are 35.968 u, 37.963 u, and 39.962 u, respectively, calculate the average atomic mass of natural argon.arrow_forwardBromine 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?arrow_forwardDefine the term atomic weight. Why might the values of atomic weights on a planet elsewhere in the universe be different from those on earth?arrow_forward
- How do isotopes of a given element differ? How are they similar?arrow_forward2.90 Naturally occurring europium has an average atomic weight of 151.964 amu. If the only isotopes of europium present are 151Eu and 153Eu, describe how you would determine the relative abundance of the two isotopes. Include in your description any information that would need to be looked up.arrow_forward2.11 Define the term isotope.arrow_forward
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