t Isotopes and Atomic Mass Most elements occur naturally as a mix of different i

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t Isotopes and Atomic Mass Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here Isotopic mass Relative abundance Isotope (amu 80.1 The atomic mass of boron is calculated as follows: (10.0 x 0.199) (11.0 x 0.801) 10.8 amu. Because the heavier isotope is more abundant, the atomic mass is closer to 11 amu than it is to 10 amu. Part A What is the atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotopic mass Relative abundance Isotope (amu) 79.9 2 83.9 10.2 87.9 78.4 Express your answer to three significant figures and include the appropriate units Value Units Submit Hints My Answers Give Up Review Part Part B What is the atomic mass of the element that consists of the following isotopes in the indicated natural abundances? Isotopic mass Relative abundance Isotope (amu 1 57.93 67.76 2 59.93 26.16 3 60.93 1.25 4 61.93 3.66 5 63.93 1.16

Explanation / Answer

Part (A) :

(79.9 x 0.114) + (83.9 x 0.102) + (87.9 x 0.784) = 86.58 amu

Part (B) :

(57.93x0.6776)+(59.93x0.2616)+(60.93x0.0125)+(61.93x0.0366)+(63.93x0.0116) = 58.7 amu

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