We must first calculate the mass defect (Am) for 56Fe. Since atomic masses (which include the electrons) are given, we must decide how to account for the electron mass: 55.9349 = mass of 56 Fe atom = mass of nucleus + 26 m. 1.0078 = mass of H atom = mass of nucleus + m, Thus, since a 56Fe nucleus is "synthesized" from 26 protons and 30 neutrons, we see that Am = (55.9349 - 26 m.) - [26(1.0078 - ma) + 30(1.0087)]. Solve for Am. Am = 0.5289 amu
We must first calculate the mass defect (Am) for 56Fe. Since atomic masses (which include the electrons) are given, we must decide how to account for the electron mass: 55.9349 = mass of 56 Fe atom = mass of nucleus + 26 m. 1.0078 = mass of H atom = mass of nucleus + m, Thus, since a 56Fe nucleus is "synthesized" from 26 protons and 30 neutrons, we see that Am = (55.9349 - 26 m.) - [26(1.0078 - ma) + 30(1.0087)]. Solve for Am. Am = 0.5289 amu
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter2: Atoms, Molecules, And Ions
Section: Chapter Questions
Problem 27Q
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