BIO206H5 Study Guide - Final Guide: Unified Atomic Mass Unit
Document Summary
Chm140 notes: there are two naturally occurring isotopes of nitrogen; n-14 (14. 003 amu) and n-15 (15. 000 amu). What can we tell about the relative abundances of the atoms from this information (without doing any calculations): there are two naturally occurring isotopes of carbon; c-12 (12. 000 amu) and c-13 (13. 003 amu). The abundance of c-12 is 98. 9% while the abundance of c-13 is 1. 1%. Explain your reasoning: a student used a chunk of copper to determine the average atomic mass of copper. The student then made the statement this means that every copper atom weighs exactly 63. 546 amu! explain whether or not you agree with this statement and why. Calculations: there are four naturally occurring isotopes of chromium; cr-50 (49. 9460 amu), cr-52 (51. 9405 amu), cr-53 (52. 9407 amu), and cr-54 (53. 9389 amu). What is the average atomic mass of chromium if the isotopic abundances are 4. 345%, 83. 789%,
