# Review Constants Periodic Table Part A Atomic mass is a weighted average of the masses of...

###### Question:

Review Constants Periodic Table Part A Atomic mass is a weighted average of the masses of the naturally occurring isotopes of that element. For example, consider isotopes of lithium: Abundance Mass Isotope (%) (amu) Li 7.5 6.015 On a mission to a newly discovered planet, an astronaut finds copper abundances of 69.15 % for Cu and 30.85 % for 65Cu. What is the atomic mass of copper for this location? The mass of Cu is 62.9300 amu . The mass of 65Cu is 64.9200 amu. Express your answer to two decimal places, and include the appropriate units. View Available Hint(s) 7 Li 92.5 7.016 The atomic mass is therefore (0.075 x 6.015) + (0.925 x 7.016) = 6.94 amu Notice that the atomic mass is closer to 7 than it is to 6. That is because the heavier isotope is more abundant. HA ? Value Units Submit Part B The astronaut then measures the abundance of silicon on the new planet, obtaining the following results: Isotope Abundance Mass (%) (amu) 28 Si 73.71 27.98 29 Si 14.93 28.98 30 Si 11.36 29.97 What is the atomic mass of silicon for this planet? Express your answer to two decimal places, and include the appropriate units. View Available Hint(s) HA ?

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