Read-To find the average atomic mass of neon, we will use the equation above and take the abundance of the first isotope times the mass of the first isotope plus the abundance of the second isotope times the mass of the second isotope plus the abundance of the third isotope times the mass of the third isotope. The equation would then look like: = (0.9048x19.9924)+(0.0027x20.9938 amu) + (0.0925x21.9914 amu)=18.089 amu +0.0516 amu +2.034 amu=20.18 amu. This is the average atomic mass of neon. Answer the questionsWhat is an isotope?What is meant by the phrase “percent abundance in nature”?Explain the difference between average and a weighted average.Highlight evidence if you can and site which paragraph and line you found the evidence. Breath in... Breath out: Again! When you inhale air, you are not just inhaling a mixture of oxygen,nitrogen, and trace gasses, but a mixture of different oxygen atoms and different nitrogen atoms. It turnsout that all oxygen atoms have the same number of protons, but some may have different numbers ofneutrons. These different-but-still-oxygen atoms are called isotopes. Some atoms have just twoisotopes; some have dozens!The average atomic mass is an experimental number determined from all of the naturally occurringisotopes of an element. Not all atoms of an element are identical. For example, chlorine has two differentisotopes that occur in nature; chlorine-35 and chlorine-37. When you look at chlorine on the PeriodicTable it has an average atomic mass of 35.45 amu. This number is the weighted average of the massesof both isotopes, not just one of them.Notice that the units were listed as amu, which stands for atomic mass units. This unit is based off themass of the isotope 12C (carbon-12). Carbon-12 was chosen as the basis for all of the masses on theperiodic table and has been defined to be exactly 12 amu. So all of the other masses on the period tableare relative to the mass of carbon-12. In that case, then why is the atomic mass of carbon on the periodictable not exactly 12 amu? Because not all carbon in nature is 12C! Most of 12C, some of it is 13C, anda very tiny amount is 14C. When these are averaged together you get the a ge atomic mass shown onthe periodic table of 12.01 amu.Since the abundances are not equal, we cannot do a typical simple average where we just add them upand divide by two. Instead, we need to perform a weighted average. The formula to calculate theaverage atomic mass is: Since the abundances are not equal, we cannot do a typical simple average where we just add them upand divide by two. Instead, we need to perform a weighted average. The formula to calculate theaverage atomic mass is:average atomic mass = [(relative abundance x mass of isotope)Remember that is the symbol for sum. In other words, we will take the sum of the relative abundanceof each isotope multiplied by its mass.ExampleNeon has three naturally occurring isotopes.SymbolNe-20Ne-21Ne-22Mass Isotopic mass Percent naturalnumber(amu)abundance20212219.992420.993821.991490.48%0.27%9.25%…..Remember that mass number is not the same as the atomic mass or isotopic mass! The mass number isthe number of protons + neutrons, while atomic mass (or isotopic mass) is the mass if you were tosomehow weigh it on a balance.

Answered: Image /qna-images/answer/784e6dbb-d178-4613-bcc5-0465935582fa.jpg

Answered: What is an isotope? What is meant by…

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...