Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Remember that is the symbol for sum. In other words, we will take the sum of the relative abundance of each isotope multiplied by its mass. Example Neon has three naturally occurring isotopes. Symbol Ne-20 Ne-21 Ne-22 Mass Isotopic mass (amu) number 20 21 22 19.9924 20.9938 21.9914 Percent natural abundance 90.48% 0.27% 9.25% ***

Remember that is the symbol for sum. In other words, we will take the sum of the relative abundance of each isotope multiplied by its mass. Example Neon has three naturally occurring isotopes. Symbol Ne-20 Ne-21 Ne-22 Mass Isotopic mass (amu) number 20 21 22 19.9924 20.9938 21.9914 Percent natural abundance 90.48% 0.27% 9.25% ***

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter2: Chemical Compounds
Section: Chapter Questions
Problem 129QRT
See similar textbooks
icon
Related questions
Question
Explain the difference between an average and a weighted average
Since the abundances are not equal, we cannot do a typical simple average where we just add them up and divide by two. Instead, we need to perform a weighted average. The formula to calculate the average 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 abundance of each isotope multiplied by its mass. Example Neon has three naturally occurring isotopes. Symbol Ne-20 Ne-21 Ne-22 Mass Isotopic mass Percent natural number (amu) abundance 20 21 22 19.9924 20.9938 21.9914 90.48% 0.27% 9.25% ….. Remember that mass number is not the same as the atomic mass or isotopic mass! The mass number is the number of protons + neutrons, while atomic mass (or isotopic mass) is the mass if you were to somehow weigh it on a balance.
Transcribed Image Text:Since the abundances are not equal, we cannot do a typical simple average where we just add them up and divide by two. Instead, we need to perform a weighted average. The formula to calculate the average 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 abundance of each isotope multiplied by its mass. Example Neon has three naturally occurring isotopes. Symbol Ne-20 Ne-21 Ne-22 Mass Isotopic mass Percent natural number (amu) abundance 20 21 22 19.9924 20.9938 21.9914 90.48% 0.27% 9.25% ….. Remember that mass number is not the same as the atomic mass or isotopic mass! The mass number is the number of protons + neutrons, while atomic mass (or isotopic mass) is the mass if you were to somehow weigh it on a balance.
Since the abundances are not equal, we cannot do a typical simple average where we just add them up and divide by two. Instead, we need to perform a weighted average. The formula to calculate the average atomic mass is: +
Transcribed Image Text:Since the abundances are not equal, we cannot do a typical simple average where we just add them up and divide by two. Instead, we need to perform a weighted average. The formula to calculate the average atomic mass is: +
Expert Solution
steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Atomic Structure and Spectra
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
Chemistry
ISBN:
9781133109655
Author:
Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:
Brooks / Cole / Cengage Learning
SEE MORE TEXTBOOKS