1.10: Calculating Average Atomic MassThe average atomic mass is the sum of the mass contributions from all natural occurring isotopes. The masscontribution is the product of the isotope mass and its percent abundance (as a decimal point). For an element withthree natural occurring isotopes A, B and C:average weighted atomic mass = mass contribution A + mass contribution B + mass contribution C= (mass A x abundance A) + (mass B x abundance B) + (mass C x abundance C)Show all work, round final answer to 0.001 amu (report to the thousandths place)Isotope Mass(amu)Percent NaturalIsotopeCalculate average weighted atomic massAbundanceNitrogen-14Nitrogen-1514.003199.6315.00010.37Hydrogen-1Hydrogen-21.0078399.9852.014100.015Magnesium-24Magnesium-25Magnesium-2623.98578.9924.98610.0025.98211.01Carbon-1212 (by definition) 98.90Carbon-1313.003361.10Carbon-1414.00324(trace)Oxygen-16Oxygen-17Oxygen-1815.9949299.76216.999130.03817.999160.200

Average atomic mass of any element is calculated by adding the product of mass of isotope multiplied…

Answered: Isotope Mass (amu) Percent Natural…

Isotope Mass (amu) Percent Natural Isotope Calculate average weighted atomic mass Abundance Nitrogen-14 Nitrogen-15 14.0031 99.63 15.0001 0.37 Hydrogen-1 Hydrogen-2 1.00783 99.985 2.01410 0.015

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

Chapter1: Chemical Foundations

Section: Chapter Questions

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

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Atoms and Molecules

An atom is the smallest unit of an element that possesses all the properties of that particular element. Molecules are the smallest unit of a substance that possess all the properties of that particular substance.

Question

1.10: Calculating Average Atomic Mass
The average atomic mass is the sum of the mass contributions from all natural occurring isotopes. The mass
contribution is the product of the isotope mass and its percent abundance (as a decimal point). For an element with
three natural occurring isotopes A, B and C:
average weighted atomic mass = mass contribution A + mass contribution B + mass contribution C
= (mass A x abundance A) + (mass B x abundance B) + (mass C x abundance C)
Show all work, round final answer to 0.001 amu (report to the thousandths place)
Isotope Mass
(amu)
Percent Natural
Isotope
Calculate average weighted atomic mass
Abundance
Nitrogen-14
Nitrogen-15
14.0031
99.63
15.0001
0.37
Hydrogen-1
Hydrogen-2
1.00783
99.985
2.01410
0.015
Magnesium-24
Magnesium-25
Magnesium-26
23.985
78.99
24.986
10.00
25.982
11.01
Carbon-12
12 (by definition) 98.90
Carbon-13
13.00336
1.10
Carbon-14
14.00324
(trace)
Oxygen-16
Oxygen-17
Oxygen-18
15.99492
99.762
16.99913
0.038
17.99916
0.200

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