
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Boron exist as 2 stable isotopes in nature. Isotopic mass (in amu) and the percent abundance data are given below
X amu 19.9%
11.009305 amu 80.1%

Transcribed Image Text:6. Boron exists as 2 stable isotopes in nature. Isotopic mass (in amu) and percent abundance data are
given below.
x amu 19.9%
11.009305 amu 80.1%
Determine the unkonwn isotopic mass (in amu).
A: 10.01
over o9ggobo angaels bris anooon enong vm
se crceA
7. An element exists as 3 stable isotopes in nature. The isotopic masses (in amu) and percent
abundances are given below.
15.994915 amu 99.757 %
16.999132 amu 0.03800%
17.99916 amu 0.2050 %
Tevsd
Determine what the element is by calculating the average atomic mass (in amu).
A: O; 15.999 amu
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps with 2 images

Knowledge Booster
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
- Silicon has three naturally occurring isotopes with the following masses and natural abundances: Isotope Mass (amu) Abundance (%) Si−28 27.9769 92.2 Si−29 28.9765 4.67 Si−30 29.9737 3.10 Calculate the atomic mass of silicon.arrow_forwardGallium consists of two isotopes, gallium-69 and gallium-71. Gallium-69 has a mass of 68.926 u and a fractional abundance of 0.601. Determine the mass of the gallium-71 isotope.arrow_forwardAn element has three naturally occurring isotopes with the following masses and natural abundances: Isotope 1 2 3 mass (amu) % abundance 24.9858 23.9898 25.9825 10.13 79.13 10.74 Identify the element, give the name of the element.arrow_forward
- 2. Suppose an element consisted of three naturally occurring isotopes. The reported average mass for the element was 75.42 amu. The following information is known: isotope I has a mass of 80.45 and makes up 2.4% of the element's atoms. Isotope II has a mass of 72.22 and makes up 30.0% of the element's atoms. What would you estimate as the mass of isotope III? What instrument is used to determine the mass and natural abundance? Provide a likely sketch of the results from this instrument.arrow_forwardWhat is the average atomic mass of titanium on that planet?arrow_forwardFind the average atomic mass of this isotope of an unknown element. mass 1 220.9038. abundance 100% mass 2 222.9041 abundance 74.8%arrow_forward
- Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.91 amu) is 48.16%. What is the mass, in amu, of the other isotope? 00000 105.87 amu 106.91 amu 106.12 amu 108.47 amu 107.87 amuarrow_forwardAn element has two isotopes, X1⁹ and X²¹. If the mass of element X is 20.2u, determine the percentage abundance of each type of isotope. Textarrow_forwardA hypothetical element has 3 stable isotopes. The masses of the isotopes and percent abundance of the first two isotopes are given. What is the percent abundance of Isotope 3? Isotope 1: 18.556 amu, 11.00% Isotope 2: 18.998 amu, 35.50% Isotope 3: 19.565 amu, ?arrow_forward
- What is the average atomic mass of chlorine if the mass of one isotope is 34.97 amu and has a per cent abundance of 75.77%. The other isotope has a mass of 36.97 amu and has a percent abundance of 24.23%. You should do a calculation and not just look at the periodic chart. 35.45 amu 35.97 amu 34.97 amu 71.95 amuarrow_forwardZinc has five naturally occurring isotopes with an average mass of 65.39 amu. If two isotopes, account for 77% of zinc. Which pair of isotopes will have the highest abundances? 64Zn, 63.9291 amu and 66Zn, 65.9260 amu 66Zn, 65.9260 amu and 67Zn, 66.9271 amu 67Zn, 66.9271 amu and 68Zn, 67.9249 amu 66Zn, 65.9260 amu and 68Zn, 67.9249 amu 67Zn, 66.9271 amu and 70Zn, 69.9253 amuarrow_forward6. Calculate the atomic mass of a cosmic sample of silicon. The three silicon isotopes have atomic masses and relative abundances of 27.9769 amu (80.2297%), 28.9765 amu (12.6832%) and 29.9738 amu (7.0872%).arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY