Q1:Silicon has three naturally-occurring isotopes: 92.23% of 28Si, with an atomic weight of 27.9769 amu, 4.68% of 29Si, with an atomic weight of 28.9765 amu, and 3.09% of 30Si, with an atomic weight of 29.9738 amu. On the basis of these data, confirm that the average atomic weight of Si is 28.0854 amu.

Q1:Silicon has three naturally-occurring isotopes: 92.23% of 28Si, with an atomic weight of 27.9769 amu, 4.68% of 29Si, with an atomic weight of 28.9765 amu, and 3.09% of 30Si, with an atomic weight of 29.9738 amu. On the basis of these data, confirm that the average atomic weight of Si is 28.0854 amu.

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...

See similar textbooks

Similar questions

Potassium has three isotopes with masses 38.9367 amu, 39.9640 amu, and 40.9618 amu. The abundance of the last isotope is 6.73%. Estimate the abundance of the other two isotopes
chlorine has two different isotopes. one isotope has a mass of 35.00 amu and another has a mass of 37.00 Which isotope is the most abundant, Cl-35 or Cl-37. Explain your answer.
Calculate the atomic mass of magnesium. The three magnesium isotopes, Mg-24, Mg-25, and Mg-26, have atomic masses and relative abundance of 23.985 amu (78.99%), 24.986 amu (10.00%), and 25.982 amu (11.01%) respectively
A hypothetical element exists as two isotopes: I = 92.00 amu and II = 98.00 amu. If the atomic mass of this element is found to be 94.10 amu, which isotope must be more abundant?
13) The element antimony has an atomic weight of 121.757 amu and only two naturally-occurring isotopes. One isotope has an abundance of 57.3% and an isotopic mass of 120.904 amu. Based on these data, what is the mass of the other isotope? a) 121.757 u b) 122.393 u c) 122.610 u d) 122.902 u
An element of unknown atomic mass has only two naturally occurring isotopes: 69X (68.935 amu, present in 55.595% abundance) and 71X (70.987 amu) Using the information above, determine the atomic mass of element X
A hypothetical element X is found to have an atomic weight of 37.45 amu. Element X has only two isotopes, X-37 and X-38. The X-37 isotope has a fractional abundance of 0.7721 and an isotopic mass of 37.24. What is the isotopic mass of the other isotope?
There are two naturally occurring isotopes of boron. 10B has a mass of 10.0129 u.11B has a mass of 11.0093 u. Determine the abundance of each isotope.
1) Antimony occurs in nature as a mixture of 2 isotopes. Sb-123 and Sb-121. If the Sb 121 has a mass of 120.9 amu and an abundance of 57.25%, and the average amu is 121.75, what is the abundance of the other isotope?
Tennessine has two naturally occurring isotopes. Tennessine-293 has an atomic mass of 292.9498 and Tennessine-296 has an atomic mass of 295.9246. Given that the average atomic mass of tennessine is 294.0018, what is the percent abundance of Tennessine-293? (Express as a percentage to two decimal places).
Consider the mass of Sulfur and Fluorine in compound A (16.6 g S, 9.80 g F) and compound B (23.2 g S, 55.0 g F). How do numbers like these support atomic theory?
A certain element XX has four isotopes. 5.845% of XX has a mass of 53.93961amuamu. 91.75% of XX has a mass of 55.93494amuamu. 2.123% of XX has a mass of 56.93539amuamu. 0.2820% of XX has a mass of 57.93328amuamu. What is the average atomic mass of element XX?