Help Mass times percentage plus mass times percentagePlus mass times percentage plus mass times percent....1. A scientist collects data on a sample of Lithium. He determines that 92.3% of the sample is lithium-7 and7.7% of the sample is lithium-6. Based on this scientist's information, what is the atomic mass of lithium?

The atomic mass of lithium = 6.938923 amu

Answered: 1. A scientist collects data on a…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter2: Atoms, Molecules, And Ions

Section: Chapter Questions

Problem 2.135QE

See similar textbooks

Similar questions

A fundamental idea of Daltons atomic theory is that atoms of an element can be neither created nor destroyed. We now know that this is not always true. Specifically, it is not true for uranium and lead atoms as they appear in nature. Are the numbers of these atoms increasing or decreasing? Explain.
Calculating Atomic Mass Magnesium has three naturally occurring isotopes with masses 23.99,24.99,and25.98amu and natural abundances 78.99,10.00,and11.01%. Calculate the atomic mass of magnesium.
The natural abundances and isotopic masses of the element neon (Ne) are Calculate the atomic mass of naturally occurring neon.
Why is it important to understand atoms?
Scientists J. J. Thomson and William Thomson (Lord Kelvin) made numerous contributions to our understanding of the atom’s structure. Which subatomic particle did J. J. Thomson discover, and what did this lead him to postulate about the nature of the atom? William Thomson postulated what became known as the “plum pudding” model of the atom’s structure. What did this model suggest?
An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with mass 205.9745 u, 22.10% of an isotope with mass 206.9759 u, and 52.40% of an isotope with mass 207.Y766 u. Calculate the average atomic mass, and identify the element.
Uranium-235 is the isotope of uranium commonly used in nuclear power plants. How many (a) protons are in its nucleus? (b) neutrons are in its nucleus? (c) electrons are in a uranium atom?
The CRC Handbook, a large reference book of chemical and physical data, lists two isotopes of rubidium (Z=37). The atomic mass of 72.15 of rubidium atoms is 84.9118u. Through a typographical oversight, the atomic mass of the second isotope is not printed. Calculate that atomic mass.
Determine whether each statement that follows is true or false. a Dalton proposed that atoms of different elements always combine on a one-to-one basis. b According to Dalton, all oxygen atoms have the same diameter. c The mass of an electron is about the same as the mass of a proton. d There are subatomic particles in addition to the electron, proton, and neutron. e The mass of an atom is uniformly distributed throughout the atom. f Most of the particles fired into the gold foil in the Rutherford experiment were not deflected. g The masses of the proton and electron are equal but opposite in sign. h Isotopes of an element have different electrical charges. i The atomic number of an element is the number of particles in the nucleus of an atom of that element. j An oxygen 16 atom has the same number of protons as an oxygen17 atom. k The nuclei of nitrogen atoms have a different number of protons from the nuclei of any other element. l Neutral atoms of sulfur have a different number of electrons from neutral atoms of any other element. m Isotopes of different elements that exhibit the same mass number exhibit similar chemical behavior. n The mass number of carbon 12 atom is exactly 12g. o Periods are arranged vertically in the periodic table. p The atomic mass of the second element in the farthest right column of the periodic table is 10u. q Nb is the symbol of the element for which Z=41. r Elements in the same column of the periodic table have similar properties. s The element for which Z=38 is in both Group 2A/2 and the fifth period.
Average Atomic Weight Part 1: Consider the four identical spheres below, each with a mass of 2.00 g. Calculate the average mass of a sphere in this sample. Part 2: Now consider a sample that consists of four spheres, each with a different mass: blue mass is 2.00 g, red mass is 1.75 g, green mass is 3.00 g, and yellow mass is 1.25 g. a Calculate the average mass of a sphere in this sample. b How does the average mass for a sphere in this sample compare with the average mass of the sample that consisted just of the blue spheres? How can such different samples have their averages turn out the way they did? Part 3: Consider two jars. One jar contains 100 blue spheres, and the other jar contains 25 each of red, blue, green, and yellow colors mixed together. a If you were to remove 50 blue spheres from the jar containing just the blue spheres, what would be the total mass of spheres left in the jar? (Note that the masses of the spheres are given in Part 2.) b If you were to remove 50 spheres from the jar containing the mixture (assume you get a representative distribution of colors), what would be the total mass of spheres left in the jar? c In the case of the mixture of spheres, does the average mass of the spheres necessarily represent the mass of an individual sphere in the sample? d If you had 80.0 grams of spheres from the blue sample, how many spheres would you have? e If you had 60.0 grams of spheres from the mixed-color sample, how many spheres would you have? What assumption did you make about your sample when performing this calculation? Part 4: Consider a sample that consists of three green spheres and one blue sphere. The green mass is 3.00 g, and the blue mass is 1.00 g. a Calculate the fractional abundance of each sphere in the sample. b Use the fractional abundance to calculate the average mass of the spheres in this sample. c How are the ideas developed in this Concept Exploration related to the atomic weights of the elements?
Mercury An isotope of mercury has 80 protons and 120 neutrons. What is the mass number of this isotope?
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

Chemistry In Focus

Chemistry

ISBN:

9781337399692

Author:

Tro, Nivaldo J.

Publisher:

Cengage Learning,

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

Chemistry In Focus

Chemistry

ISBN:

9781337399692

Author:

Tro, Nivaldo J.

Publisher:

Cengage Learning,

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

1. A scientist collects data on a sample of Lithium. He determines that 92.3% of the sample is lithium-7 and 7.7% of the sample is lithium-6. Based on this scientist's information, what is the atomic mass of lithium?