A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System. Mass-spectroscopic analysis produced the followingdata on the isotopes of ruthenium in these samples:mass relativeisotope (amu) abundance100,Ru 99.90 95.4%99.Ru 98.914.6%Use these measurements to complete the entry for ruthenium in the Periodic Table that would be used on 98765 ALEKS. Round your entry for the atomic massto 3 significant digits.?ArCaution: your correct answer will have the same format but not necessarily the same numbers as the entry for ruthenium in the Periodic Table we use here onEarth.Ru☐

The objective of the question is to calculate the atomic mass of ruthenium on the planetesimal 98765…

Answered: A robot spacecraft returned samples…

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter3: Atoms And Elements

Section: Chapter Questions

Problem 2SC

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Mass spectrometric analysis showed that there are four isotopes of an unknown element having the following masses and abundances: Three elements in the periodic table that have atomic weights near these values are lanthanum (La), atomic number 57, atomic weight 138.9055; cerium (Ce), atomic number 58, atomic weight 140.115; and praseodymium (Pr), atomic number 59, atomic weight 140.9076. Using the data above, calculate the atomic weight, and identify the element if possible.
2-102 An element consists of 90.51% of an isotope with a mass of 19.992 amu, 0.27% of an isotope with a mass of 20.994 amu, and 9.22% of an isotope with a mass of 21.990 amu. Calculate the average atomic mass and identify the element.
Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% 6Li and 92.5% 7Li, which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% 6Li (and the rest 7Li). Calculate the average atomic mass values for each of these two sources.
Calculate the molar mass (atomic weight) of naturally occurring uranium from the masses of the two major isotopes of uranium (235U = 235.0409; 238U = 238.0508) and their natural abundances.
Atomic structure. (a) The synthetic radioactive element technetium is used in many medical studies. Give the number of electrons, protons, and neutrons in an atom of technetium-99. (b) Radioactive americium-241 is used in house-hold smoke detectors and in bone mineral analysis. Give the number of electrons, protons, and neutrons in an atom of americium-241.
2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?
2-101 Complete the following table: Symbol Atomic number Atomic weight Mass number # of protons # of neutrons # of electrons H 0 Li 4 3 Al 26 58 78 17 20
Classify the following as metals, nonmetals, or metalloids: a.argon b.element 3 c.Ge d.boron e.Pm
The following are properties of isotopes of two elements that are essential in our diet. Determine the number of protons, neutrons and electrons in each and name them. atomic number 26, mass number 58, charge of 2+ atomic number 53, mass number 127, charge of 1
1. Which is the more abundant isotope of copper, 63Cu or 65Cu? 63Cu 65Cu
The element gallium, used in gallium arsenide semiconductors, has an atomic weight of 69.72 amu. There are only two isotopes of gallium, Ga with a mass of 6.9257 amu and Ga with a mass of 70.9249 amu. What are the isotopic abundances of gallium? Gallium melts just above room temperature
2-27 If each atom in Problem 2-26 acquired two more neutrons, what element would each then be?

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