16 53 25 S Mn Iodine 32.06 126.905 54.938 Atomic # = Atomic # = Atomic # = Atomic Mass = Atomic Mass = Atomic Mass% = # of Protons = # of Protons = # of Protons = # of Neutrons = # of Neutrons% = # of Neutrons% = # of Electrons = # of Electrons = # of Electrons 3D 12 18 19 Mg K Argon 24.305 39.948 39.098 Atomic #= Atomic #= Atomic #= Atomic Mass = Atomic Mass% = Atomic Mass = # of Protons%3D # of Protons = # of Protons = # of Neutrons%3D # of Neutrons = # of Neutrons%3D # of Electrons = # of Electrons = # of Electrons%3D 79 1 9. H. Gold Fluorine 196.967 1.008 18.998 Atomic # = Atomic #= Atomic # = Atomic Mass = Atomic Mass = Atomic Mass = # of Protons = # of Protons%3D # of Protons = # of Neutrons%3= # of Neutrons D # of Neutrons # of Electrons%3D # of Electrons = # of Electrons =

16 53 25 S Mn Iodine 32.06 126.905 54.938 Atomic # = Atomic # = Atomic # = Atomic Mass = Atomic Mass = Atomic Mass% = # of Protons = # of Protons = # of Protons = # of Neutrons = # of Neutrons% = # of Neutrons% = # of Electrons = # of Electrons = # of Electrons 3D 12 18 19 Mg K Argon 24.305 39.948 39.098 Atomic #= Atomic #= Atomic #= Atomic Mass = Atomic Mass% = Atomic Mass = # of Protons%3D # of Protons = # of Protons = # of Neutrons%3D # of Neutrons = # of Neutrons%3D # of Electrons = # of Electrons = # of Electrons%3D 79 1 9. H. Gold Fluorine 196.967 1.008 18.998 Atomic # = Atomic #= Atomic # = Atomic Mass = Atomic Mass = Atomic Mass = # of Protons = # of Protons%3D # of Protons = # of Neutrons%3= # of Neutrons D # of Neutrons # of Electrons%3D # of Electrons = # of Electrons =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section: Chapter Questions

Problem 11QRT: Match these by placing the correct notation in the appropriate blank. 3467Se3367As3567Br3672Kr a....

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Average atomic masses listed by JUPAC are based on a study of experimental results. Bromine has two isotopes 79Br and 81Br, whose masses (78.9 183 and 80.9 163 amu) and abundances (50.69% and 49.3 1%) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.
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?
Match these by placing the correct notation in the appropriate blank. 3467Se3367As3567Br3672Kr a. Contains 33 neutrons b. Contains greatest number of neutrons c. Contains equal number of protons and neutrons d. Contains the same number of neutrons as there are protons in As-67
Radon is a radioactive gas that can cause lung cancer. It has been detected in the basement of some homes. In an atom of Rn-220, (a) how many protons are there? (b) how many neutrons are there?
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.
An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.
Naturally occurring silver (Ag) consists of two isotopes. One of the isotopes has a mass of 106.90509 amu and 51.84% abundance. What is the atomic mass of the other isotope?
In what way are isotopes of a given element always different? In what way(s) are they always the same?
Define the term atomic weight. Why might the values of atomic weights on a planet elsewhere in the universe be different from those on earth?
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