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Ch.2 - Atoms, Molecules, and Ions
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All textbooksBrown 15th EditionCh.2 - Atoms, Molecules, and IonsProblem 35

Chapter 2, Problem 35

Only two isotopes of copper occur naturally: 63Cu (atomic mass = 62.9296 amu; abundance 69.17%) 65Cu (atomic mass = 64.9278 amu; abundance 30.83%). Calculate the atomic weight (average atomic mass) of copper.

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Hi everyone here we have a question telling us that lead has four stable isotopes listed with their atomic mass and abundance respectively. 204 lead 203.9730 Atomic mass units 1.4 206 lead to 5.9745 Atomic Mass units 24.1% 207 Lead, 206.9759 Atomic Mass units 22.1% and 208 lead 207.9767 Atomic Mass units 52.4%. And our goal is to calculate the atomic mass of blood. So to do that, we take our atomic mass units times are abundance for each isotope and add them together. So we're going to take 1.4 and it's a percent. So divided by Times .9730 Atomic mass units plus 24.1 Divided by Times .9745 Atomic mass units plus 22.1 divided by Times 206.9759 Atomic mass units plus 52.4, Divided by Times 207.9767 Atomic Mass Units. And that equals 2. plus 49. plus 45. Plus 108.9798 And that equals 207. Atomic mass units. And that is our final answer. Thank you for watching Bye.
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Textbook Question

Write the correct symbol, with both superscript and subscript, for each of the following. Use the list of elements in the front inside cover as needed: (d) the isotope of magnesium that has an equal number of protons and neutrons.

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The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of 10.81 amu. Which is the best explanation?

a. The measurement of atomic mass is only reliable to two significant figures.

b. The atomic weight is an average of many individual atoms.

c. The atomic weight is an average of many isotopes of the same nuclear composition.

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(b) Why is the atomic weight of carbon reported as 12.011 in the table of elements and the periodic table in the front inside cover of this text?

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Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass = 84.9118 amu; abundance = 72.15%) and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85%). Calculate the atomic weight of rubidium

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(a) Thomson's cathode-ray tube (Figure 2.4) and the mass spectrometer (Figure 2.11) both involve the use of electric or magnetic fields to deflect charged particles. What are the charged particles involved in each of these experiments?

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Consider the mass spectrometer shown in Figure 2.11. Determine whether each of the following statements is true or false. If false, correct the statement to make it true: (a) The paths of neutral (uncharged) atoms are not affected by the magnet.

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