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Chapter 2: Q26E (page 120)

The 18O: 16O abundance ratio in some meteorites is greater than that used to calculate the average atomic mass of oxygen on earth. Is the average mass of an oxygen atom in these meteorites greater than, less than, or equal to that of a terrestrial oxygen atom?

Short Answer

Expert verified

The average atomic mass of an oxygen atom will be greater than the terrestrial oxygen atom.

Step by step solution

01

– Determine the definition of average atomic mass

The mass of an element of atomic masses is a weighted, average mass of all the isotopes present in a naturally occurring sample of that element. This is equal to the sum of each individual isotope’s mass multiplied by its fractional abundance.

02

– Determine the Formula of Average mass

Average mass =\(\sum\limits_i {{{(fractional\,\,abundance \times isotopic\,mass)}_i}} \)

03

 – Determine how the average atomic mass of an oxygen atom will be greater than the terrestrial oxygen atom

It is because the average atomic mass of an element is directly proportional to the fractional abundance of the isotopes. So, if abundance increases then the average atomic mass also increases.

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Most popular questions from this chapter

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.

Open theBuild an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBld)and click on the

Atom icon.

a. Pick any one of the first 10 elements that you would like to build and state its symbol.

b. Drag protons, neutrons, and electrons onto the atom template to make an atom of your element.

State the numbers of protons, neutrons, and electrons in your atom, as well as the net charge and mass number.

c. Click on “Net Charge” and “Mass Number,” check your answers to (b), and correct, if needed.

d. Predict whether your atom will be stable or unstable. State your reasoning.

e. Check the “Stable/Unstable” box. Was your answer to (d) correct? If not, first predict what you can do to make a Stable atom of your element, and then do it and see if it works. Explain your reasoning.

Explain why the symbol for element sulfur and the formula for a molecule of sulfur differ.

Question: Write the formulas of the following compounds:

(a) rubidium bromide

(b) magnesium selenide

(c) sodium oxide

(d) calcium chloride

(e) hydrogen fluoride

(f) gallium phosphide

(g) aluminum bromide

(h) ammonium sulfate

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the “Mix Isotopes” tab, hide the “Percent Composition” and “Average Atomic Mass” boxes, and then select the element boron.

(a) Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts.

(b) Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice.

(c) Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes fromtheir bins or click on “More” and then move the sliders to the appropriate amounts.

(d) Reveal the “Percent Composition” and “Average Atomic Mass” boxes. How well does your mixture match withyour prediction? If necessary, adjust the isotope amounts to match your prediction.

(e) Select “Nature’s” mix of isotopes and compare it to your prediction. How well does your prediction comparewith the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match “Nature’s”amounts as closely as possible.
See all solutions

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