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Chapter 2: Q58E (page 127)
Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:
a. NiCO3
b. MoO3
c.Co(NO3)2
d. V2O5
e. MnO2
f. Fe2O3
a. Nickel Carbonate
b. Molybdenum trioxide
c. Cobalt nitrate
d. Vanadium (V) oxide
e. Manganese (IV) oxide
f. Iron (III) oxide
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Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes:\(\begin{aligned}{}\left( a \right){\rm{ }}{}_3^7Li{\rm{ }}\\\left( b \right){\rm{ }}{}_{52}^{125}Te{\rm{ }}\\\left( c \right){\rm{ }}{}_{47}^{109}Ag{\rm{ }}\\\left( d \right){\rm{ }}{}_7^{15}N{\rm{ }}\\\left( e \right){\rm{ }}{}_{15}^{31}P\end{aligned}\)
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.
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.
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring, the 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 10.819, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundance leading to the two values of the average atomic masses of boron from these two countries.
Explain why the symbol for an atom of the element oxygen and the formula for a molecule of oxygen differ.
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