6. Isotopes. Silicon (Si) is a major component of semiconductor chips. It has three naturallyoccurring isotopes: 285i, 2°Si, and 30Si. Determine the numbers of protons, electrons, and neutrons inan atom of each silicon isotope. TSilver (Ag; Z = 47) has 46 known isotopes, but only 2 occur naturally, 107Ag and 109Ag. Given thefollowing data, calculate the atomic mass of AgIsotopeMass (amu)Abundance (%)107 AgAg106.9050951.84109108.9047648.16

Calculate electron, proton and neutron in each case---

6. Isotopes. Silicon (Si) is a major component of semiconductor chips. It has three naturally occurring isotopes: 285i, 29Si, and 30Si. Determine the numbers of protons, electrons, and neutrons in an atom of each silicon isotope. Silver (Ag; Z = 47) has 46 known isotopes, but only 2 occur naturally, 107Ag and 10Ag. Given the following data, calculate the atomic mass of Ag ): Isotope Mass (amu) Abundance (%) 107 'Ag "Ag 106.90509 51.84 109 108.90476 48.16

6. Isotopes. Silicon (Si) is a major component of semiconductor chips. It has three naturally occurring isotopes: 285i, 29Si, and 30Si. Determine the numbers of protons, electrons, and neutrons in an atom of each silicon isotope. Silver (Ag; Z = 47) has 46 known isotopes, but only 2 occur naturally, 107Ag and 10Ag. Given the following data, calculate the atomic mass of Ag ): Isotope Mass (amu) Abundance (%) 107 'Ag "Ag 106.90509 51.84 109 108.90476 48.16

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter2: Atoms And Molecules

Section: Chapter Questions

Problem 2.74PAE: 2.74 The accompanying table provides the identity of the two naturally occurring isotopes for four...

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Chlorine has two isotopes, Cl-35 and Cl-37. Their abundances are 75.53% and 24.47%, respectively. Assume that the only hydrogen isotope present is H-1. (a) How many different HCI molecules are possible? (b) What is the sum of the mass numbers of the two atoms in each molecule? (c) Sketch the mass spectrum for HCI if all the positive ions are obtained by removing a single electron from an HCI molecule.
Europium has two stable isotopes, 151Eu and 153Eu, with masses of 150.9197 u and 152.9212 u, respectively. Calculate the percent abundances of these isotopes of europium.
Strontium has four stable isotopes. Strontium-84 has a very low natural abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Knowing that the atomic weight of strontium is 87.62, which of the more abundant isotopes predominates?
Indium oxide contains 4.784 g of indium for every 1.000 g of oxygen. In 1869, when Mendeleev first presented his version of the periodic table, he proposed the formula In2O3 for indium oxide. Before that time it was thought that the formula was InO. What values for the atomic mass of indium are obtained using these two formulas? Assume that oxygen has an atomic mass of 16.00.
The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
A cube of sodium has length 1.25 in. How many atoms are in that cube? (Note: dNa=0.968 g/cm3.)
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring 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 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
2.91 Strontium has four stable isotopes. Strontium—84 has a very low natural abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Knowing that the atomic weight of strontium is 87.62, which of the more abundant isotopes predominates?
An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with mass 205.9745 u, 22.10% of an isotope with mass 206.9759 u, and 52.40% of an isotope with mass 207.Y766 u. Calculate the average atomic mass, and identify the element.
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. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible. 21. Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.
2.74 The accompanying table provides the identity of the two naturally occurring isotopes for four elements and the atomic weights for those elements. (In each case, the two isotopes differ in mass number by two.) Which element has the mass spectrum shown? Explain your answer.