(a) Atoms are very small compared to objects on the macroscopic scale. The radius of a gold atom is 144 pm. What is this value in meters and in centimeters? 1.44e-10 m 1.446-8 cm (b) The mass of a single gold atom is 3.27x10-22 g. Suppose enough Au atoms were lined up like beads on a string to span a distance of 30.5 cm (12 inches). How many atoms would be required? What mass in grams of Au would be used? Could you weigh out this amount of gold using a typical laboratory balance? (e) Taking the density of gold metal to be 19.3 g/cm³, calculate the mass of metal needed to form a piece of Au wire with the same length as the distance in b, but with a diameter of 1.00 mm. Hint: The volume of a cylinder is n times its radius squared times its height. (V-nr² h) 9 How many gold atoms does this represent? 9 atoms atoms

(a) Atoms are very small compared to objects on the macroscopic scale. The radius of a gold atom is 144 pm. What is this value in meters and in centimeters? 1.44e-10 m 1.446-8 cm (b) The mass of a single gold atom is 3.27x10-22 g. Suppose enough Au atoms were lined up like beads on a string to span a distance of 30.5 cm (12 inches). How many atoms would be required? What mass in grams of Au would be used? Could you weigh out this amount of gold using a typical laboratory balance? (e) Taking the density of gold metal to be 19.3 g/cm³, calculate the mass of metal needed to form a piece of Au wire with the same length as the distance in b, but with a diameter of 1.00 mm. Hint: The volume of a cylinder is n times its radius squared times its height. (V-nr² h) 9 How many gold atoms does this represent? 9 atoms atoms

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A fictitious element only has two naturally occurring isotopes: X and Y. If isotope X has a mass of 132.5 amu and a percent abundance of 44.4%, what is the mass in grams of 6.09×1023 atoms of isotope Y given that the average mass of the element is 136.2 amu?
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a)For carbon-12 and carbon-14, how many protons and neutrons are in each nucleus? Carbon-12 has protons. Carbon-12 has neutrons. Carbon-14 has protons. Carbon-14 has neutrons. (1b )Assuming neutral atoms, how many electrons are present in an atom of carbon-12 and in an atom of carbon-14? Carbon-12 has electrons. Carbon-14 has electrons.
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